How would each of the following changes affect the number of microstates availab
ID: 952251 • Letter: H
Question
How would each of the following changes affect the number of microstates available to a system: increase in temperature, decrease in volume, change of state from liquid to gas? Using the heat of vaporization in Appendix calculate the entropy change for the vaporization of water at 25 degree C and at 100 degree C. From your knowledge of microstates and the structure of liquid water, explain the difference in these two values. What do you expect for the sign of AS in a chemical reaction in which two moles of gaseous reactants are converted to three moles of gaseous products? For which of the processes in Exercise 19.9 does the entropy of the system increase? In a chemical reaction two gases combine to form a solid. What do you expect for the sign of AS? How does the entropy of the system change in the processes described in Exercise 19.10? How does the entropy of the system change when a solid melts, a gas liquefies, a solid sublimes? How does the entropy of the system change when the temperature of the system increases, the volume of a gas increases, equal volumes of ethanol and water are mixed to form a solution.Explanation / Answer
19.32
- sign. Which means delta S decreases. Entropy is the randomness of a system. In a solid system moleculea are closely packed and it has a particular shape. Therefore disordeness of a solid system is lower than the gas system.
19.34
a- when temperature increases entropy increases.. best example is when heat is supplied, a liquid evaporises a gas creates.. entropy of a gas is higher than the entropy of a liquid.
b- entropy increases. Because now the gas has more space to move.. therefore disordeness increases
c- ethanol and water molecules can make inter molecular hydrogen bonds. Then then can attach together. So disordeness dcreasea.. entropy also decreasea.
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