Question

Which one of the following reactions demonstrates that $H_2{O}_2$ acts as an oxidising agent in the basic medium?

• A. $N{a}_{2}C{O}_3+H_2{O}_2\to N{a}_2{O}_2+H_{2}O+C{O}_2$
• B. $2\left[Fe\right(CN{)}_6{]}^{3-}+H_2{O}_2+2O{H}^{-}\to 2\left[Fe\right(CN{)}_6{]}^{4-}+2H_{2}O+O_2$
• C. $M{n}^{2+}+H_2{O}_2+2O{H}^{-}\to Mn{O}_2+2H_{2}O$
• D. $Mn{O}_2+H_2{O}_2+2H^{+}\to M{n}^{2+}+2H_{2}O+O_2$

Answer 1

Answer: (C)

$M{n}^{2+}+H_2{O}_2+2O{H}^{-}\to Mn{O}_2+2H_{2}O$

Solution:

Oxidizing agents itself undergo reduction (gain of electrons) hence in the following reactions, $H_2{O}_2$ acts as Oxidizing agents.

$M{n}^{2+}+H_2{O}_2+2O{H}^{-}\to Mn{O}_2+2H_{2}O$

This is an oxidation -reduction (redox) reaction:

$M{n}^{2+}-2e^{-}\to M{n}^{4+}$ (oxidation)

$2O^{-}+2e^{-}\to 2O^{2-}$ (Reduction)

$M{n}^{2+}$ is a reducing agent, $H_2{O}_2$ is an oxidizing agent

Hence option C is correct