Question
Which of the following equations depict the oxidising nature of $${H_2}{O_2}?$$
A.
$$2MnO_4^ - + 6{H^ + } + 5{H_2}{O_2} \to $$ $$2M{n^{2 + }} + 8{H_2}O + 5{O_2}$$
B.
$$2F{e^{3 + }} + 2{H^ + } + {H_2}{O_2} \to $$ $$2F{e^{2 + }} + 2{H_2}O + {O_2}$$
C.
$$2{I^ - } + 2{H^ + } + {H_2}{O_2} \to {I_2} + 2{H_2}O$$
D.
$$KI{O_4} + {H_2}{O_2} \to KI{O_3} + {H_2}O + {O_2}$$
Answer :
$$2{I^ - } + 2{H^ + } + {H_2}{O_2} \to {I_2} + 2{H_2}O$$
Solution :
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), $$MnO_4^ - $$ 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 $${I^{5 + }}.$$