Comproportionation occurs between

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(D) comproportionation reaction is a type of redox reaction where two reactants,each containing the same element but in different oxidation states,for

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$MnO_4^{-}(aq.) + Mn^{2+}(aq.)$

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(D) comproportionation reaction is a type of redox reaction where two reactants,each containing the same element but in different oxidation states,form a product in which the element is in an intermediate oxidation state.In the reaction between $MnO_4^{-}$ ($Mn$ is $+7$) and $Mn^{2+}$ ($Mn$ is $+2$),they react to form $MnO_2$ ($Mn$ is $+4$).Since $+4$ is intermediate between $+7$ and $+2$,this is a comproportionation reaction.The reaction is: $2MnO_4^{-}(aq.) + 3Mn^{2+}(aq.) + 4OH^{-}(aq.) \rightarrow 5MnO_2(s) + 2H_2O(l)$.

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