When a large bubble rises from the bottom of a lake to the surface, its radius doubles. The atmospheric pressure is equal to that of a column of water of height H. The depth of the lake is:

1. H

2. 2H

3. 7H

4. 8H

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:

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

A gas at pressure ${\mathrm{P}}_0$ is contained in a vessel. If the masses of all the molecules are halved and their speeds doubled, the resulting pressure would be:

1. $4{\mathrm{P}}_0$

2. $2{\mathrm{P}}_0$

3. ${\mathrm{P}}_0$

4. $\frac{{\mathrm{P}}_0}{2}$

If the pressure of a gas is doubled, then the average kinetic energy per unit volume of the gas will be:

The translational kinetic energy of n moles of a diatomic gas at absolute temperature T is given by:
1. $\frac{5}{2}nRT$
2. $\frac{3}{2}nRT$
3. $\mathit{5}nRT$
4. $\frac{7}{2}nRT$

Two isotherms are drawn at temperatures ${\mathrm{T}}_1$ $\mathrm{and}$ ${\mathrm{T}}_2$ as shown. The ratio of mean speed  at ${\mathrm{T}}_1$ $\mathrm{and}$ ${\mathrm{T}}_2$ is:
  

The translational kinetic energy of oxygen molecules at room temperature is 60 J. Their rotational kinetic energy will be?

1. 40 J

2. 60 J

3. 50 J

4. 20 J

When the gas in an open container is heated, the mean free path:

The change in the internal energy of an ideal gas does not depend on?