Question

Which of the following equations depicts only the oxidizing nature of $H_2{O}_2$?

• A. $C{l}_2+H_2{O}_2\to 2HCl+O_2$
• B. $KI{O}_4+H_2{O}_2\to KI{O}_3+H_{2}O+O_2$
• C. $2I^{-}+H_2{O}_2+2H^{+}\to I_2+2H_{2}O$
• D. $I_2+H_2{O}_2+2O{H}^{-}\to 2I^{-}+2H_{2}O+O_2$

Answer 1

The correct option is C $2I^{-}+H_2{O}_2+2H^{+}\to I_2+2H_{2}O$

(a) $C{l}_2+H_2{\stackrel{-1}{O}}_2\to 2HCl+{\stackrel{0}{O}}_2$
In this reaction, oxygen is undergoing oxidation from $-1$ to $0$ oxidation state. Hence, $H_2{O}_2$ behaves as a reducing agent.

(b) $KI{O}_4+H_2{\stackrel{-1}{O}}_2\to KI{O}_3+H_2\stackrel{-2}{O}+{\stackrel{0}{O}}_2$
In this reaction, oxygen is undergoing oxidation from $-1$ to $0$ oxidation state and reduction from $-1$ to $-2$ oxidation state. Hence, $H_2{O}_2$ behaves as a reducing as well as oxidizing agent.

(c) $2I^{-}+H_2{\stackrel{-1}{O}}_2+2H^{+}\to I_2+2H_2\stackrel{-2}{O}$
In this reaction, oxygen is undergoing reduction from $-1$ to $-2$ oxidation state. Hence, $H_2{O}_2$ behaves as an oxidizing agent.

(d) $I_2+H_2{\stackrel{-1}{O}}_2+2O{H}^{-}\to 2I^{-}+2H_2\stackrel{-2}{O}+{\stackrel{0}{O}}_2$
In this reaction, oxygen is undergoing oxidation from $-1$ to $0$ oxidation state and reduction from $-1$ to $-2$ oxidation state. Hence, $H_2{O}_2$ behaves as a reducing as well as oxidizing agent.