10. Imagine you have a system in which you have 54 grams of ice. You can melt this ice and then vaporize it all at 0 C. The melting and vaporization are done reversibly into a balloon held at a pressure of 0.250 bar. Here are some facts about water you may wish to know. The density of liquid water at 0 C is 1 g/cm³. The density of ice at 0 C is 0.917 g/cm³. The enthalpy of vaporization of liquid water is 2.496 kJ/gram and the enthalpy of fusion of solid water is 333.55 J/gram. H. Are the solid and the liquid in equilibrium at the melting point? How do you know? I. How much energy does the water absorb as heat when it vaporizes? J How much work is involved in vaporizing the ice? K. What is total change in energy for vaporizing the water? L. What is the entropy change for vaporizing the water? M. What is the change in Helmholtz energy for vaporizing the water? N. What is the change in Gibbs energy for vaporizing the water? O. One of the things the Helmholtz energy is good for is telling you the maximum amount of work that can be gained from a thermodynamic process since AA = AU - TAS, where TAS tells you about heat, and the change in energy minus the heat gives you the work. Does it work in this case? P. If instead of melting the ice and vaporizing the liquid, you instead sublimed the ice directly to the vapor phase, what would be the change in AU, AH, AA, and AG? What makes this calculation straightforward?
10. Imagine you have a system in which you have 54 grams of ice. You can melt this ice and then vaporize it all at 0 C. The melting and vaporization are done reversibly into a balloon held at a pressure of 0.250 bar. Here are some facts about water you may wish to know. The density of liquid water at 0 C is 1 g/cm³. The density of ice at 0 C is 0.917 g/cm³. The enthalpy of vaporization of liquid water is 2.496 kJ/gram and the enthalpy of fusion of solid water is 333.55 J/gram. H. Are the solid and the liquid in equilibrium at the melting point? How do you know? I. How much energy does the water absorb as heat when it vaporizes? J How much work is involved in vaporizing the ice? K. What is total change in energy for vaporizing the water? L. What is the entropy change for vaporizing the water? M. What is the change in Helmholtz energy for vaporizing the water? N. What is the change in Gibbs energy for vaporizing the water? O. One of the things the Helmholtz energy is good for is telling you the maximum amount of work that can be gained from a thermodynamic process since AA = AU - TAS, where TAS tells you about heat, and the change in energy minus the heat gives you the work. Does it work in this case? P. If instead of melting the ice and vaporizing the liquid, you instead sublimed the ice directly to the vapor phase, what would be the change in AU, AH, AA, and AG? What makes this calculation straightforward?
College Physics
10th Edition
ISBN:9781285737027
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
Chapter10: Thermal Physics
Section: Chapter Questions
Problem 64AP: Two small containers, each with a volume of 1.00 102cm3, contain helium gas at 0C and 1.00 atm...
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Transcribed Image Text:10. Imagine you have a system in which you have 54 grams of ice. You can melt this
ice and then vaporize it all at 0 C. The melting and vaporization are done reversibly
into a balloon held at a pressure of 0.250 bar. Here are some facts about water you
may wish to know. The density of liquid water at 0 C is 1 g/cm³. The density of ice at 0
C is 0.917 g/cm³. The enthalpy of vaporization of liquid water is 2.496 kJ/gram and the
enthalpy of fusion of solid water is 333.55 J/gram.
Transcribed Image Text:H. Are the solid and the liquid in equilibrium at the melting point? How do you know?
I. How much energy does the water absorb as heat when it vaporizes?
J How much work is involved in vaporizing the ice?
K. What is total change in energy for vaporizing the water?
L. What is the entropy change for vaporizing the water?
M. What is the change in Helmholtz energy for vaporizing the water?
N. What is the change in Gibbs energy for vaporizing the water?
O. One of the things the Helmholtz energy is good for is telling you the maximum
amount of work that can be gained from a thermodynamic process since AA = AU -
TAS, where TAS tells you about heat, and the change in energy minus the heat gives
you the work. Does it work in this case?
P. If instead of melting the ice and vaporizing the liquid, you instead sublimed the ice
directly to the vapor phase, what would be the change in AU, AH, AA, and AG? What
makes this calculation straightforward?
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