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Q. No.An increase in the temperature of a gas-filled in a container would lead to:
| 1. | decrease in the intermolecular distance. |
| 2. | increase in its mass. |
| 3. | increase in its kinetic energy. |
| 4. | decrease in its pressure. |
The ratio of the average translatory kinetic energy of He gas molecules to gas molecules is:
1.
2.
3.
4. 1
The translational kinetic energy of n moles of a diatomic gas at absolute temperature T is given by:
1.
2.
3.
4.
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:
| 1. | \(14\times10^{-13}\) | 2. | \(10\times10^{-12}\) |
| 3. | \(10^{6}\) | 4. | \(2\times10^{6}\) |
Without change in temperature, a gas is forced in a smaller volume. Its pressure increases because its molecules:
| 1. | strike the unit area of the container wall more often. |
| 2. | strike the unit area of the container wall at a higher speed. |
| 3. | strike the unit area of the container wall with greater force. |
| 4. | have more energy. |
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 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 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. \(0.768\)
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Q. No.
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