Question

Statement I: The entropy of steam is greater than the entropy of liquid water.
Statement II: At ${100}^{o}C$, the average kinetic energy of the steam molecules is greater than the average kinetic energy of the liquid water molecules.

• A. Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.
• B. Both the Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.
• C. Statement 1 is correct but Statement 2 is not correct.
• D. Statement 1 is not correct but Statement 2 is correct.
• E. Both the Statement 1 and Statement 2 are not correct.

Answer 1

The correct option is C Statement 1 is correct but Statement 2 is not correct.

Steam and water exist together and are in equilibrium at boiling point. But entropy of steam is more because randomness of $H_{2}O$ is greater in gaseous state than in liquid state.

So statement $I$ is true

The average kinetic energy of a molecule depends on temperature. Hence at $100℃$, both steam and water will have same average kinetic energy.

So statement $II$ is false.