Question

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

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

Answer 1

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

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

In above reaction, $H_2{O}_2$ oxidises $I^{-}$ to $I_2$ and itself gets reduced to $H_{2}O$ so, this reaction depicts oxidising nature of $H_2{O}_2$
In equation (b) iodine gets reduced to +7 to +5 state.
In equation (c) chlorine gets reduced to 0 to -1 state
In equation (d) iodine gets reduced to +0 to -1 state.
Equations in options (b) , (c), (d) depict the reducing nature of $H_2{O}_2$
Option (a) is correct