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 |
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. | \({3 \over 2}NKT\) |
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. \(0.768\)
Two containers of equal volumes contain the same gas at pressures \(P_1\) and \(P_2\) and absolute temperatures \(T_1\) and \(T_2\), respectively. On joining the vessels, the gas reaches a common pressure \(P\) and common temperature \(T\). The ratio \(\frac{P}{T}\) is equal to:
1. | \(\frac{P_1}{T_1}+\frac{P_2}{T_2}\) | 2. | \(\frac{P_1T_1+P_2T_2}{(T_1+T_2)^2}\) |
3. | \(\frac{P_1T_2+P_2T_1}{(T_1+T_2)^2}\) | 4. | \(\frac{P_1}{2T_1}+\frac{P_2}{2T_2}\) |