Chemistry

Problem

Consider the following unbalanced redox reaction occurring under standard conditions:

\mathrm{MnO_4^-\,(aq) + Fe^{2+}\,(aq) + H^{+}\,(aq) \rightarrow Mn^{2+}\,(aq) + Fe^{3+}\,(aq) + H_2O\,(l)}

The standard free-energy change for the reaction as written (per mole of

\mathrm{MnO_4^-}

consumed) is

\Delta G^\circ = -3.90\times10^5\,\text{J}

. What is the corresponding standard cell potential

E^\circ_{\text{cell}}

? (Assume

F = 9.65\times10^4\,\text{C\,mol}^{-1}\,e^{-}

.) a)

-0.81\ \text{V}

0.41\ \text{V}

0.81\ \text{V}

1.35\ \text{V}