Which of the following oxides undergoes dispr | vedclass

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(B) Disproportionation is a reaction where an element in an intermediate oxidation state is simultaneously oxidized and reduced.In the case of $N_2O_4

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$N_2O_4$

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(B) Disproportionation is a reaction where an element in an intermediate oxidation state is simultaneously oxidized and reduced.In the case of $N_2O_4$,the oxidation state of nitrogen is $+4$.When $N_2O_4$ reacts with $NaOH$,it forms a mixture of nitrite $(NO_2^-)$ and nitrate $(NO_3^-)$ salts:$N_2O_4 + 2NaOH \rightarrow NaNO_2 + NaNO_3 + H_2O$.Here,nitrogen is reduced from $+4$ to $+3$ in $NaNO_2$ and oxidized from $+4$ to $+5$ in $NaNO_3$.

Which of the following oxides undergoes disproportionation with $NaOH$ solution?

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