Direction this section contains Assertion and Reason type question each question has 4 choice (1)(2)(3)(4) out of only which one is correct
(1) Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion (2)Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion (3)Assertion is correct but Reason is incorrect (4) Both Assertion and Reason are incorrect
Assertion(A):The decomposition of hydrogen peroxide to form water and oxygen peroxide to form water and oxygen is an example of disproportional reaction
Reason(R):The oxygen of peroxide is in -1 oxidation state and it is converted to zeto oxidation state in `O_2` and -2 oxidation state in `H_2O`

Options

A. Both assertion and reason are correct and reason is the correct explanation of the assertion
B. Both assertion and reason are correct but reason is not the correct explantion
C. Assertion is correct but reason is incorrect
D. Both assertion and reason are incorrect

Answer

To solve the assertion and reason type question, we need to analyze both the assertion and the reason provided.

### Step-by-Step Solution:

1. **Understanding the Assertion:**
- The assertion states that the decomposition of hydrogen peroxide (H₂O₂) to form water (H₂O) and oxygen (O₂) is an example of a disproportionation reaction.
- A disproportionation reaction is a specific type of redox reaction where a single substance is both oxidized and reduced.

2. **Analyzing the Reaction:**
- The decomposition reaction can be written as:
\[ 2 H_2O_2 \rightarrow 2 H_2O + O_2 \]
- In this reaction, we need to determine the oxidation states of the oxygen in H₂O₂, H₂O, and O₂.

3. **Determining Oxidation States:**
- In hydrogen peroxide (H₂O₂), the oxidation state of oxygen is -1.
- In water (H₂O), the oxidation state of oxygen is -2.
- In molecular oxygen (O₂), the oxidation state of oxygen is 0.

4. **Identifying Oxidation and Reduction:**
- The oxygen in H₂O₂ goes from -1 (in H₂O₂) to 0 (in O₂), indicating that it is oxidized.
- The oxygen in H₂O₂ also goes from -1 (in H₂O₂) to -2 (in H₂O), indicating that it is reduced.
- Since one species (oxygen) is both oxidized and reduced, this confirms that the reaction is indeed a disproportionation reaction.

5. **Understanding the Reason:**
- The reason states that the oxygen of peroxide is in -1 oxidation state and it is converted to 0 oxidation state in O₂ and -2 oxidation state in H₂O.
- This statement accurately describes the changes in oxidation states during the reaction.

6. **Conclusion:**
- Both the assertion and the reason are correct.
- However, the reason does not provide a complete explanation of why the reaction is classified as a disproportionation reaction; it merely states the changes in oxidation states without defining disproportionation.

### Final Answer:
The correct option is (2): Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion.