# Why are van der Waals' forces between gas molecules strong near its critical temperature?

My textbook says

…easily liquefiable gases i.e. with higher critical temperatures are readily adsorbed as van der Waals' forces are stronger near the critical temperatures.

What I do understand is that at a temperature higher than the critical temperature $$(T_\mathrm c)$$ the gas molecules have higher kinetic energy which is why they're unable to form strong bonds.

But, what if the temperature is lower than the critical temperature? Or is my reasoning incorrect?

• You're missing the point. I'm pretty sure this text was about adsorption in specific, rather high temp. and in such temp. when the critical is higher then adsorption stronger. I wonder why an issue stemming from such misunderstanding, got 4 upvotes already. – Mithoron May 2 at 22:43