Assertion : No of moles of H2 in 0.224 L of hydrogen is 0.01 mole.
Reason : 22.4 L of `H_(2)` at STP contain `6.023 xx 10^(23)` moles.

Options

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

Answer

To solve the assertion and reason question, we will analyze both the assertion and the reason step by step.

### Step-by-Step Solution:

1. **Understanding the Assertion:**
- The assertion states that the number of moles of H2 in 0.224 L of hydrogen is 0.01 mole.
- At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 L.

2. **Calculating Moles from Volume:**
- To find the number of moles in 0.224 L of H2, we can use the formula:
\[ \text{Number of moles} = \frac{\text{Volume of gas (L)}}{\text{Molar volume at STP (L/mol)}} \]
- Substituting the values:
\[ \text{Number of moles} = \frac{0.224 \text{ L}}{22.4 \text{ L/mol}} = 0.01 \text{ moles} \]
- This confirms that the assertion is correct.

3. **Understanding the Reason:**
- The reason states that 22.4 L of H2 at STP contains \(6.023 \times 10^{23}\) molecules.
- We know that 1 mole of any substance contains \(6.023 \times 10^{23}\) entities (Avogadro's number).
- Therefore, 22.4 L of H2 (which is 1 mole) indeed contains \(6.023 \times 10^{23}\) molecules.

4. **Identifying the Error in the Reason:**
- The reason incorrectly states that 22.4 L of H2 contains \(6.023 \times 10^{23}\) moles instead of molecules.
- The correct statement should be that 22.4 L of H2 contains \(6.023 \times 10^{23}\) molecules, not moles.

5. **Conclusion:**
- The assertion is correct, while the reason is incorrect. Therefore, the correct option is that the assertion is true and the reason is false.

### Final Answer:
- Assertion: True
- Reason: False