http://www.physicsbook.gatech.edu/api.php?action=feedcontributions&feedformat=atom&user=Ssivakumar36Physics Book - User contributions [en]2026-05-05T16:18:30ZUser contributionsMediaWiki 1.42.7http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27662Sign of a Potential Difference2017-04-08T18:56:12Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
[[File:Rsz_2212eq1.png|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors, as shown below. <br />
<br />
[[File:Rsz 2212eq2.png|center]]<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
== Sign of Potential Difference ==<br />
<br />
[[File:Rsz_2212eq3.png|center]]<br />
<br />
<br />
For the last scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''. To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
<br />
== Examples ==<br />
Remember:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''<br />
<br />
[[File:Old_examples.jpg|center]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
[[File:Rsz_2212eq4.png|center]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Rsz_2212eq4.png&diff=27661File:Rsz 2212eq4.png2017-04-08T18:54:28Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27405Sign of a Potential Difference2017-04-05T04:59:33Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
[[File:Rsz_2212eq1.png|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors, as shown below. <br />
<br />
[[File:Rsz 2212eq2.png|center]]<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
== Sign of Potential Difference ==<br />
<br />
[[File:Rsz_2212eq3.png|center]]<br />
<br />
<br />
For the last scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''. To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg|center]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27404Sign of a Potential Difference2017-04-05T04:55:27Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
[[File:Rsz_2212eq1.png|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors, as shown below. <br />
<br />
[[File:Rsz 2212eq2.png|center]]<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
== Sign of Potential Difference ==<br />
<br />
[[File:Rsz_2212eq3.png|center]]<br />
<br />
<br />
For the last scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''. To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27403Sign of a Potential Difference2017-04-05T04:22:43Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
[[File:Rsz_2212eq1.png|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors. <br />
<br />
[[File:Rsz 2212eq2.png|center]]<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
[[File:Rsz_2212eq3.png|center]]<br />
<br />
(1) Same Direction<br />
In this scenario, the dot product yields a positive result, so when multiplied by the negative term in the equation, the resulting potential difference will be '''negative'''.<br />
<br />
(2) Opposite Direction<br />
When the electric field and displacement are in opposite directions, the result of the dot product will be negative which leads to a '''positive potential difference''' after multiplying that result by -1. <br />
<br />
(3) Directions are Perpendicular<br />
For this scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''.<br />
To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
Moving forward with the concept of potential difference, this concept will be useful to remember for solving problems.<br />
<br />
== Indicating Path Direction (sign convention) ==<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. <br />
For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Rsz_2212eq3.png&diff=27402File:Rsz 2212eq3.png2017-04-05T04:21:57Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27401Sign of a Potential Difference2017-04-05T04:20:38Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
[[File:Rsz_2212eq1.png|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors. <br />
<br />
[[File:Rsz 2212eq2.png|center]]<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
[[File:2212eq3.jpg|2212eq3.jpg]]<br />
<br />
(1) Same Direction<br />
In this scenario, the dot product yields a positive result, so when multiplied by the negative term in the equation, the resulting potential difference will be '''negative'''.<br />
<br />
(2) Opposite Direction<br />
When the electric field and displacement are in opposite directions, the result of the dot product will be negative which leads to a '''positive potential difference''' after multiplying that result by -1. <br />
<br />
(3) Directions are Perpendicular<br />
For this scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''.<br />
To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
Moving forward with the concept of potential difference, this concept will be useful to remember for solving problems.<br />
<br />
== Indicating Path Direction (sign convention) ==<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. <br />
For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Rsz_2212eq2.png&diff=27400File:Rsz 2212eq2.png2017-04-05T04:19:30Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27399Sign of a Potential Difference2017-04-05T04:18:26Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
[[File:Rsz_2212eq1.png|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors. <br />
<br />
<br />
[[File:PotentialDiff_efield_eq.jpg|center]]<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
[[File:2212eq3.jpg|2212eq3.jpg]]<br />
<br />
(1) Same Direction<br />
In this scenario, the dot product yields a positive result, so when multiplied by the negative term in the equation, the resulting potential difference will be '''negative'''.<br />
<br />
(2) Opposite Direction<br />
