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(A) The reaction is $2Ca(OH)_2 + 2Cl_2 \longrightarrow Ca(OCl)_2 + CaCl_2 + 2H_2O$.In this reaction,the oxidation state of $Cl$ in $Cl_2$ is $0$. In t

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for disproportionation reaction.

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(A) The reaction is $2Ca(OH)_2 + 2Cl_2 \longrightarrow Ca(OCl)_2 + CaCl_2 + 2H_2O$.In this reaction,the oxidation state of $Cl$ in $Cl_2$ is $0$. In the products,the oxidation state of $Cl$ in $Ca(OCl)_2$ is $+1$ and in $CaCl_2$ is $-1$.Since the same element $(Cl)$ is simultaneously oxidized and reduced,this is a disproportionation reaction.Therefore,the correct assignment is $A$.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Ca(OH)_2 + Cl_2 \longrightarrow CaOCl_2 + H_2O$

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.$Ca(OH)_2 + Cl_2 \longrightarrow CaOCl_2 + H_2O$