`KMnO_(4)` on heating to red hot gives

Options

A. `K_(2)MnO_(4)+ MnO_(2)+O_(2)`
B. `K_(2)MnO_(3) + MnO_(2)+ O_(2)`
C. `K_(2)O+ MnO_(2)+ O_(2)`
D. None of these

Answer

To determine the products formed when potassium permanganate (KMnO₄) is heated to red hot temperatures, we can follow these steps:

### Step 1: Understand the Reaction Conditions
When KMnO₄ is heated to a temperature greater than 500 °C, it undergoes thermal decomposition.

**Hint**: Remember that heating often leads to decomposition reactions in compounds.

### Step 2: Write the Decomposition Reaction
The decomposition of KMnO₄ can be represented by the following balanced chemical equation:
\[ 2 \text{KMnO}_4 \rightarrow \text{K}_2\text{MnO}_4 + \text{MnO}_2 + \text{O}_2 \]

**Hint**: Look for the products formed from the breakdown of KMnO₄.

### Step 3: Identify the Products
From the balanced equation, we can identify the products:
- Potassium manganate (K₂MnO₄)
- Manganese dioxide (MnO₂)
- Oxygen gas (O₂)

**Hint**: Ensure you account for all products formed in the reaction.

### Step 4: Conclusion
Thus, when KMnO₄ is heated to red hot temperatures, it decomposes to form K₂MnO₄, MnO₂, and O₂.

**Final Answer**: The products of the reaction are K₂MnO₄, MnO₂, and O₂.