When the electric field and displacement are in opposite directions, the result of the dot product will be negative which leads to a '''positive potential difference''' after multiplying that result by -1. <br />
<br />
(3) Directions are Perpendicular<br />
For this scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''.<br />
To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
Moving forward with the concept of potential difference, this concept will be useful to remember for solving problems.<br />
<br />
== Indicating Path Direction (sign convention) ==<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. <br />
For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Rsz_2212eq1.png&diff=27398File:Rsz 2212eq1.png2017-04-05T04:17:44Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:2212eq1.png&diff=27337File:2212eq1.png2017-04-04T06:15:09Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Pleasework.png&diff=27336File:Pleasework.png2017-04-04T06:14:15Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27335Sign of a Potential Difference2017-04-04T05:58:46Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
<br />
[[File:PotEnergy&Diff_eq.jpg|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors. <br />
<br />
<br />
[[File:PotentialDiff_efield_eq.jpg|center]]<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
[[File:2212eq3.jpg|2212eq3.jpg]]<br />
<br />
(1) Same Direction<br />
In this scenario, the dot product yields a positive result, so when multiplied by the negative term in the equation, the resulting potential difference will be '''negative'''.<br />
<br />
(2) Opposite Direction<br />
When the electric field and displacement are in opposite directions, the result of the dot product will be negative which leads to a '''positive potential difference''' after multiplying that result by -1. <br />
<br />
(3) Directions are Perpendicular<br />
For this scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''.<br />
To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
Moving forward with the concept of potential difference, this concept will be useful to remember for solving problems.<br />
<br />
== Indicating Path Direction (sign convention) ==<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. <br />
For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:2212eq3.jpg&diff=27334File:2212eq3.jpg2017-04-04T05:53:30Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27333Sign of a Potential Difference2017-04-04T05:41:43Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
<br />
[[File:PotEnergy&Diff_eq.jpg|center]]<br />
<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors. <br />
<br />
[[File:PotentialDiff_efield_eq.jpg|center]]<br />
<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
(1) Same Direction<br />
In this scenario, the dot product yields a positive result, so when multiplied by the negative term in the equation, the resulting potential difference will be '''negative'''.<br />
<br />
(2) Opposite Direction<br />
When the electric field and displacement are in opposite directions, the result of the dot product will be negative which leads to a '''positive potential difference''' after multiplying that result by -1. <br />
<br />
(3) Directions are Perpendicular<br />
For this scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''.<br />
To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
Moving forward with the concept of potential difference, this concept will be useful to remember for solving problems.<br />
<br />
== Indicating Path Direction (sign convention) ==<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. <br />
For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg]]<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Integralexa.jpg&diff=27332File:Integralexa.jpg2017-04-04T05:33:57Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Firstpic.png&diff=27331File:Firstpic.png2017-04-04T05:20:56Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Thefirst.jpg&diff=27330File:Thefirst.jpg2017-04-04T05:18:45Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27329Sign of a Potential Difference2017-04-04T05:15:46Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
[[File:PotEnergy&Diff_eq.jpg]]<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors. <br />
[[File:PotentialDiff_efield_eq.jpg]]<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
(1) Same Direction<br />
In this scenario, the dot product yields a positive result, so when multiplied by the negative term in the equation, the resulting potential difference will be '''negative'''.<br />
<br />
(2) Opposite Direction<br />
When the electric field and displacement are in opposite directions, the result of the dot product will be negative which leads to a '''positive potential difference''' after multiplying that result by -1. <br />
<br />
(3) Directions are Perpendicular<br />
For this scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''.<br />
To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
Moving forward with the concept of potential difference, this concept will be useful to remember for solving problems.<br />
<br />
== Indicating Path Direction (sign convention) ==<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. <br />
For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
<br />
== Examples ==<br />
[[File:Old_examples.jpg]]<br />
**because of site formatting this image is unable to be viewed in its original format<br />
*To view the image in the upright orientation follow this link: https://drive.google.com/open?id=0BxZ16KwNznRoaXV4a25TMmJVUEU<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Old_examples.jpg&diff=27328File:Old examples.jpg2017-04-04T05:14:35Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Sign_of_a_Potential_Difference&diff=27288Sign of a Potential Difference2017-04-02T22:21:59Z<p>Ssivakumar36: </p>
