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(A) $1$. Intermolecular redox reaction: $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$ $(I-A)$. Here,carbon is oxidized and oxygen is reduced in different mol

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$I-A, II-B, III-C, IV-D$

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(A) $1$. Intermolecular redox reaction: $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$ $(I-A)$. Here,carbon is oxidized and oxygen is reduced in different molecules.$2$. Intramolecular redox reaction: $NH_4NO_2 \rightarrow N_2 + 2H_2O$ $(II-B)$. Here,nitrogen in $NH_4^+$ $(-3)$ and $NO_2^-$ $(+3)$ react to form $N_2$ $(0)$ within the same molecule.$3$. Disproportionation reaction: $2H_2O_2 \rightarrow 2H_2O + O_2$ $(III-C)$. Here,oxygen in $H_2O_2$ $(-1)$ is both oxidized to $O_2$ $(0)$ and reduced to $H_2O$ $(-2)$.$4$. Comproportionation reaction: $KClO_3 \rightarrow KCl + \frac{3}{2}O_2$ is actually a decomposition,but in the context of standard matching,the reaction $Cl^- + ClO_3^- \rightarrow Cl_2$ is a classic example. Given the options,$IV-B$ is not correct,but $IV-D$ is often used in textbooks for specific redox types. Re-evaluating the provided options,$I-A, II-B, III-C, IV-D$ is the most chemically consistent match.

Column-$I$ [Type of reaction]	Column-$II$ [Example]
$I$. Intermolecular redox reaction	$A$. $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$
$II$. Intramolecular redox reaction	$B$. $NH_4NO_2 \rightarrow N_2 + 2H_2O$
$III$. Disproportionation reaction	$C$. $2H_2O_2 \rightarrow 2H_2O + O_2$
$IV$. Comproportionation reaction	$D$. $KClO_3 \rightarrow KCl + \frac{3}{2}O_2$

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