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Asked by Awdhesh Last Modified
Answer The standard molar entropy of a substance typically increases when it undergoes a phase change from a solid to a liquid, and then from a liquid to a gas. This is because as a substance transitions from a more ordered state (solid) to a less ordered state (liquid or gas), the number of possible microstates increases, leading to an increase in entropy.
Therefore, the standard molar entropy of H2O(s)H2O(s) is expected to be greater than that of H2O(l)H2O(l).
This is because in the solid phase, the molecules of water (H2OH2O) are more ordered and constrained in their positions, resulting in lower entropy compared to the liquid phase, where the molecules are free to move and have more disorder.
So, the standard molar entropy of H2O(s)H2O(s) is expected to be more than 70 J K−1−1 mol−1−1.
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