Question

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

• A. $2\left[Fe\right(CN{)}_6]4-+2H^{+}+H_2{O}_2\to 2[Fe(CN{)}_6{]}^{3-}+2H_{2}O$
• B. $I_2+H_2{O}_2+2O{H}^{-}\to 2I^{-}+2H_{2}O+O_2$
• C. $M{n}^{2+}+H_2{O}_2\to M{n}^{4+}+2O{H}^{-}$
• D. $PbS+4H_2{O}_2\to PbS{O}_4+4H_{2}O$

Answer 1

The correct option is B $I_2+H_2{O}_2+2O{H}^{-}\to 2I^{-}+2H_{2}O+O_2$

In (A), $F{e}^{+2}$ is oxidized to $F{e}^{+3}$ which shows the oxidizing nature of $H_2{O}_2$.

In (B), $I_2$ is reduced to $I^{-}$ which shows the reducing nature of $H_2{O}_2$.

In (C), $M{n}^{+2}$ is oxidized to $M{n}^{+4}$ which shows the oxidizing nature of $H_2{O}_2$.

In (D), $S^{2-}$ is oxidized to $S^{+6}$ which shows the oxidizing nature of $H_2{O}_2$

Answer: (B)