Consider the following reaction
\(\mathrm{MnO_4^- + 8H^+ + 5e^- \to Mn^{2+} + 4H_2O},\ E^\circ = 1.51\ \mathrm{V}\).
The quantity of electricity required in Faraday to reduce five moles of \(\mathrm{MnO_4^-}\) is ___________. (Integer answer)
\(\mathrm{MnO_4^- + 8H^+ + 5e^- \to Mn^{2+} + 4H_2O},\ E^\circ = 1.51\ \mathrm{V}\).
The quantity of electricity required in Faraday to reduce five moles of \(\mathrm{MnO_4^-}\) is ___________. (Integer answer)
Show Hint
Correct Answer: 25
Solution and Explanation
For 5 mol \(\mathrm{MnO_4^-}\): charge = \(5 \times 5 = 25\) F.
Answer: 25
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