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. |
A gas at pressure is contained in a vessel. If the masses of all the molecules are halved and their speeds doubled, the resulting pressure would be:
1.
2.
3.
4.
The mean free path for a gas, with molecular diameter \(d\) and number density \(n,\) can be expressed as:
1. \( \frac{1}{\sqrt{2} n \pi \mathrm{d}^2} \)
2. \( \frac{1}{\sqrt{2} n^2 \pi \mathrm{d}^2} \)
3. \(\frac{1}{\sqrt{2} n^2 \pi^2 d^2} \)
4. \( \frac{1}{\sqrt{2} n \pi \mathrm{d}}\)
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. | \(2\times10^{6}\) |
The graph between volume and temperature in Charle's law is?
1. an ellipse
2. a circle
3. a straight line
4. a parabola
If the pressure of a gas is doubled, then the average kinetic energy per unit volume of the gas will be:
1. | half of its initial value. | 2. | double its initial value. |
3. | one-fourth of its initial value. | 4. | four times its initial value. |
The translational kinetic energy of n moles of a diatomic gas at absolute temperature T is given by:
1.
2.
3.
4.
Two isotherms are drawn at temperatures as shown. The ratio of mean speed at is:
1. | 1: 4 | 2. | 1: 2 |
3. | 2: 1 | 4. | 4: 1 |
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:
1. | Increases |
2. | Decreases |
3. | Remains the same |
4. | Any of the above depending on the molar mass |