Question

Identify the correct statements from the following: A) At 298 K, the potential of the hydrogen electrode placed in a solution of pH = 10 is -0.59 V.
B) The limiting molar conductivity of \( \text{Ca}^{2+} \) and \( \text{Cl}^- \) is 119 and 76 \( \text{S cm}^2 \text{mol}^{-1} \), respectively. The limiting molar conductivity of \( \text{CaCl}_2 \) is 195 \( \text{S cm}^2 \text{mol}^{-1} \).
C) The correct relationship between \( K_c \) and \( E_{\text{cell}} \) is \( E_{\text{cell}} = \frac{2.303RT}{nF} \log K_c \).

• A. A, B, C
• B. A, B only
• C. A, C only
• D. B, C only

Hint:

For electrochemical reactions, the relationship between the cell potential and the equilibrium constant is governed by the Nernst equation, which can help determine the direction of the reaction.

Answer 1

The Correct Option is C

A) The potential of the hydrogen electrode in a solution with pH = 10 is correctly calculated using the Nernst equation, resulting in -0.59 V. B) The limiting molar conductivities of \( \text{Ca}^{2+} \) and \( \text{Cl}^- \) are correctly stated, but the limiting conductivity of \( \text{CaCl}_2 \) is actually 195 \( \text{S cm}^2 \text{mol}^{-1} \). C) The relationship between the equilibrium constant \( K_c \) and the cell potential \( E_{\text{cell}} \) is correctly expressed as \( E_{\text{cell}} = \frac{2.303RT}{nF} \log K_c \).