In the absence of intermolecular forces of attraction,the observed pressure $P$ will be

What is the effect of a decrease in the number of molecules per unit volume on the mean free path?

In the van der Waals equation $\left( P + \frac{a}{V^2} \right)(V - b) = RT$,what do $a$ and $b$ represent?

The mean free path $\ell$ for a gas molecule depends upon the diameter $d$ of the molecule as:

We have $0.5 \, g$ of hydrogen gas in a cubic chamber of size $3 \, cm$ kept at $NTP$. The gas in the chamber is compressed keeping the temperature constant until a final pressure of $100 \, atm$ is reached. Is one justified in assuming the ideal gas law in the final state? (Hydrogen molecules can be considered as spheres of radius $1 \, \mathring{A}$).

The value of critical temperature in terms of Vander Waals constants $a$ and $b$ is