Chapter 10, Problem 1DQ

For the process $\text{A}(l)\to \text{A}(g)$ , which direction is favoredby changes in energy probability? Positional probability?Explain your answer. If you wanted to favor theprocess as written, would you raise or lower the temperatureof the system? Explain.

Interpretation Introduction

Interpretation:

For the process $\text{A}\left(\text{l}\right)\to \text{A}\left(\text{g}\right)\text{,}$ the favored direction due to change in energy probability, position probability and positional probability needs to be determined. To favor the process, whether the temperature of the system is raised or lowered needs to be determined.

Concept Introduction :

In an isothermal and isobaric (constant pressure and temperature) thermodynamic system, Gibbs free energy is a measure of the amount of energy available to do work.

Answer to Problem 1DQ

To favor the process as written the temperature of the system must be raised because the conversion of liquid to gas is an endothermic reaction.

Explanation of Solution

As molecules in gaseous state could move faster than the molecules in the liquid state thus, the gaseous molecules contain more kinetic energy and hence $\text{A}\left(\text{l}\right)\to \text{A}\left(\text{g}\right)\text{,}$ direction is favored by energy randomness. The direction of liquid to gas is favored by positional randomness.

This is because the movement of the gaseous molecules is more random than liquid molecules of a substance.

To favor the process as written, the temperature of the system must be raised because the conversion of liquid to gas is an endothermic reaction.