The ratio of the specific heats in terms of degrees of freedom (\(n\)) is given by:
1. \(1+1/n\)
2. \(1+n/3\)
3. \(1+2/n\)
4. \(1+n/2\)
1. | 2 moles of helium occupying 1 m3 at 300 K |
2. | 56 kg of nitrogen at \(10^5 ~\text{Nm}^{-2}\) and 300 K |
3. | 8 grams of oxygen at 8 atm and 300 K |
4. | \(6 \times 10^{26}\) molecules of argon occupying 40 m3 at 900 K |
The molecules of a given mass of gas have rms velocity of 200 ms-1 at \(27^{\circ}\mathrm{C}\) and 1.0 x 105 Nm-2 pressure. When the temperature and pressure of the gas are increased to, respectively, \(127^{\circ}\mathrm{C}\) and 0.05 X 105 Nm-2, rms velocity of its molecules in ms-1 will become:
1. 400/√3
2. 100√2/3
3. 100/3
4.100√2
At room temperature, the rms speed of the molecules of certain diatomic gas is found to be \(1930\) m/s. The gas is:
1. \(H_2\)
2. \(F_2\)
3. \(O_2\)
4. \(Cl_2\)
At which temperature the velocity of \(\mathrm{O_2}\) molecules will be equal to the velocity of \(\mathrm{N_2}\) molecules at \(0^\circ \mathrm{C}?\)
1. | \(40^\circ \mathrm{C}\) | 2. | \(93^\circ \mathrm{C}\) |
3. | \(39^\circ \mathrm{C}\) | 4. | Cannot be calculated |
If the pressure in a closed vessel is reduced by drawing out some gas, the mean free path of the molecules:
1. | decreases |
2. | increases |
3. | remains unchanged |
4. | increases or decreases according to the nature of the gas |
The specific heat of an ideal gas is:
1. proportional to
2. proportional to T2.
3. proportional to T3.
4. independent of
The specific heat of a gas:
1. | has only two values \(Cp\) and \(Cv\). |
2. | has a unique value at a given temperature. |
3. | can have any value between 0 and ∞. |
4. | depends upon the mass of the gas. |
For hydrogen gas \(C_P-C_V=a\) and for oxygen gas \(C_P-C_V=b\) where molar specific heats are given. So the relation between \(a\) and \(b\) is given by: (where \(C_p\) and \(C_V\) in J mol-1 K-1)
1. \(a=16b\)
2. \(b=16a\)
3. \(a=4b\)
4. \(a=b\)
The translatory kinetic energy of a gas per \(\text{g}\) is:
1. | \({3 \over 2}{RT \over N}\) | 2. | \({3 \over 2}{RT \over M}\) |
3. | \({3 \over 2}RT \) | 4. | \({3 \over 2}NKT\) |