Gas deviates from ideal gas nature because molecules

Assertion : Greater the value of van der Waal's constant $a$,greater is the liquefaction of gas.
Reason : $a$ indirectly measures the magnitude of attractive forces between the molecules.

At $300 \, K$ temperature and $40 \, atm$ pressure,if one mole of $CO_2$ occupies $0.4 \, L$,then it is:

The compressibility factor $(Z)$ of a gas is greater than unity at $1 \, atm$ and $273 \, K$. Therefore:

The correct option regarding a container containing $1 \, mol$ of a gas in a $22.4 \, L$ container at $273 \, K$ is:

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?