Which one of the following is an example of a disproportionation reaction?

Which ion undergoes disproportionation in an aqueous solution?

Observe the following reaction:
$Cl_{2(g)} + 2OH^{-}_{(aq)} \rightarrow ClO^{-}_{(aq)} + Cl^{-}_{(aq)} + H_2O_{(l)}$
Identify the correct statements about this reaction:
$I$. $Cl_{2(g)}$ is oxidized to $ClO^{-}_{(aq)}$
$II$. $Cl_{2(g)}$ is oxidized to $Cl^{-}_{(aq)}$
$III$. $Cl_{2(g)}$ is reduced to $ClO^{-}_{(aq)}$
$IV$. $Cl_{2(g)}$ is reduced to $Cl^{-}_{(aq)}$
The correct answer is:

What products are expected from the disproportionation reaction of hypochlorous acid?

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$H_2O_2 \xrightarrow{R.T} H_2O + \frac{1}{2} O_2$

The reaction $Cl_2 + 2OH^{-} \to ClO^{-} + Cl^{-} + H_2O$ represents the process of bleaching. Identify and name the species that bleaches the substances due to its oxidising action.