The pressures of a gas filled in the bulb of a constant volume gas thermometer at temperatures $0°\mathrm{C}$ and $100°\mathrm{C}$ are 27.50 cm and 37.50 cm of Hg respectively. At an unknown temperature, the pressure is 32.45 cm of Hg. The unknown temperature is:

1. $30°\mathrm{C}$

2. $39°\mathrm{C}$

3. $49.5°\mathrm{C}$

4. $29.6°\mathrm{C}$

A graph is plotted by taking pressure along the y-axis and centigrade temperature along the x-axis for an ideal gas at constant volume. The x-intercept of the graph is:

1. $-273.15°\mathrm{C}$

2. $-273.15 \mathrm{K}$

3. $-273°\mathrm{C}$

4. $-273 \mathrm{K}$

Heat is  associated with:

Which one of the following graphs represents the behaviour of an ideal gas?

1. 

2. 

3. 

4. 

A jar has a mixture of hydrogen and oxygen gases in the ratio of 1: 5. The ratio of mean kinetic energies of hydrogen and oxygen molecules is:

1. 1: 16

2. 1: 4

3. 1: 5

4. 1: 1

A vessel contains a mixture of one mole of oxygen and two moles of nitrogen at 300 K. The ratio of the average rotational kinetic energy per O₂ molecule to that per N₂ molecule is:

1. 1: 1

2. 1: 2

3. 2: 1

4. Depends on the moments of inertia of the two molecules

A closed compartment containing gas is moving with some acceleration in horizontal direction. Neglecting effect of gravity, pressure in the compartment is:

1. same everywhere

2. lower in the front

3. lower in the rear side

4. lower in the upper side

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

1. the total energy per unit volume.

2. only the translational part of energy because rotational energy is very small compared to the 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 is average over all the molecules is zero.

When an ideal gas is compressed adiabatically, its temperature rises and thus, the molecules on the average have more kinetic energy than before. The kinetic energy
increases:

1. because of collisions with moving parts of the wall only.

2. because of collisions with the entire wall.

3. because the molecules gets accelerated in their motion inside the volume.

4. because of redistribution of energy amongst the molecules.

Two closed containers of equal volume are filled with air at pressure ${\mathrm{P}}_0$ and temperature ${\mathrm{T}}_0$. Both are connected by a narrow tube. If one of the containers is maintained at temperature ${\mathrm{T}}_0$ and the other at temperature T, then new pressure in the container will be:

1. $\frac{2{\mathrm{P}}_0\mathrm{T}}{\mathrm{T}+{\mathrm{T}}_0}$

2. $\frac{{\mathrm{P}}_0\mathrm{T}}{\mathrm{T}+{\mathrm{T}}_0}$

3. $\frac{{\mathrm{P}}_0\mathrm{T}}{2(\mathrm{T}+{\mathrm{T}}_0)}$

4. $\frac{\mathrm{T}+{\mathrm{T}}_0}{{\mathrm{P}}_0}$