Assertion : 1 mole of `H_2` and `O_(2)` each occupy 22.4 L at standard temperature and pressure.
Reason : Molar volume for all gases at the standard temperature and pressure has the same value.

Options

A. If both assertion and reason are true and reason is the correct explanation of assertion.
B. If both assertion and reason are true but reason is not the correct explanation of assertion.
C. If assertion is true but reason is false.
D. If both assertion and reason are false.

Answer

To analyze the assertion and reason provided in the question, we will break down the concepts involved step by step.

### Step 1: Understanding the Assertion
The assertion states that 1 mole of \( H_2 \) (hydrogen gas) and 1 mole of \( O_2 \) (oxygen gas) each occupy 22.4 liters at standard temperature and pressure (STP).

**Explanation**:
At STP, which is defined as a temperature of 0 degrees Celsius (273.15 K) and a pressure of 1 atmosphere (atm), one mole of any ideal gas occupies a volume of 22.4 liters. Thus, it is correct to say that both \( H_2 \) and \( O_2 \) will occupy 22.4 liters when measured under these conditions.

### Step 2: Understanding the Reason
The reason states that the molar volume for all gases at standard temperature and pressure has the same value.

**Explanation**:
This statement is also true. According to Avogadro's law, equal volumes of gases at the same temperature and pressure contain an equal number of molecules. Therefore, regardless of the type of gas, 1 mole of any gas occupies the same volume (22.4 liters) at STP.

### Step 3: Conclusion
Both the assertion and the reason are true, and the reason correctly explains why the assertion is true.

### Final Answer
- **Assertion**: True
- **Reason**: True
- **Conclusion**: The reason supports the assertion.