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

The ratio of the average translatory kinetic energy of He gas molecules to ${\mathrm{O}}_2$ gas molecules is:

1. $\frac{25}{21}$

2. $\frac{21}{25}$

3. $\frac{3}{2}$

4. 1

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. $\frac{7}{2}nRT$

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:

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

The average translational kinetic energy of \(O_2\) (molar mass \(32\)) molecules at a particular temperature is \(0.048~\text{eV}\). The translational kinetic energy of \(N_2\) (molar mass \(28\)) molecules in \(\text{eV}\) at the same temperature is:
1. \(0.0015\)
2. \(0.003\)
3. \(0.048\)
4. \(0.768\)