Which of the following are disproportionation | vedclass

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(D) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.$(A)$ $2 NO_{2(g)} + 2 NaOH_{(aq)

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$A, B, C$

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(D) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.$(A)$ $2 NO_{2(g)} + 2 NaOH_{(aq)} \rightarrow NaNO_{2(aq)} + NaNO_{3(aq)} + H_2O_{(l)}$: Nitrogen in $NO_2$ $(+4)$ is oxidized to $NO_3^-$ $(+5)$ and reduced to $NO_2^-$ $(+3)$. This is a disproportionation reaction.$(B)$ $Cl_{2(g)} + 2 NaOH_{(aq)} \rightarrow NaClO_{(aq)} + NaCl_{(aq)} + H_2O_{(l)}$: Chlorine in $Cl_2$ $(0)$ is oxidized to $ClO^-$ $(+1)$ and reduced to $Cl^-$ $(-1)$. This is a disproportionation reaction.$(C)$ $3 ClO^- \rightarrow 2 Cl^- + ClO_3^-$: Chlorine in $ClO^-$ $(+1)$ is reduced to $Cl^-$ $(-1)$ and oxidized to $ClO_3^-$ $(+5)$. This is a disproportionation reaction.$(D)$ $3 Mg_{(s)} + N_{2(g)} \rightarrow Mg_3N_{2(s)}$: This is a combination reaction,not a disproportionation reaction.

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