Which of the following are disproportionation | vedclass

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(A) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.$(A)$ $Cl_2 + 2 NaOH \rightarrow

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$A, B, D$ only

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(A) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.$(A)$ $Cl_2 + 2 NaOH \rightarrow NaCl + NaOCl + H_2O$: The oxidation state of $Cl$ changes from $0$ to $-1$ (reduction) and from $0$ to $+1$ (oxidation). This is a disproportionation reaction.$(B)$ $2 H_2O_2 \rightarrow 2 H_2O + O_2$: The oxidation state of $O$ in $H_2O_2$ is $-1$. It changes to $-2$ in $H_2O$ (reduction) and to $0$ in $O_2$ (oxidation). This is a disproportionation reaction.$(C)$ $2 KMnO_4 \rightarrow K_2MnO_4 + MnO_2 + O_2$: The oxidation state of $Mn$ changes from $+7$ to $+6$ and $+4$ (both reduction). This is not a disproportionation reaction.$(D)$ $3 MnO_4^{2-} + 4 H^+ \rightarrow 2 MnO_4^- + MnO_2 + 2 H_2O$: The oxidation state of $Mn$ changes from $+6$ to $+7$ (oxidation) and from $+6$ to $+4$ (reduction). This is a disproportionation reaction.Thus, reactions $(A)$, $(B)$, and $(D)$ are disproportionation reactions.

Which of the following are disproportionation reactions?
$(A)$ $Cl_2 + 2 NaOH \rightarrow NaCl + NaOCl + H_2O$
$(B)$ $2 H_2O_2 \rightarrow 2 H_2O + O_2$
$(C)$ $2 KMnO_4 \rightarrow K_2MnO_4 + MnO_2 + O_2$
$(D)$ $3 MnO_4^{2-} + 4 H^+ \rightarrow 2 MnO_4^- + MnO_2 + 2 H_2O$

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Which of the following are disproportionation reactions?$(A)$ $Cl_2 + 2 NaOH \rightarrow NaCl + NaOCl + H_2O$$(B)$ $2 H_2O_2 \rightarrow 2 H_2O + O_2$$(C)$ $2 KMnO_4 \rightarrow K_2MnO_4 + MnO_2 + O_2$$(D)$ $3 MnO_4^{2-} + 4 H^+ \rightarrow 2 MnO_4^- + MnO_2 + 2 H_2O$