Question

The reaction of zinc with \( \text{Cu}^{2+} \) produces the following. Entropy change \( \Delta S \) is given by \( 96.5 J \cdot \text{mol}^{-1} \cdot \text{K}^{-1} \).

• A. \( 2 \times 10^4 \, \text{V} \, \text{K}^{-1} \)
• B. \( 10 \times 10^3 \, \text{V} \, \text{K}^{-1} \)
• C. \( 5 \times 10^4 \, \text{V} \, \text{K}^{-1} \)
• D. \( 9.65 \times 10^4 \, \text{V} \, \text{K}^{-1} \)

Hint:

Entropy change is related to the amount of disorder in a system and can be calculated using thermodynamic equations.

Answer 1

The Correct Option is A

Step 1: Applying the entropy change equation.
The entropy change of a system is related to the energy produced in the system. By using the given values for entropy and potential change, the required value is calculated.

Step 2: Conclusion.
The entropy change value is \( 2 \times 10^4 \, \text{V} \, \text{K}^{-1} \), corresponding to option (1).