Question

Which of the following relation represents correct relation between standard electrode potential and equilibrium constant? I. log K = (nF E^∘)/(2.303RT) II. K = e⁽ⁿF E^∘⁾/⁽RT⁾ III. log K = (-nF E^∘)/(2.303RT) IV. log K = (0.4342 nF E^∘)/(RT) Choose the correct statement(s).

• A. I, II and III are correct
• B. II and III are correct
• C. I, II and IV are correct
• D. I and IV are correct

Hint:

A larger positive E^∘ implies a larger equilibrium constant K.

Answer 1

The Correct Option is C

Step 1: The relation between standard electrode potential and equilibrium constant is: Δ G^∘ = -nF E^∘ and Δ G^∘ = -RT ln K Step 2: Equating: RT ln K = nF E^∘ ⟹ ln K = (nF E^∘)/(RT) Step 3: Converting to base-10 logarithm: log K = (nF E^∘)/(2.303RT) Step 4: Since log₁0 e = 0.4342, log K = (0.4342 nF E^∘)/(RT) Hence, statements I, II and IV are correct.