Which one of the following is a disproportion | vedclass

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

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$4 KClO_{3(s)} \stackrel{\Delta}{\longrightarrow} KCl_{(s)} + 3 KClO_{4(s)}$

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(C) disproportionation reaction is a type of redox reaction in which the same element is simultaneously oxidized and reduced.In the reaction $4 KClO_{3(s)} \stackrel{\Delta}{\longrightarrow} KCl_{(s)} + 3 KClO_{4(s)}$:The oxidation state of chlorine in $KClO_3$ is $+5$.In $KCl$, the oxidation state of chlorine is $-1$ (reduction).In $KClO_4$, the oxidation state of chlorine is $+7$ (oxidation).Since the same element (chlorine) is both oxidized and reduced, this is a disproportionation reaction.

Which one of the following is a disproportionation reaction?

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