Consider the half-cell reduction reaction: Mn^2++2 e^- → Mn, E^0=-1.18 V; Mn^2+ → Mn^3++ e^-, E^0=-1.51 V The E^0 for the reaction 3 Mn^2+ → Mn^0+2…

Consider the half-cell reduction reaction : $$\begin{aligned} & \mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^0=-1.18 \mathrm{~V} \\ & \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^0=-1.51 \mathrm{~V} \end{aligned} $$ The $\displaystyle \mathrm{E}^0$ for the reaction $\displaystyle 3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^0+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are, respectively :