Van Der Waals Equation

The van der Waals constant $a$ represents the magnitude of intermolecular attractive forces. It increases with molecular size, molecular mass, and the presence of hydrogen bonding. Let us analyze the given gases:

Argon (Ar): Being a noble gas, Ar has the weakest intermolecular forces and the lowest value of $a$ .
Methane ( $%5Ctext%7BCH%7D_4$ ): $%5Ctext%7BCH%7D_4$ has stronger London dispersion forces than Ar due to its larger molecular size.
Water ( $%5Ctext%7BH%7D_2%5Ctext%7BO%7D$ ): $%5Ctext%7BH%7D_2%5Ctext%7BO%7D$ has significant hydrogen bonding, increasing its $a$ value further.
Benzene ( $%5Ctext%7BC%7D_6%5Ctext%7BH%7D_6$ ): $%5Ctext%7BC%7D_6%5Ctext%7BH%7D_6$ is a large aromatic molecule with strong dispersion forces, giving it the highest $a$ value among the given gases.

Thus, the increasing order of $a$ is:

$Ar%20(A)%20%3C%20CH_4%20(B)%20%3C%20H_2O%20(C)%20%3C%20C_6H_6%20(D)%20.$

High-Yield Trend

Chapter Questions
1 MCQs

Official Solution

Van Der Waals Equation

High-Yield Trend

Chapter Questions 1 MCQs

Official Solution

Chapter Questions
1 MCQs