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(D) The reaction is: $\underline{N_2}O_4 + H_2O \longrightarrow HNO_3 + HNO_2$.In this reaction,$N_2O_4$ undergoes disproportionation upon hydrolysis.

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If the products are two oxyacids,one with an $-ic$ suffix and the other with an $-ous$ suffix.

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(D) The reaction is: $\underline{N_2}O_4 + H_2O \longrightarrow HNO_3 + HNO_2$.In this reaction,$N_2O_4$ undergoes disproportionation upon hydrolysis.The products are $HNO_3$ (Nitric acid) and $HNO_2$ (Nitrous acid).$HNO_3$ is an oxyacid with an $-ic$ suffix (Nitric acid).$HNO_2$ is an oxyacid with an $-ous$ suffix (Nitrous acid).Therefore,the products are two oxyacids,one with an $-ic$ suffix and the other with an $-ous$ suffix.

In the following reaction,assign the state for the underlined atom in the products of complete hydrolysis at $R.T.$:
$\underline{N_2}O_4 + H_2O \longrightarrow HNO_3 + HNO_2$

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In the following reaction,assign the state for the underlined atom in the products of complete hydrolysis at $R.T.$:$\underline{N_2}O_4 + H_2O \longrightarrow HNO_3 + HNO_2$