Asserton :- `KClO_(3)rarrKClO_(4)+KCl`
This is a disporportionation type reaction.
Reason :- The reaction in which one substance oxidise or reduce is known as disproportionation reaction.

Options

A. If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
B. If both Assertion & Reason are True but Reason is not a correct explanation of the Assertion.
C. If Assertion is True but the Reason is False.
D. If both Assertion & Reason are False.

Answer

To solve the question regarding the assertion and reason about the reaction \( KClO_3 \rightarrow KClO_4 + KCl \), we will analyze the reaction step by step.

### Step 1: Identify the Assertion and Reason
- **Assertion**: The reaction \( KClO_3 \rightarrow KClO_4 + KCl \) is a disproportionation type reaction.
- **Reason**: A reaction in which one substance oxidizes and reduces itself is known as a disproportionation reaction.

### Step 2: Understand Disproportionation Reactions
A disproportionation reaction is a specific type of redox reaction where a single substance is both oxidized and reduced, resulting in two different products.

### Step 3: Determine the Oxidation States
To confirm whether the reaction is a disproportionation reaction, we need to find the oxidation states of chlorine in the reactant and products.

1. **In \( KClO_3 \)**:
- Potassium (K) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- Let the oxidation state of Cl be \( x \).
- The equation for the oxidation state is:
\[ +1 + x + 3(-2) = 0 \implies +1 + x - 6 = 0 \implies x = +5 \]
- Therefore, the oxidation state of Cl in \( KClO_3 \) is +5.

2. **In \( KClO_4 \)**:
- Potassium (K) has an oxidation state of +1.
- Let the oxidation state of Cl be \( y \).
- The equation for the oxidation state is:
\[ +1 + y + 4(-2) = 0 \implies +1 + y - 8 = 0 \implies y = +7 \]
- Therefore, the oxidation state of Cl in \( KClO_4 \) is +7.

3. **In \( KCl \)**:
- Potassium (K) has an oxidation state of +1.
- Let the oxidation state of Cl be \( z \).
- The equation for the oxidation state is:
\[ +1 + z = 0 \implies z = -1 \]
- Therefore, the oxidation state of Cl in \( KCl \) is -1.

### Step 4: Analyze the Changes in Oxidation States
- In \( KClO_3 \), Cl is at +5.
- In \( KClO_4 \), Cl is at +7 (oxidation).
- In \( KCl \), Cl is at -1 (reduction).

This shows that the same element (Cl) is undergoing both oxidation (from +5 to +7) and reduction (from +5 to -1).

### Step 5: Conclusion
Since chlorine in \( KClO_3 \) is both oxidized and reduced in the reaction, we conclude that the assertion is correct: the reaction is indeed a disproportionation reaction. However, the reason provided is not entirely accurate because it does not specify that the same substance must undergo both oxidation and reduction.

### Final Answer
- **Assertion**: True
- **Reason**: False
- Therefore, the correct option is **C**: Assertion is true, but the reason is false.