If the volume of the gas containing $n$ number of molecules is $V,$ then the pressure will decrease due to the force of intermolecular attraction in the proportion:

Consider an ideal gas confined in an isolated closed chamber. As the gas undergoes an adiabatic expansion,the average time of collision between molecules increases as $V^q$,where $V$ is the volume of the gas. The value of $q$ is $\left( \gamma = \frac{C_P}{C_V} \right)$.

An ideal gas in a closed container is slowly heated. As its temperature increases,which of the following statements are true?
$(A)$ The mean free path of the molecules decreases.
$(B)$ The mean collision time between the molecules decreases.
$(C)$ The mean free path remains unchanged.
$(D)$ The mean collision time remains unchanged.

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

Estimate the mean free path and collision frequency of a nitrogen molecule in a cylinder containing nitrogen at $2.0 \; atm$ and temperature $17\,^{\circ} C$. Take the radius of a nitrogen molecule to be roughly $1.0 \; \mathring{A}$. Compare the collision time with the time the molecule moves freely between two successive collisions (Molecular mass of $N_{2} = 28.0 \; u$).

The mean free path of molecules of a gas (radius $r$) is inversely proportional to