Which of the following reactions are disproportionation reaction? (a) $2Cu^+ \longrightarrow Cu^{2+} + Cu^0$ (

Question

Which of the following reactions are disproportionation reaction? (a) $2Cu^+ \longrightarrow Cu^{2+} + Cu^0$ (b) $3MnO_4^{2-} + 4H^+ \longrightarrow 2MnO_4^- + MnO_2 + 2H_2O$ (c) $2KMnO_4 \xrightarrow{\Delta} K_2MnO_4 + MnO_2 + O_2$ (d) $2MnO_4^- + 3Mn^{2+} + 2H_2O \longrightarrow 5MnO_2 + 4H^+$

Accepted Answer

A disproportionation reaction is one where the same element is simultaneously oxidized and reduced. (a) $Cu^+$ ($+1$) goes to $Cu^{2+}$ ($+2$, oxidation) and $Cu^0$ ($0$, reduction). (b) $Mn$ in $MnO_4^{2-}$ ($+6$) goes to $MnO_4^-$ ($+7$, oxidation) and $MnO_2$ ($+4$, reduction). (c) $KMnO_4$ decomposition is not disproportionation. (d) $Mn$ in $MnO_4^-$ ($+7$) and $Mn^{2+}$ ($+2$) both go to $MnO_2$ ($+4$), which is comproportionation.

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