Question

Which of the following equation depict the oxidising nature of $H_2{O}_2$?

• A. $2Mn{O}_4^{-}+6H^{+}+5H_2{O}_2\to 2M{n}^2+8H_{2}O+5O_2$
• B. $2F{e}^{3+}+2H^{+}+H_2{O}_2\to 2F{e}^2+2H_{2}O+O_2$
• C. $2I^{-}+2H^{+}+H_2{O}_2\to I_2+2H_{2}O$
• D. $KI{O}_4+H_2{O}_2\to KI{O}_3+H_{2}O+O_2$

Answer 1

Answer: (C)

$2I^{-}+2H^{+}+H_2{O}_2\to I_2+2H_{2}O$

Oxidising nature of $H_2{O}_2$ means it oxidises other substance and itself gets reduced. In such reactions $O_2$ is not evolved.

In (a), $Mn{O}_4^{-}$ gets reduced from $M{n}^{7+}$ to $M{n}^{2+}$.

In (b), $F{e}^{3+}$ gets reduced to $F{e}^{2+}$

In (c), $I^{-}$ gets oxidised to $I_2$.

In (d), $KI{O}_4$ gets reduced from $I^{7+}$ to $I^{5+}$.

Therefore in option (C) is correct Answer.