Which of the following reactions is NOT a dis | vedclass

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(C) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.In option $A$: $KO_2 + H_2O + CO_

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$PbO_2 + H_2O 	o PbO + H_2O_2$

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(C) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.In option $A$: $KO_2 + H_2O + CO_2 	o KHCO_3 + O_2$. The oxidation state of $O$ in $KO_2$ is $-1/2$. In $KHCO_3$,it is $-2$,and in $O_2$,it is $0$. This is a disproportionation reaction.In option $B$: $KClO_3 	o KClO_4 + KCl$. The oxidation state of $Cl$ changes from $+5$ to $+7$ (oxidation) and $-1$ (reduction). This is a disproportionation reaction.In option $C$: $PbO_2 + H_2O 	o PbO + H_2O_2$. The oxidation state of $Pb$ changes from $+4$ to $+2$ (reduction). The oxidation state of $O$ in $PbO_2$ is $-2$ and in $H_2O_2$ is $-1$. This is $NOT$ a disproportionation reaction because only $Pb$ is reduced and $O$ is oxidized; they are different elements.In option $D$: This is a Cannizzaro-type reaction where the same carbon atom undergoes oxidation and reduction. This is a disproportionation reaction.

Which of the following reactions is $NOT$ a disproportionation reaction?

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