<hr />
<div>CLAIMED BY SHREENU SIVAKUMAR (SPRING 2017)<br />
<br />
<br />
----<br />
This article covers the sign of potential difference, and how to determine the sign in different situations involving a particle and an electric field.<br />
<br />
== Introduction ==<br />
<br />
Recall from previous sections that the change in '''potential energy''' is equal to the charge times the change in '''potential difference'''. From Conservation of Energy, we know that an ''increase'' in potential energy is related to a ''decrease'' in kinetic energy, and vice versa. Furthermore, recall that the change in potential energy, potential difference, kinetic energy, etc. can be positive ''or'' negative.<br />
[[File:PotEnergy&Diff_eq.jpg]]<br />
In this article we will see how the change in potential energy can be positive, negative, or zero and then we will be able to look back and see how the sign of this change relates to the potential energy, kinetic energy, and so on. <br />
<br />
== Direction of Path vs. Direction of Electric Field ==<br />
<br />
From the equation relating potential difference with electric field and motion, we can see that the sign of the potential difference is dependent on the direction of both the electric field and displacement vectors. <br />
[[File:PotentialDiff_efield_eq.jpg]]<br />
For this equation, note that the result of the cross product between the electric field and displacement is negated before finding the potential difference. Furthermore, it is important to note that the electric field and displacement vectors are multiplied by the dot product. Because of this dot product, we will analyze 3 different scenarios: path in the direction of the electric field, path in the ''opposite'' direction of the electric field, and the path moving ''perpendicular'' to the direction of the electric field.<br />
<br />
(1) Same Direction<br />
In this scenario, the dot product yields a positive result, so when multiplied by the negative term in the equation, the resulting potential difference will be '''negative'''.<br />
<br />
(2) Opposite Direction<br />
When the electric field and displacement are in opposite directions, the result of the dot product will be negative which leads to a '''positive potential difference''' after multiplying that result by -1. <br />
<br />
(3) Directions are Perpendicular<br />
For this scenario it will be critical to have a strong understanding of the dot product and how to calculate it. Remember that a dot product multiplies terms that are in the same direction before being summed for a total. This means that when finding the dot product of two perpendicular vectors, the result will be '''zero'''.<br />
To better understand this, imagine the electric field between two very long capacitor plates. The electric field points from one plate to the other, let's say in the +x direction. If you wanted to move a charge at any location between the plates in either the +y or -y direction, your displacement vector would point in one of these directions. Whether you moved the particle +y or -y direction, the dot product of the electric field and displacement will be zero. <br />
Moving forward with the concept of potential difference, this concept will be useful to remember for solving problems.<br />
<br />
== Indicating Path Direction (sign convention) ==<br />
<br />
Consistent with previous convention, the delta symbol indicates "final - initial." We will use this same notation in showing the direction of the path. <br />
For example: Vb - Va ---> signifies the potential difference between location B (final) and location A (initial).<br />
<br />
<br />
== Examples ==<br />
[[File:Examples.jpg]]<br />
**because of site formatting this image is unable to be viewed in its original format<br />
*To view the image in the upright orientation follow this link: https://drive.google.com/open?id=0BxZ16KwNznRoaXV4a25TMmJVUEU<br />
<br />
== Summary ==<br />
When determining the sign of the potential difference, there will be 3 different scenarios that will determine whether the sign of the potential difference is positive, negative, or zero. Pay close attention to notation when considering the change in a quantity (potential, displacement, etc..) in order to avoid confusing the wrong sign. Attention to detail when find the sign of potential difference will make solving the more difficult problems at the end of the chapter a little easier. The following summary of the 3 scenarios is extremely helpful:<br />
<br />
Path going in direction of ''E'' ------> Potential is '''decreasing'''<br />
<br />
Path going opposite to ''E'' -------> Potential is '''increasing'''<br />
<br />
Path perpendicular to ''E'' --------> Potential '''does not change'''</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=25220Boiling Point2016-11-27T22:31:41Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
<br />
==References==<br />
<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24161Boiling Point2016-11-25T23:58:22Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24160Boiling Point2016-11-25T23:58:01Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
<br />
[['''Clausius-Clapeyron Equation''']]<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
