Chapter 4, Problem 4.25E

The value of $\Delta G$ for any phase change at constant $p$ is exactly $0$. Knowing this determine $\Delta S$ for the process

$\text{Au}\left(\text{1}\text{mol},l\right)\to \text{Au}\left(\text{1}\text{mol},\text{g}\right)$

at $2808°\text{C}$ and constant pressure. The enthalpy of vaporization of $\text{Au}$ is $343\text{kJ}/\text{mol}$. Explain why this value is so much larger than the value of $\Delta S$ calculated in the previous exercise.