The decomposition of `KClO_(3)` to KCl and `O_(2)` on heating is an example of :

Options

A. Intermolecular redox change
B. Intermolecular redox change
C. Disproportionation or auto redox change
D. None

Answer

To solve the question regarding the decomposition of KClO₃ to KCl and O₂ on heating, we can follow these steps:

### Step 1: Write the balanced chemical equation for the reaction.
The decomposition reaction can be represented as:
\[ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 \]

### Step 2: Determine the oxidation states of the elements involved.
- In KClO₃:
- K (Potassium) has an oxidation state of +1.
- Cl (Chlorine) has an oxidation state of +5.
- O (Oxygen) has an oxidation state of -2.

- In KCl:
- K (Potassium) remains +1.
- Cl (Chlorine) has an oxidation state of -1.

- In O₂:
- O (Oxygen) has an oxidation state of 0.

### Step 3: Identify the changes in oxidation states.
- Chlorine changes from +5 in KClO₃ to -1 in KCl, indicating a reduction (gain of electrons).
- Oxygen changes from -2 in KClO₃ to 0 in O₂, indicating an oxidation (loss of electrons).

### Step 4: Classify the reaction.
Since both oxidation and reduction are occurring in this reaction, it is classified as a redox reaction. Furthermore, since the same compound (KClO₃) contains elements that undergo both oxidation and reduction, this is an example of an intramolecular redox reaction.

### Conclusion:
The decomposition of KClO₃ to KCl and O₂ on heating is an example of an **intramolecular redox reaction**.

---