Which of the following equation depicts the oxidizing nature of H₂O₂?

Solution

Chemistry ma’am · 3 steps

Track the oxygen of H₂O₂: ending up in water means it was reduced, so it was the oxidant.

1. Oxygen in H2O2. In H₂O₂ each oxygen is in the -1 state, halfway between 0 (in O₂) and -2 (in H₂O). So H₂O₂ can go either way.
2. Two possible roles. If H₂O₂ becomes H₂O, oxygen goes from -1 to -2. It is reduced, so it is the oxidizing agent. If H₂O₂ gives off O₂, oxygen goes from -1 to 0. It is oxidized, so it is the reducing agent.

   Option	H₂O₂ becomes	Other species	H₂O₂ acts as
   (a)	O₂ (O: -1 → 0)	Cl: 0 → -1, reduced	reducing agent
   (b)	O₂ (O: -1 → 0)	I: +7 → +5, reduced	reducing agent
   (c)	H₂O (O: -1 → -2)	I: -1 → 0, oxidized	oxidizing agent
   (d)	O₂ (O: -1 → 0)	I: 0 → -1, reduced	reducing agent

3. So. Only in (c) does H₂O₂ take electrons. It oxidizes I⁻ to I₂ in acidic medium and is itself reduced to water. The answer is (c).

The idea to keep. H₂O₂ is an oxidant when it turns into H₂O (O goes -1 to -2) and a reductant when it releases O₂ (O goes -1 to 0). Look at its product first.

Answer from the NTA final answer key. Solution by PrepWiser.