The pressure of a van der Waals gas is less than the pressure of an ideal gas because of

$1 \ mol$ of a real gas is kept at a high pressure of $100 \ bar$ at $300 \ K$. If the van der Waals constant $b$ is $0.005 \ L \ mol^{-1}$,what are the values of the compressibility factor $Z$ of the gas and the $\%$ deviation of volume from ideality?

$Z$	$\%$ Deviation

Between $NH_3$ and $N_2$,which one has a higher value of $(i) \ a$ and which one has a higher value of $(ii) \ b$? (Where $a$ and $b$ are van der Waals constants.)

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?

The temperature at which the second virial coefficient of a real gas is zero is called:

Under what conditions do real gases behave as ideal gases?