[['''Boiling Point Elevation Equation''']]<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24159Boiling Point2016-11-25T23:57:31Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24158Boiling Point2016-11-25T23:57:16Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24156Boiling Point2016-11-25T23:56:47Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24155Boiling Point2016-11-25T23:56:21Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24152Boiling Point2016-11-25T23:55:13Z<p>Ssivakumar36: </p>
<hr />
<div>'''Claimed for editing: Shreenu Sivakumar'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24151Boiling Point2016-11-25T23:50:40Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes. It is a very important property that often helps to solve many problems about a system, especially in chemical engineering. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24149Boiling Point2016-11-25T23:48:30Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>''' <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24147Boiling Point2016-11-25T23:47:53Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants below: <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
i = <br />
<br />
b<sub>solute</sub> = <br />
<br />
From here the equation can be used: <br />
<br />
ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub> = <br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24145Boiling Point2016-11-25T23:46:20Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution, b<sub>B</sub> = b<sub>solute</sub> · i<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants. <br />
<br />
K<sub>b</sub> = <br />
<br />
b<sub>B</sub> = <br />
<br />
ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>=<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24142Boiling Point2016-11-25T23:43:02Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = Molality of the solution<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would first include initializing the constants. <br />
<br />
K = ???<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24140Boiling Point2016-11-25T23:40:19Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = [[Ebullioscopic constant]]<br />
<br />
'''b<sub>B</sub>''' = <br />
<br />
T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24139Boiling Point2016-11-25T23:37:50Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub>'''<br />
<br />
<br />
The constants in the equation can be defined as:<br />
<br />
'''ΔT<sub>b</sub>''' = boiling point elevation, which is equal to T<sub>b, solution</sub> - T<sub>b, solvent </sub><br />
<br />
'''K<sub>b</sub>''' = <br />
<br />
'''b<sub>B</sub>''' = <br />
<br />
T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24129Boiling Point2016-11-25T23:22:02Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
<br />
[[File:ClausiusClapeyron.png]]<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
This equation accounts for a solution's boiling point being higher than just the solvent's boiling point. This equation should be used when The equation is:<br />
<br />
'''ΔT<sub>b</sub> = K<sub>b</sub>· b<sub>B</sub><br />
'''<br />
The constants in the equation can be defined as:<br />
<br />
ΔT<sub>b</sub><br />
<br />
T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:ClausiusClapeyron.png&diff=24120File:ClausiusClapeyron.png2016-11-25T23:01:57Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=File:Neuron12345.jpg&diff=24118File:Neuron12345.jpg2016-11-25T23:01:02Z<p>Ssivakumar36: </p>
<hr />
<div></div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24114Boiling Point2016-11-25T22:52:30Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24083Boiling Point2016-11-25T21:50:54Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J * <math> mol^{-1} </math> * <math> K^{-1} </math><br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24078Boiling Point2016-11-25T21:47:40Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J/(mol*K) <br />
<br />
'''P''' = vapor pressure at the specific pressure given<br />
<br />
'''P<sub>0</sub>''' = pressure that corresponds to the T<sub>0</sub> used<br />
<br />
'''ΔH<sub>vap</sub>''' = heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24077Boiling Point2016-11-25T21:45:28Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
<br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
'''R''' = ideal gas constant, 8.3144598 J/(mol*K) <br />
<br />
'''P''' = <br />
<br />
'''P<sub>0</sub>''' = <br />
<br />
H<sub>vap</sub>= heat of vaporization of the liquid<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24076Boiling Point2016-11-25T21:35:50Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
This equation should be used when the vapor pressure and heat of vaporization for the liquid are known for a specific temperature and you are trying to calculate the boiling point. <br />
<br />
''The constants in the equation can be defined as:''<br />
<br />
'''T<sub>B</sub>''' = boiling point at the specific temperature<br />
<br />
'''T<sub>0</sub>''' = temperature at which the liquid boils<br />
<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[https://en.wikipedia.org/wiki/Boiling_point]<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24075Boiling Point2016-11-25T21:25:15Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=24074Boiling Point2016-11-25T21:24:51Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
Boiling point is a key property of matter in which the vapor pressure of a liquid equals the pressure around the liquid and the liquid turns into a vapor. The boiling point of a substance is highly dependent on the environment around the substance. For example, at a high pressure a liquid has a higher boiling point than it would have at atmospheric pressure. Similarly, at low pressure a liquid has a lower boiling point. Another environmental factor that affects the boiling point of a liquid is whether the liquid is in a partial vacuum. In this state, the boiling point of a liquid will be lower than the boiling point of the same liquid at atmospheric pressure. In addition, different liquids boil at different temperatures for a set pressure. <br />
