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(C) The Van der Waals equation for real gases is given by $(P + a(n/V)^2)(V - nb) = nRT$.In this equation,the term $a(n/V)^2$ represents the correctio

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$(n/V)^2$

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(C) The Van der Waals equation for real gases is given by $(P + a(n/V)^2)(V - nb) = nRT$.In this equation,the term $a(n/V)^2$ represents the correction factor for the pressure due to intermolecular attractive forces.Here,$n$ is the number of molecules and $V$ is the volume of the gas.The force of attraction experienced by a molecule at the surface of the gas is proportional to the density of the molecules,which is $(n/V)$.Since the pressure reduction is proportional to the product of the density of molecules hitting the wall and the density of molecules pulling them back,the pressure decrease is proportional to $(n/V) 	imes (n/V) = (n/V)^2$.Therefore,the pressure decreases in the proportion $(n/V)^2$.Thus,option $(C)$ is the correct answer.

If the volume of the gas containing $n$ number of molecules is $V,$ then the pressure will decrease due to the force of intermolecular attraction in the proportion:

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