`KMnO_4` on heating gives

Options

A. `K_2MnO_4, Mn_2O_3`
B. `K_2MnO_4, MnO, O_2`
C. `K_2MnO_4, MnO_2, O_2`
D. `K_2MnO_4, MnO_2, O_3`

Explanation

To solve the question regarding the thermal decomposition of potassium permanganate (KMnO₄) upon heating, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Compound**:
- Potassium permanganate (KMnO₄) is a strong oxidizing agent and is known for its deep purple color.

2. **Heating KMnO₄**:
- When KMnO₄ is heated, it undergoes thermal decomposition. The reaction typically occurs at around 513 K (or 240 °C).

3. **Products of Decomposition**:
- The decomposition of KMnO₄ produces potassium manganate (K₂MnO₄), manganese dioxide (MnO₂), and oxygen gas (O₂).

4. **Writing the Balanced Equation**:
- The balanced chemical equation for the decomposition of KMnO₄ can be written as:
\[ 2 \, KMnO_4 \, (s) \rightarrow K_2MnO_4 \, (s) + MnO_2 \, (s) + O_2 \, (g) \]
- Here, we have 2 moles of KMnO₄ yielding 1 mole of K₂MnO₄, 1 mole of MnO₂, and 1 mole of O₂.

5. **Oxidation States**:
- In KMnO₄, manganese (Mn) has an oxidation state of +7.
- In K₂MnO₄, manganese has an oxidation state of +6, and in MnO₂, it has an oxidation state of +4.
- This indicates that manganese is reduced during the reaction.

6. **Conclusion**:
- Therefore, upon heating KMnO₄, we get K₂MnO₄, MnO₂, and O₂ as products.

### Final Answer:
Upon heating potassium permanganate (KMnO₄) at 513 K, it decomposes to form potassium manganate (K₂MnO₄), manganese dioxide (MnO₂), and oxygen gas (O₂).

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