Consider the following standard electrode potential values: Fe^3+_( aq ) + e^- → Fe^2+_( aq ) E^°=+0.77 V MnO_4^-_( aq ) +8 H^++5 e^- → Mn^2+_( aq )…

Consider the following standard electrode potential values : $\displaystyle \mathrm{Fe}^{3+}{ }_{(\mathrm{aq})}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}{ }_{(\mathrm{aq})} \mathrm{E}^{\circ}=+0.77 \mathrm{~V}$ $\displaystyle \mathrm{MnO}_{4}{ }^{-}{ }_{(\mathrm{aq})}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}_{2} \mathrm{O}_{(l)} \mathrm{E}^{\circ}=+1.51 \mathrm{~V}$ What is the cell potential for the redox reaction ?