For the following gases,the values of 'a' (va | vedclass

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(B) The van der Waals constant $'a'$ is a measure of the magnitude of intermolecular attractive forces between gas molecules.Greater the value of $'a'

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$N_2$

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(B) The van der Waals constant $'a'$ is a measure of the magnitude of intermolecular attractive forces between gas molecules.Greater the value of $'a'$,stronger are the intermolecular forces,and easier it is to liquefy the gas.Conversely,a smaller value of $'a'$ indicates weaker intermolecular forces,making the gas more difficult to liquefy.Comparing the given values: $CH_4 (2.25) > CO (1.46) > O_2 (1.36) > N_2 (1.35)$.Since $N_2$ has the smallest value of $'a'$ $(1.35)$,it has the weakest intermolecular forces and will be the most difficult to liquefy.

For the following gases,the values of $'a'$ (van der Waals constant) are given in parentheses: $CH_4 (2.25)$,$N_2 (1.35)$,$O_2 (1.36)$,and $CO (1.46)$. Which gas will be the most difficult to liquefy?

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