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(A) disproportionation reaction is a type of redox reaction in which the same element is simultaneously oxidized and reduced.In the reaction $3 MnO_{4

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$3 MnO_{4}^{2-} + 4 H^{+} \rightarrow 2 MnO_{4}^{-} + MnO_{2} + 2 H_{2}O$

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(A) disproportionation reaction is a type of redox reaction in which the same element is simultaneously oxidized and reduced.In the reaction $3 MnO_{4}^{2-} + 4 H^{+} \rightarrow 2 MnO_{4}^{-} + MnO_{2} + 2 H_{2}O$:$1$. The oxidation state of $Mn$ in $MnO_{4}^{2-}$ is $+6$.$2$. In $MnO_{4}^{-}$,the oxidation state of $Mn$ is $+7$ (Oxidation).$3$. In $MnO_{2}$,the oxidation state of $Mn$ is $+4$ (Reduction).Since the same element $(Mn)$ is both oxidized and reduced,this is a disproportionation reaction.

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

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$1 \ mole$ of $MnO_4^{2-}$ in neutral aqueous medium disproportionates to:

$3ClO^- \to ClO_3^- + 2Cl^-$; This reaction is an example of which of the following?

The $Mn^{3+}$ ion is unstable in solution and undergoes disproportionation to give $Mn^{2+}$,$MnO_2$,and $H^{+}$ ion. Write a balanced ionic equation for the reaction.

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