Which one of the following is an example of disproportionation...

Which one of the following is an example of disproportionation reaction?

Options

A $3{MnO}_{4}^{2 -} + 4{H}^{+} \to 2{MnO}_{4}^{-} + {MnO}_{2} + 2{H}_{2}O$
B ${MnO}_{4}^{-} + 4{H}^{+} + 4{e}^{-} \to {MnO}_{2} + 2{H}_{2}O$
C $10{I}^{-} + 2{MnO}_{4}^{-} + 16{H}^{+} \to 2{Mn}^{2} + + 8{H}_{2}O + 5{I}_{2}$
D $8{MnO}_{4}^{-} + 3{S}_{2}{O}_{3}^{2 -} + {H}_{2}O \to 8{MnO}_{2} + 6{SO}_{4}^{2 -} + 2{OH}^{-}$

Correct answer

A. $3{MnO}_{4}^{2 -} + 4{H}^{+} \to 2{MnO}_{4}^{-} + {MnO}_{2} + 2{H}_{2}O$

Step-by-step solution

Disproportionation reaction, also sometimes called dismutation reaction, is basically a type of redox reaction involving simultaneous reduction and oxidation of atoms of the same element from one oxidation state (OS) to two different oxidation states.

$\overset{+ 6}{3{MnO}_{4}^{2 -}} + 4{H}^{+} ⟶ \overset{+ 7}{2{MnO}_{4}^{-}} + \overset{+ 4}{{MnO}_{2}} + 2{H}_{2}O$

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