Question

The reaction of aqueous KMnO₄ with H₂O₂ in acidic conditions gives:

• A. Mn²⁺ and O₂
• B. Mn²⁺ and O₃
• C. Mn⁴⁺ and MnO₂
• D. Mn⁴⁺ and O₂

Answer 1

The Correct Option is A

 The reaction between aqueous KMnO₄ (Potassium permanganate) and H₂O₂ (Hydrogen peroxide) in acidic conditions is a common redox reaction. In this reaction, KMnO₄ acts as an oxidizing agent, and H₂O₂ acts as a reducing agent.

The balanced chemical equation for the reaction is:

\(2 \text{KMnO}_4 + 3 \text{H}_2\text{SO}_4 + 5 \text{H}_2\text{O}_2 \rightarrow 2 \text{MnSO}_4 + 5 \text{O}_2 + 8 \text{H}_2\text{O} + K_2\text{SO}_4\)

Let's break down the reaction into half-reactions to understand the changes in oxidation states:

• Reduction Half-Reaction: Mn in KMnO₄ is reduced from +7 in MnO₄^- to +2 in Mn²⁺:
• Oxidation Half-Reaction: O in H₂O₂ is oxidized from -1 in H₂O₂ to 0 in O₂:

This reaction results in the formation of Mn²⁺ ions and the liberation of O₂ gas.

Therefore, the correct answer is: Mn²⁺ and O₂.

To conclude, in the redox reaction of KMnO₄ and H₂O₂ under acidic conditions, Mn²⁺ ions are produced, and O₂ gas is released, which matches the correct option given.