<br />
===A Mathematical Model===<br />
There are several equations that relate to boiling point, including the Clausius–Clapeyron equation and the boiling point elevation equation. <br />
<br />
'''Clausius-Clapeyron Equation'''<br />
<br />
{\displaystyle T_{\text{B}}={\Bigg (}{\frac {1}{T_{0}}}-{\frac {R\,\ln {\frac {P}{P_{0}}}}{\Delta H_{\text{vap}}}}{\Bigg )}^{-1},}<br />
<br />
T_{B} is the boiling point at the pressure of interest,<br />
{\displaystyle R} R is the ideal gas constant,<br />
{\displaystyle P} P is the vapour pressure of the liquid at the pressure of interest,<br />
{\displaystyle P_{0}} P_{0} is some pressure where the corresponding {\displaystyle T_{0}} T_{0} is known (usually data available at 1 atm or 100 kPa),<br />
{\displaystyle \Delta H_{\text{vap}}} {\displaystyle \Delta H_{\text{vap}}} is the heat of vaporization of the liquid,<br />
{\displaystyle T_{0}} T_{0} is the boiling temperature,<br />
{\displaystyle \ln } \ln is the natural logarithm.<br />
<br />
<br />
'''Boiling Point Elevation Equation'''<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36http://www.physicsbook.gatech.edu/index.php?title=Boiling_Point&diff=23819Boiling Point2016-11-23T23:50:03Z<p>Ssivakumar36: </p>
<hr />
<div>'''CLAIMED FOR EDITING BY SHREENU SIVAKUMAR'''<br />
<br />
==The Main Idea==<br />
<br />
The main idea of this page is a description of the property of matter that is it's boiling point. In short, the boiling point is the temperature at which the vapor pressure of a liquid is equal to the pressure on the liquid.<br />
<br />
===A Mathematical Model===<br />
<br />
The main mathematical model for this property is the boiling point elevation equation. This equation takes into account the effect that adding a solute to a solvent has on it's boiling point. For example &#916;T = i K<sub>b</sub>m, where &#916;T is the temperature difference that arises from adding the solute, i is the van 't Hoff factor which is equivalent to the number of substances a molecule ionizes into (i.e NaCl is 2, sugar is 1, MgCl<sub>2</sub> is 3), K<sub>b</sub> is a thermodynamic constant relating to the solvent, and m is the molality.<br />
<br />
===A Computational Model===<br />
<br />
Creating a computational model for this equation would be pretty easy, you would first have to initialize the constants, which would be i, K<sub>b</sub>, and either m or the information that goes into calculating molality. <br />
<br />
K = ???<br />
<br />
<br />
m = moles of solute/mass of solvent<br />
<br />
<br />
i = ???<br />
<br />
<br />
&#916;T = i*K*m<br />
<br />
==Examples==<br />
<br />
An example of an easy, middling and difficult problem are included in the link below. An easy example would be problems 3-5, a middling example would be problems 6, 8, 9, and 10. A difficult example would be the bonus problems.<br />
<br />
[http://www.chemteam.info/Solutions/BP-elevation-probs1-to-10.html Boiling Point Elevation]<br />
<br />
==Connectedness==<br />
Boiling point in itself is very important in many every day processes and especially in my major (chemical engineering). It is a very important property that often helps to solve many problems about a system. <br />
One universal use for boiling point elevation is in cooking. Adding a solute such as salt to water that you are trying to boil will cause it to be hotter than it would be otherwise when the boiling point has not been elevated. <br />
A large amount of solute would be necessary to acquire an appreciable increase, however there is a very small increase no matter how much you use. Boiling point elevation is also used in sugar refining; at some points during the process the syrup is boiled and the temperature at which it boils depends on the concentration of sugar at that time.<br />
<br />
==History==<br />
<br />
In 1741, Anders Celsius defined his temperature scale on the melting and boiling temperature of water. <br />
Although Celsius did not discover the thermometer – both Philo and Hero of Alexandria (who also mentioned steam power in 50 BC) described such a principle – his design was much more precise than any previous such invention. <br />
Celsius scaled his measurements as 0 for boiling point and 100 for freezing point but the order was later reversed.<br />
<br />
== See also ==<br />
<br />
For information on melting point, a very similar property, see [[Melting Point]]<br />
<br />
===Further reading===<br />
<br />
An article from Purdue:<br />
<br />
[https://www.chem.purdue.edu/gchelp/liquids/boil.html Boiling]<br />
<br />
An article out of the Britannica Online Encyclopedia:<br />
<br />
[http://www.britannica.com/science/boiling-point Boiling Point]<br />
<br />
===External links===<br />
<br />
See Below<br />
<br />
==References==<br />
<br />
[http://www.ehow.com/info_8344665_uses-boiling-point-elevation.html Uses of Boiling Point Elevation]<br />
[http://www.chemteam.info/Solutions/BP-elevation.html Boiling Point Elevation]<br />
[https://www.chem.tamu.edu/class/majors/tutorialnotefiles/intext.htm Chemistry Basics]<br />
[http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/melting.php Melting Point, Freezing Point, Boiling Point]<br />
[http://didyouknow.org/celsius/ Boiling Point of Water]<br />
[[Category:Properties of Matter]]</div>Ssivakumar36