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

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

Under what conditions does a real gas obey the relation $PV = RT$?

$A$ system consists of two types of gas molecules $A$ and $B$ having the same number density $2 \times 10^{25} \, /m^3$. The diameters of $A$ and $B$ are $10 \, \mathring{A}$ and $5 \, \mathring{A}$ respectively. They undergo collisions at room temperature. The ratio of the average distance covered by molecule $A$ to that of $B$ between two successive collisions is $..... \times 10^{-2}$.

Consider an ideal gas at pressure $p$,volume $V$ and temperature $T$. The mean free path for molecules of the gas is $L$. If the radius of gas molecules,as well as pressure,volume and temperature of the gas are doubled,then the mean free path will be

For a gas,$C_{p} - C_{V} = R$ in state $P$ and $C_{p} - C_{V} = 1.10 R$ in state $Q$. If $T_{P}$ and $T_{Q}$ are the temperatures in states $P$ and $Q$ respectively,then which of the following is true?