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(A) In the reaction $2Se_2Cl_2 \xrightarrow{\Delta} SeCl_4 + 3Se$,the oxidation state of $Se$ in $Se_2Cl_2$ is $+1$.In $SeCl_4$,the oxidation state of

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for disproportionation reaction.

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(A) In the reaction $2Se_2Cl_2 \xrightarrow{\Delta} SeCl_4 + 3Se$,the oxidation state of $Se$ in $Se_2Cl_2$ is $+1$.In $SeCl_4$,the oxidation state of $Se$ is $+4$.In $Se$,the oxidation state of $Se$ is $0$.Since the same element $(Se)$ is simultaneously oxidized (from $+1$ to $+4$) and reduced (from $+1$ to $0$),this is a disproportionation reaction.Therefore,the correct assignment is $(A)$.

Assign $A, B, C, D$ from the given type of reaction.
$2Se_2Cl_2 \xrightarrow{\Delta} SeCl_4 + 3Se$

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Assign $A, B, C, D$ from the given type of reaction.$2Se_2Cl_2 \xrightarrow{\Delta} SeCl_4 + 3Se$