Question

Hydrogen peroxide, in its reaction with $KI{O}_4$ and $N{H}_{2}OH$ respectively, is acting as a:

• A. reducing agent, oxidising agent
• B. reducing agent, reducing agent
• C. oxidising agent, oxidising agent
• D. oxidising agent, reducing agent

Answer 1

The correct option is A reducing agent, oxidising agent

$H_2{O}_2$ reacts with $KI{O}_4$ as follows,

$K\stackrel{+7}{I}{O}_4+H_2{O}_2\to K\stackrel{+5}{I}{O}_3+H_{2}O+O_2$

In the reaction of $KI{O}_4$ with $H_2{O}_2$, the oxidation state of $I$ varies from $+7$ to $+5$, i.e., oxidation state decreases. Thus $KI{O}_4$ gets reduced and hence, $H_2{O}_2$ acts as a reducing agent.

$H_2{O}_2$ reacts with $N{H}_{2}OH$ as follows:

$2\stackrel{-1}{N}{H}_{2}OH+4H_2{O}_2\to {\stackrel{+3}{N}}_2{O}_3+7H_{2}O$

In this reaction, the oxidation state of $N$ varies from $-1$ to $+3$ i.e., oxidation state increases and hence $H_2{O}_2$ acts as an oxidising agent.