The density of acetic acid vapor at $300 \mathrm{K}$ and $1 \mathrm{atm}$ is $5 \mathrm{mg} {\mathrm{cm}}^{-3}$. The number of acetic acid molecules in the cluster that is formed in the gas phase is the closest to 

The volume vs. temperature graph of $1$ mole of an ideal gas is given below. The pressure of the gas (in $\mathrm{atm}$) at $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$, respectively, are

In the following compressibility factor $\left(\mathrm{Z}\right)$ vs. pressure graph at $300 \mathrm{K}$, the compressibility of ${\mathrm{CH}}_4$ at pressures $<200 \mathrm{bar}$ deviates from ideal behaviour because:

If ${10}^{-4}{\mathrm{dm}}^3$ of water is introduced into a $1.0 {\mathrm{dm}}^3$ flask at $300 \mathrm{K}$, how many moles of water are in the vapour phase when equilibrium is established? (Given: Vapour pressure of ${\mathrm{H}}_2\mathrm{O}$ at $300 \mathrm{K}$ is $3170 \mathrm{Pa}, \mathrm{R}=8.314 \mathrm{J} {\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$ )

Assertion: Van der Waals equation describes the behaviour of real gases.

Reason: The kinetic theory postulates that negligible volume of gaseous molecules and intermolecular forces of attraction do not stand correct at high pressure and low temperature.