Question

For the following half-cell reactions,

E^{\circ}

values are:

\begin{aligned} & \mathrm{Mn}^{2+}(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}(l) \longrightarrow \mathrm{MnO}_2(\mathrm{~s})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-} ; E^{\circ}=-123 \mathrm{~V} \\ & \mathrm{MnO}_4^{-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+3 \mathrm{e}^{-} \longrightarrow \mathrm{MnO}_2(\mathrm{~s})+2 \mathrm{H}_2 \mathrm{O}(l) ; E^{\circ}=+1.70 \mathrm{~V} \end{aligned}

Thus,

Accepted Answer

$\mathrm{MnO}_2$ disproportionates to $\mathrm{Mn}^{2+}$ and $\mathrm{MnO}_4^{-}$in acid solution

Answer

$\mathrm{Mn}^{2+}$ reacts with $\mathrm{MnO}_4^{-}$ in acid solution to form $\mathrm{MnO}_2$

Answer

$\mathrm{Mn}\left(\mathrm{MnO}_4\right)_2$ is stable in acid solution

Answer

None of the above

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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