The reaction of aqueous `KMnO_4` with `H_2O_2` gives

Options

A. `Mn^(4+)` and `O_2`
B. `Mn^(2+)` and `O_2`
C. `Mn^(2+)` and `O_3`
D. `Mn^(4+)` and `MnO_2`

Explanation

To solve the question regarding the reaction of aqueous KMnO4 with H2O2, we will analyze the oxidation states of the elements involved and write the balanced chemical equation for the reaction.

### Step-by-Step Solution:

1. **Identify the Reactants**: The reactants are potassium permanganate (KMnO4) and hydrogen peroxide (H2O2).

2. **Determine the Oxidation States**:
- In KMnO4, the oxidation state of manganese (Mn) is +7. This can be calculated as follows:
- Potassium (K) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2. Since there are 4 oxygen atoms, the total contribution from oxygen is -8.
- Therefore, the equation becomes:
\[ +1 + x - 8 = 0 \implies x = +7 \]
- In H2O2, the oxidation state of oxygen is -1. This can be calculated as follows:
- Each hydrogen (H) has an oxidation state of +1. With 2 hydrogen atoms, the total contribution is +2.
- Let x be the oxidation state of oxygen:
\[ +2 + 2x = 0 \implies 2x = -2 \implies x = -1 \]

3. **Identify the Changes in Oxidation States**:
- KMnO4 (Mn changes from +7 to +2) is reduced.
- H2O2 (O changes from -1 to 0) is oxidized.

4. **Write the Balanced Chemical Equation**:
- The balanced equation for the reaction is:
\[ \text{MnO}_4^- + 5 \text{H}_2\text{O}_2 + 6 \text{H}^+ \rightarrow 2 \text{Mn}^{2+} + 5 \text{O}_2 + 8 \text{H}_2\text{O} \]

5. **Conclusion**: The products of the reaction between KMnO4 and H2O2 in acidic medium are manganese ions (Mn²⁺), oxygen gas (O₂), and water (H₂O).

### Final Answer:
The reaction of aqueous KMnO4 with H2O2 gives manganese ions (Mn²⁺), oxygen gas (O₂), and water (H₂O).

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