Diatomic molecules like hydrogen have energies due to both translational as well as rotational motion. The equation in kinetic theory \(PV = \dfrac{2}{3}E,\)$$ \(E\) is:

1.	the total energy per unit volume.
2.	only the translational part of energy because rotational energy is very small compared to translational energy.
3.	only the translational part of the energy because during collisions with the wall, pressure relates to change in linear momentum.
4.	the translational part of the energy because rotational energies of molecules can be of either sign and its average over all the molecules is zero.

The mean free path \(l\) for a gas molecule depends upon the diameter, \(d\) of the molecule as:

What is the graph between volume and temperature in Charle's law?
1. An ellipse
2. A circle
3. A straight line
4. A parabola

Match Column-I and Column-II and choose the correct match from the given choices.

An increase in the temperature of a gas-filled in a container would lead to:

The mean free path for a gas, with molecular diameter \(d\) and number density \(n,\) can be expressed as:
1. \( \dfrac{1}{\sqrt{2} n \pi {d}^2} \)

2. \( \dfrac{1}{\sqrt{2} n^2 \pi {d}^2} \)

3. \(\dfrac{1}{\sqrt{2} n^2 \pi^2 d^2} \)

4. \( \dfrac{1}{\sqrt{2} n \pi {d}}\)

Without change in temperature, a gas is forced in a smaller volume. Its pressure increases because its molecules:

If at a pressure of \(10^6\) dyne/cm², one gram of nitrogen occupies \(2\times10^4\) c.c. volume, then the average energy of a nitrogen molecule in erg is: