If the intermolecules forces vanish away, the volume occupied by the molecules contained in `4.5 kg` water at stantard temperature and pressure will be given by

Options

A. `5.6 m^(3)`
B. `4.5m^(3)`
C. `11.2` litre
D. `11.2 m^(3)`

Explanation

To solve the problem of finding the volume occupied by 4.5 kg of water when intermolecular forces vanish, we will follow these steps:

### Step-by-Step Solution

1. **Identify the Given Data**:
- Mass of water (m) = 4.5 kg
- Molar mass of water (H₂O) = 18 g/mol = 0.018 kg/mol
- Standard pressure (P) = 1 atm = 101325 Pa
- Standard temperature (T) = 273 K

2. **Calculate the Number of Moles (n)**:
The number of moles can be calculated using the formula:
\[ n = \frac{m}{M} \]
where \( M \) is the molar mass.
\[ n = \frac{4.5 \text{ kg}}{0.018 \text{ kg/mol}} = 250 \text{ moles} \]

3. **Use the Ideal Gas Equation**:
The ideal gas equation is given by:
\[ PV = nRT \]
Rearranging to find the volume (V):
\[ V = \frac{nRT}{P} \]

4. **Substitute the Values**:
- \( R \) (universal gas constant) = 8.314 J/(mol·K)
- Substitute \( n = 250 \text{ moles} \), \( R = 8.314 \text{ J/(mol·K)} \), \( T = 273 \text{ K} \), and \( P = 101325 \text{ Pa} \):
\[ V = \frac{250 \times 8.314 \times 273}{101325} \]

5. **Calculate the Volume**:
- Performing the calculation:
\[ V = \frac{250 \times 8.314 \times 273}{101325} \approx 5.6 \text{ m}^3 \]

6. **Conclusion**:
The volume occupied by 4.5 kg of water at standard temperature and pressure, when intermolecular forces vanish, is approximately **5.6 m³**.