Given van der Waals constant a for NH_{3},H_{ | vedclass

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(A) The ease of liquefaction of a gas is directly proportional to the magnitude of the van der Waals constant $a$,which represents the intermolecular

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$NH_{3}$

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(A) The ease of liquefaction of a gas is directly proportional to the magnitude of the van der Waals constant $a$,which represents the intermolecular forces of attraction.Greater value of $a$ implies stronger intermolecular forces,leading to a higher critical temperature $(T_{C})$.Comparing the given values: $a(NH_{3}) = 4.17$,$a(H_{2}) = 0.244$,$a(O_{2}) = 1.36$,and $a(CO_{2}) = 3.59$.Since $NH_{3}$ has the highest value of $a$ $(4.17)$,it has the strongest intermolecular forces and is the most easily liquefied gas among the given options.

Given van der Waals constant $a$ for $NH_{3}$,$H_{2}$,$O_{2}$ and $CO_{2}$ are respectively $4.17$,$0.244$,$1.36$ and $3.59$,which one of the following gases is most easily liquefied?

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