STATEMENT -1 : 18 ml of `H_(2)O` and 18 ml of `CO_(2)` at 277 K have same no. of moles.
and
STATEMENT -2 : Density of `H_(2)O` is more than `CO_(2)`.

Options

A. Statement -1 is True, Statement -2 is True, Statement -2 is a correct explanation for Statmenet -1.
B. Statement -1 is True, Statement -2 is True, Statement-2 is NOT a correct explanation for Statement -9
C. Statement -1 is True, Statement -2 is False
D. Statement -1 is False, Statmenet -2 is True

Answer

To solve the problem, we need to analyze both statements provided in the question.

### Step 1: Analyze Statement 1
**Statement 1:** 18 ml of H₂O and 18 ml of CO₂ at 277 K have the same number of moles.

To determine if this statement is true or false, we need to calculate the number of moles of both substances using the formula:

\[ \text{Number of moles} = \frac{\text{Mass}}{\text{Molar mass}} \]

1. **Calculate the mass of H₂O:**
- Density of H₂O = 1 g/ml (approximately)
- Volume of H₂O = 18 ml
- Mass of H₂O = Density × Volume = 1 g/ml × 18 ml = 18 g

2. **Calculate the number of moles of H₂O:**
- Molar mass of H₂O = 18 g/mol
- Number of moles of H₂O = \(\frac{18 \text{ g}}{18 \text{ g/mol}} = 1 \text{ mole}\)

3. **Calculate the mass of CO₂:**
- Density of CO₂ (at room temperature) ≈ 1.98 g/L = 0.00198 g/ml
- Volume of CO₂ = 18 ml
- Mass of CO₂ = Density × Volume = 0.00198 g/ml × 18 ml = 0.03564 g

4. **Calculate the number of moles of CO₂:**
- Molar mass of CO₂ = 44 g/mol
- Number of moles of CO₂ = \(\frac{0.03564 \text{ g}}{44 \text{ g/mol}} ≈ 0.00081 \text{ moles}\)

Since 1 mole of H₂O is much greater than 0.00081 moles of CO₂, **Statement 1 is false.**

### Step 2: Analyze Statement 2
**Statement 2:** The density of H₂O is more than CO₂.

At room temperature:
- Density of H₂O ≈ 1 g/ml (liquid)
- Density of CO₂ ≈ 0.00198 g/ml (gas)

Since 1 g/ml (H₂O) is greater than 0.00198 g/ml (CO₂), **Statement 2 is true.**

### Conclusion
- **Statement 1:** False
- **Statement 2:** True

Thus, the correct answer is that Statement 1 is false and Statement 2 is true.

### Final Answer
- Statement 1 is false.
- Statement 2 is true.