Question

$H_2$ gas is adsorbed on activated charcoal to a very little extent in comparison to easily liquefiable gases due to ____________.

• A. very strong van der Waal’s interaction.
• B. very high critical temperature.
• C. very weak van der Waals forces.
• D. very low critical temperature.

Answer 1

Answer: (C), (D)

very low critical temperature.

Due to the smaller size , the $H_2$ molecule has lesser intermolecular forces of attraction. So, $H_2$ gas has weaker van der Waals force of attraction.

Therefore, $\left(A\right)$ is wrong and $\left(B\right)$ is correct.

Higher the value of critical temperature, more easily a gas will be liquefiable and will be adsorbed readily.

Since $H_2$ gas has lower value of critical temperature, it cannot be easily adsorbed on activated charcoal.

Therefore, $\left(C\right)$ is correct but $\left(D\right)$ is wrong.