Which of the following equation depicts the oxidizing nature of

Question:

Which of the following equation depicts the oxidizing nature of $\mathrm{H}_{2} \mathrm{O}_{2}$ ?

  1.  $\mathrm{Cl}_{2}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow 2 \mathrm{HCl}+\mathrm{O}_{2}$

  2. $\mathrm{KlO}_{4}+\mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{KlO}_{3}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$

  3. $2 \mathrm{I}^{-}+\mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{H}^{+} \rightarrow \mathrm{I}_{2}+2 \mathrm{H}_{2} \mathrm{O}$

  4. $\mathrm{I}_{2}+\mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{OH}^{-} \rightarrow 2 \mathrm{I}^{-}+2 \mathrm{H} 2 \mathrm{O}+\mathrm{O}_{2}$

Correct Option: , 3

Solution:

$2 \mathrm{l}^{-}+\mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{H}^{+} \rightarrow \mathrm{I}_{2}+2 \mathrm{H}_{2} \mathrm{O}$

Oxygen reduces from $-1$ to $-2$ So, its reduction will takes place. Hence it will behave as oxidising agent or it shows oxidising nature. While in other option it change from $(-1)$ to 0 .

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