Question

Which of the following equations depict the oxidising nature of $H_2O_2$?

• A. $2MnO_{4}^{-} + 6H^{+} + 5H_{2}O_{2} \to 2Mn^{2+} + 8H_{2}O + 5O_{2}$
• B. $2Fe^{3+} + 2H^+ + H_2O_2 \to 2Fe^{2+} + 2H_2O + O_2$
• C. $2I^- + 2H^+ + H_2O_2 \to I_2 + 2H_2O$
• D. $KIO_4 + H_2O_2 \to KIO_3 + H_2O + O_2$

Answer 1

Answer: (C)

Oxidising nature of $H_2O_2$ means it oxidises other substance and itself gets reduced. In such reactions $O_2$ is not evolved.
In (a), $MnO_4^-$ gets reduced from $Mn^{7+}$ to $Mn^{2+}$.
In (b), $Fe^{3+}$ gets reduced to $Fe^{2+}$.
In (c), $I^-$ gets oxidised to $I_2$.
In (d), $KIO_4$ gets reduced from $I^{7+}$ to $I^{5+}$ .