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

The correct option is 5.6 m³.

Step-by-step Explanation:

When the intermolecular forces of attraction between water molecules vanish completely, water no longer exists in its liquid state. Instead, the molecules behave like an ideal gas. Therefore, we can apply the ideal gas laws and properties to determine the volume occupied by the water molecules at standard temperature and pressure (STP).

First, we find the molar mass of water ($H_{2}O$):
$M=18\text{g/mol}=18\times {10}^{-3}\text{kg/mol}$

The given mass of water is:
$m=4.5\text{kg}$

Now, we calculate the number of moles ($n$) of water molecules:
$n=\frac{m}{M}$
Substitute the values into the formula:
$n=\frac{4.5}{18\times {10}^{-3}}=250\text{moles}$

At standard temperature and pressure (STP), 1 mole of any ideal gas occupies a volume of:
$V_0=22.4\text{litres}=22.4\times {10}^{-3}{\text{m}}^3$

Therefore, the total volume ($V$) occupied by 250 moles of water molecules under these conditions is:
$V=n\times V_0$
Substitute the values to find the final volume:
$V=250\times 22.4\times {10}^{-3}{\text{m}}^3$
$V=5.6{\text{m}}^3$