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).
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).
Show Hint
A larger positive E^∘ implies a larger equilibrium constant K.
Updated On: Mar 19, 2026
- I, II and III are correct
- II and III are correct
- I, II and IV are correct
- I and IV are correct
Show Solution
Verified By Collegedunia
The Correct Option is C
Solution and Explanation
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.
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