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(D) In the reaction $NH_4NO_3 \xrightarrow{\Delta} N_2O + 2H_2O$,the oxidation state of nitrogen in $NH_4^+$ is $-3$ and in $NO_3^-$ is $+5$. In the p

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Both $(B)$ and $(C)$.

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(D) In the reaction $NH_4NO_3 \xrightarrow{\Delta} N_2O + 2H_2O$,the oxidation state of nitrogen in $NH_4^+$ is $-3$ and in $NO_3^-$ is $+5$. In the product $N_2O$,the oxidation state of nitrogen is $+1$. Since the oxidation state of nitrogen changes from $-3$ and $+5$ to $+1$,this is a comproportionation reaction. Additionally,this is a thermal decomposition reaction where a single compound breaks down into simpler substances upon heating. Therefore,the reaction is both a comproportionation and a thermal decomposition redox reaction.

Assign $A, B, C, D$ from the given type of reaction: $NH_4NO_3 \xrightarrow{\Delta} N_2O + 2H_2O$.

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