Question:

If \(E^\circ_{MnO_4^-/MnO_2} = x \, V\) and \(E^\circ_{MnO_2/Mn^{2+}} = y \, V\), what is the value of \(E^\circ_{MnO_4^-/Mn^{2+}}\)?

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Combine electrode potentials using electron-weighted averaging, not direct addition.
Updated On: Jun 20, 2026
  • \( \frac{3x + 2y}{3} \)
  • \( \frac{3x + 2y}{5} \)
  • \( \frac{5x + 3y}{2} \)
  • \( \frac{3x + 5y}{3} \)
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The Correct Option is B

Solution and Explanation

Step 1: Understand concept of standard electrode potential.
When multiple redox steps are involved, overall potential is not simple addition but weighted based on electron transfer numbers in each step.

Step 2: Break into half reactions.

MnO\(_4^-\) → MnO\(_2\) corresponds to 3 electron change. MnO\(_2\) → Mn\(^{2+}\) corresponds to 2 electron change.

Step 3: Use energy additivity principle.

\[ \Delta G^\circ = -nFE^\circ \] Total free energy change is additive, so: \[ n_{total}E_{total} = n_1E_1 + n_2E_2 \]

Step 4: Substitute values.

Total electrons = 5: \[ 5E = 3x + 2y \]

Step 5: Solve for E.

\[ E = \frac{3x + 2y}{5} \]

Step 6: Final conclusion.

Thus standard potential for overall reaction is weighted average based on electrons transferred.
Final Answer: \[ \boxed{\frac{3x + 2y}{5}} \]
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