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(A) In the reaction $K_2MnO_4 + H^{+} \longrightarrow KMnO_4 + MnO_2 + H_2O$,the oxidation state of $Mn$ in $K_2MnO_4$ is $+6$.In $KMnO_4$,the oxidati

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$A$. for disproportionation reaction.

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(A) In the reaction $K_2MnO_4 + H^{+} \longrightarrow KMnO_4 + MnO_2 + H_2O$,the oxidation state of $Mn$ in $K_2MnO_4$ is $+6$.In $KMnO_4$,the oxidation state of $Mn$ is $+7$ (oxidation).In $MnO_2$,the oxidation state of $Mn$ is $+4$ (reduction).Since the same element $(Mn)$ in the same oxidation state $(+6)$ is simultaneously oxidized to $+7$ and reduced to $+4$,this is a disproportionation reaction.Therefore,the correct assignment is $A$.

Assign $A, B, C, D$ from the given type of reaction.
$K_2MnO_4 + H^{+} \longrightarrow KMnO_4 + MnO_2 \downarrow$

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Assign $A, B, C, D$ from the given type of reaction.$K_2MnO_4 + H^{+} \longrightarrow KMnO_4 + MnO_2 \downarrow$