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JEE Main 2023 · 24 Jan · Shift 2

JEE Main 2023 Chemistry question on Hydrogen and s-Block Elements

In which of the following reactions the hydrogen peroxide acts as a reducing agent?
  1. A.
    HOCl+H2O2→H3O++Cl−+O2\text{HOCl} + \text{H}_2\text{O}_2 \rightarrow \text{H}_3\text{O}^+ + \text{Cl}^- + \text{O}_2
  2. B.
    Mn2++H2O2→Mn4++2OH−\text{Mn}^{2+} + \text{H}_2\text{O}_2 \rightarrow \text{Mn}^{4+} + 2\text{OH}^-
  3. C.
    2Fe2++H2O2→2Fe3++2OH−2\text{Fe}^{2+} + \text{H}_2\text{O}_2 \rightarrow 2\text{Fe}^{3+} + 2\text{OH}^-
  4. D.
    PbS+4H2O2→PbSO4+4H2O\text{PbS} + 4\text{H}_2\text{O}_2 \rightarrow \text{PbSO}_4 + 4\text{H}_2\text{O}
Show answer and solution

Correct option: A

Solution

In HOCl + H₂O₂, the oxygen in H₂O₂ starts at -1 oxidation state and is oxidized to 0 in O₂, meaning H₂O₂ loses electrons and acts as the reducing agent. Simultaneously, Cl in HOCl goes from +1 to -1 (Cl⁻), so HOCl is the oxidizing agent. In all other options, H₂O₂ oxidizes the other species (Fe²⁺→Fe³⁺, Mn²⁺→Mn⁴⁺, S²⁻→S⁶⁺) while its own oxygen is reduced from -1 to -2, making H₂O₂ the oxidizing agent there.

[JEE Main 2023 · 24 Jan · Shift 2]

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