The diameter of an oxygen molecule is $2.94 \times 10^{-10} \ m$. The van der Waals gas constant '$b$' in $m^3/mol$ is:

The mean free path of gas molecules depends on $(d =$ molecular diameter$)$

Two gases-argon (atomic radius $0.07 \; nm$,atomic weight $40$) and xenon (atomic radius $0.1 \; nm$,atomic weight $140$) have the same number density and are at the same temperature. The ratio of their respective mean free times is closest to:

$A$ real gas behaves like an ideal gas if its

How does the mean free path of a gas depend on temperature?

Calculate the value of mean free path $(\lambda)$ for oxygen molecules at temperature $27^{\circ} C$ and pressure $1.01 \times 10^{5} Pa$. Assume the molecular diameter $d = 0.3 nm$ and the gas is ideal. Given Boltzmann constant $k = 1.38 \times 10^{-23} J K^{-1}$. (Result in $nm$)