Question

${Cl{O}_3}^{-}+C{l}^{-}\to C{l}_2+Cl{O}_2$
Which of the following is correct for this reaction:

• A. Its a disproportion reaction
• B. $Cl$ is both oxidised and reduced
• C. $Cl$ is both reducing and oxydising agent
• D. All of these

Answer 1

The correct option is D All of these

The given reaction is disproportion reaction as $Cl$ in the reaction is oxidized as well as reduced. Disproportionation is a specific type of redox reaction in which an element from a reaction undergoes both oxidation and reduction to form two different products.

In the reaction the oxidation state of $Cl$ in ${Cl{O}_3}^{-}$ is $+5$ which is decreasing to either $0$ in $C{l}_2$ or $+4$ in $Cl{O}_2$. Means $Cl$ is reduced and acting as oxidizing agent.

And the oxidation state of $Cl$ in ${Cl}^{-}$ is $-1$ which is increasing to either $0$ in $C{l}_2$ or $+4$ in $Cl{O}_2$. Means $Cl$ is oxidized and acting as reducing agent.