Question

Which of the following equations depict the oxidising nature
of H₂O₂?
(a) 2MnO₂⁻ + 6H⁺ + 5H₂O₂ → 2Mn²⁺ + 8H₂O + 5O₂
(b) 2Fe³⁺ + 2H⁺ + H₂O₂ → 2Fe²⁺ + 2H₂O + O₂
(c) 2I⁻ + 2H⁺ + H₂O₂ → I₂ + 2H₂O
(d) KIO₄ + H₂O₂ → KIO₃ + H₂O + O₂

Answer 1

Answer:

(b) 2Fe3+2H+H2O2=2Fe2+2H2O+O2

Answer 2

The following equations depict the oxidising nature  of H₂O₂

(c) 2I⁻ + 2H⁺ + H₂O₂ → I₂ + 2H₂O

In the third reaction,

2I⁻ + 2H⁺ + H₂O₂ →I₂ + 2H₂O

The oxidation no. of iodine in I⁻ is -1 in the reactant side.

It increases to 0 in I₂ in the product side.

So, due to H₂O₂, the oxidation no. of iodine increases from -1 to 0 (I⁻ to I₂).

Therefore we can say that here H₂O₂ acts as an oxidising agent.

Option (c) is correct.