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(B) The constant $ 'a'$ in the van der Waals equation represents the magnitude of intermolecular attractive forces. Greater the value of $ 'a'$,strong

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$N_2$

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(B) The constant $ 'a'$ in the van der Waals equation represents the magnitude of intermolecular attractive forces. Greater the value of $ 'a'$,stronger are the intermolecular forces,which makes the gas easier to liquefy. Conversely,a smaller value of $ 'a'$ indicates weaker intermolecular forces,making the gas more difficult to liquefy. Comparing the given values: $N_2 (1.35) Since $N_2$ has the lowest value of $ 'a'$,it has the weakest intermolecular forces and will be the most difficult to liquefy.

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

Consider the following gases and their corresponding $ 'a'$ values given in parentheses: $CH_4 (2.25), N_2 (1.35), O_2 (1.36)$,and $CO (1.46)$. Which of these gases will be the most difficult to liquefy?

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