Answer:
1. 8.8kJ/mol
2. The process is not favorable.
3. The reason is in the answer.
4. Process 1.
Explanation:
1. ΔG° = ΔG° products - ΔG° reactants
ΔG° = -228.4kJ/mol - (-237.2kJ/mol) = 8.8kJ/mol
2. The process is not favorable because ΔG > 0
3. As the reaction is an equilibrium, a little amount of water will change from liquid to gas. This is the reason because of water has a measurable equilibrium vapor pressure.
4. Entropy is greater in process 1 because the structure of H2O(s) is more organized than H2O(l) (S of H2O(s) is lower than H2O(l)).
ΔS of H2O(s)⇄H2O(g) is greater than H2O(l)⇄H2O(g)