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Question: In the reaction: \(Cl_{2} + OH^{-} \rightarrow Cl^{-} + ClO_{4}^{-} + H_{2}O\)...

In the reaction:

Cl2+OH−→Cl−+ClO4−+H2OCl_{2} + OH^{-} \rightarrow Cl^{-} + ClO_{4}^{-} + H_{2}O

A

Chlorine is oxidized.

B

Chlorine is reduced.

C

Chlorine is oxidised as well as reduced.

D

Chlorine is neither oxidised nor reduced.

Answer

Chlorine is oxidised as well as reduced.

Explanation

Solution

: Cl2+OH−→Cl−+ClO4−+H2OCl_{2} + OH^{-} \rightarrow Cl^{-} + ClO_{4}^{-} + H_{2}O

Cl02→Cl−−1{\overset{0}{Cl}}_{2} \rightarrow \overset{- 1}{Cl^{-}} (Reduction)

Cl20→Cl+7O4−\overset{0}{Cl_{2}} \rightarrow \overset{+ 7}{Cl}O_{4}^{-} (Oxidation)