The reaction of aqueous `KMnO_(4)` with `H_(2)O_(2)` i acidic conditions 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 potassium permanganate (KMnO₄) with hydrogen peroxide (H₂O₂) under acidic conditions, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reactants and Conditions**:
- The reactants are potassium permanganate (KMnO₄) and hydrogen peroxide (H₂O₂).
- The reaction occurs in acidic conditions, typically using sulfuric acid (H₂SO₄) as the acid.

2. **Write the Balanced Chemical Equation**:
- The balanced equation for the reaction can be written as follows:
\[ 2 \text{KMnO}_4 + 5 \text{H}_2\text{O}_2 + 6 \text{H}^+ \rightarrow 2 \text{Mn}^{2+} + 5 \text{O}_2 + 8 \text{H}_2\text{O} \]
- Here, potassium sulfate (K₂SO₄) is also formed, but for the purpose of this question, we focus on manganese and oxygen products.

3. **Determine the Oxidation States**:
- In KMnO₄, manganese (Mn) has an oxidation state of +7.
- In H₂O₂, the oxidation state of oxygen is -1.
- In the products, Mn is reduced to +2 and oxygen is released as O₂ (oxidation state 0).

4. **Identify the Changes in Oxidation States**:
- Mn changes from +7 in KMnO₄ to +2 in Mn²⁺, indicating a reduction.
- Oxygen in H₂O₂ changes from -1 to 0, indicating oxidation.

5. **Conclusion**:
- The products of the reaction are manganese ions (Mn²⁺) and molecular oxygen (O₂).
- Therefore, the correct answer to the question is **Mn²⁺ and O₂**.

### Final Answer:
The reaction of aqueous KMnO₄ with H₂O₂ in acidic conditions gives **Mn²⁺ and O₂**.

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