Question

Consider the following statements:
Statement I: The entropy of pure crystalline solid approaches zero as the temperature approaches absolute zero value.
Statement II: For a reaction at equilibrium, \(\Delta G\) is zero.

• A. Both statements I and II are correct.
• B. Both statements I and II are not correct.
• C. Statement I is correct, but statement II is not correct.
• D. Statement I is not correct, but statement II is correct.

Hint:

Understanding the third law of thermodynamics and the conditions for chemical equilibrium is crucial for correctly interpreting changes in entropy and Gibbs free energy.

Answer 1

The Correct Option is A

To solve this problem, we need to analyze two statements and determine which one is correct regarding entropy and Gibbs free energy at equilibrium.

1. Analyzing Statement I:
Statement I says, "The entropy of pure crystalline solid approaches zero as the temperature approaches absolute zero value." This is a correct statement based on the Third Law of Thermodynamics, which states that the entropy of a perfect crystalline solid approaches zero as the temperature approaches 0 K.

2. Analyzing Statement II:
Statement II says, "For a reaction at equilibrium, \( \Delta G \) is zero." This is also correct. At equilibrium, the Gibbs free energy \( \Delta G \) is zero because the system has reached a state where no net change occurs.

3. Final Answer:
Both statements I and II are correct. Therefore, the correct option is the one where both statements are correct.

Final Answer:
The correct option is (A) Both statements I and II are correct.