Question

Which of the following equations depicts the oxidizing nature of ${\mathrm{H}}_2{\mathrm{O}}_2$?

• A. ${\mathrm{Cl}}_2+{\mathrm{H}}_2{\mathrm{O}}_2\to 2\mathrm{HCl}+{\mathrm{O}}_2$
• B. ${\mathrm{KIO}}_4+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{KIO}}_3+{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$
• C. $2{\mathrm{I}}^{-}+{\mathrm{H}}_2{\mathrm{O}}_2+2{\mathrm{H}}^{+}\to {\mathrm{l}}_2+2{\mathrm{H}}_2\mathrm{O}$
• D. ${\mathrm{I}}_2+{\mathrm{H}}_2{\mathrm{O}}_2+2{\mathrm{OH}}^{-}\to 2{\mathrm{l}}^{-}+2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

Answer 1

The correct option is C

$2{\mathrm{I}}^{-}+{\mathrm{H}}_2{\mathrm{O}}_2+2{\mathrm{H}}^{+}\to {\mathrm{l}}_2+2{\mathrm{H}}_2\mathrm{O}$

The explanation for the correct options: (C)

• Oxidation: When there is a positive change in the oxidation state, Oxidation happens.
• ${\mathrm{H}}_2{\mathrm{O}}_2$ because of its oxidizing tendency, it oxidizes other substances and reduces itself.

$2{\mathrm{I}}^{-}+{\mathrm{H}}_2{\mathrm{O}}_2+2{\mathrm{H}}^{+}\to {\mathrm{l}}_2+2{\mathrm{H}}_2\mathrm{O}$

Here, the Iodide ion is getting oxidized to iodine because it switches from $\left(-1\right)$ to $0$.

The explanation for the incorrect options:

(a)

• It will be higher as oxygen drops. As a result, it will behave as an oxidizer or display oxidation indications. In other cases, it switches from
• There is evolution in such a reaction.

(b)

• As oxygen levels fall, they will rise. As a result, it will act as an oxidizer or show signs of oxidation. In other circumstances, it reverts to
• In such a reaction, there is evolution.

(d)

• As the amount of oxygen in the atmosphere decreases, it will rise. As a result, it will either act as an oxidizer or show signs of oxidation.
• In some circumstances, it will swap from one to the other. In this type of reaction, there is evolution.

Hence option (c) is correct: While it changes from $\left(-1\right)$ to $0$ in other choices.