At relatively high pressure,the van der Waals equation reduces to

The values of van der Waals' constant '$a$' for gases $O_2, N_2, NH_3$,and $CH_4$ are $1.360, 1.390, 4.170$,and $2.253 \ L^2 \ atm \ mol^{-2}$ respectively. The gas which can be most easily liquefied is

The van der Waals equation for $CH_4$ at low pressure is:

For a real gas,deviations from ideal gas behavior are maximum at:

Consider the van der Waals constants,$a$ and $b,$ for the following gases.

Gas	$Ar$	$Ne$	$Kr$	$Xe$
$a \ (atm \ dm^6 \ mol^{-2})$	$1.3$	$0.2$	$5.1$	$4.1$
$b \ (10^{-2} \ dm^3 \ mol^{-1})$	$3.2$	$1.7$	$1.0$	$5.0$

Which gas is expected to have the highest critical temperature?

What is the difference in the pressure-volume $(P-V)$ graph (at constant $T$) for a real gas and an ideal gas?