A gas mixture consist of 2 moles of and 4 moles of Ar at temperature T. Neglecting all vibrational modes, the total internal energy of the system is:
(1)4RT
(2) 15RT
(3)9RT
(4)11RT
One mole of an ideal monatomic gas undergoes a process described by the equation constant. The heat capacity of the gas during this process is:
(1)
(2)
(3)
(4)
A given sample of an ideal gas occupies a volume V at a pressure p and absolute temperature T. The mass of each molecule of the gas is m. Which of the following gives the density of the gas?
(1) p/(kT) (2) pm / (kT)
(3) p/ (kTV) (4) mkT
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
A monoatomic gas at a pressure p, having a volume V expands isothermally to a volume 2 V and then adiabatically to a volume 16 V. The final pressure of the gas is: (take γ=5/3)
(1) 64ρ
(2) 32ρ
(3) ρ/64
(4) 16ρ
The molar specific heats of an ideal gas at constant pressure and volume are denoted by CP and CV respectively. If γ=CP/CV and R is the universal gas constant, then CV is equal to
(1) 1+γ/1-γ
(2)R/(γ-1)
(3)(γ-1)/R
(4)γR
If and denote the specific heats (per unit mass) of an ideal gas of molecular weight M
(1)
(2)
(3)
(4)
At what temperature will the \(\text{rms}\) speed of oxygen molecules become just sufficient for escaping from the earth's atmosphere?
(Given: Mass of oxygen molecule \((m)= 2.76\times 10^{-26}~\text{kg}\), Boltzmann's constant \(k_B= 1.38\times10^{-23}~\text{J K}^{-1}\))
1. \(2.508\times 10^{4}~\text{K}\)
2. \(8.360\times 10^{4}~\text{K}\)
3. \(5.016\times 10^{4}~\text{K}\)
4. \(1.254\times 10^{4}~\text{K}\)
Two vessels separately contain two ideal gases \(\mathrm{A}\) and \(\mathrm{B}\) at the same temperature, the pressure of \(\mathrm{A}\) being twice that of \(\mathrm{B}\). Under such conditions, the density of \(\mathrm{A}\) is found to be \(1.5\) times the density of \(\mathrm{B}\). The ratio of molecular weight of \(\mathrm{A}\) and \(\mathrm{B}\) is:
1. | \(\frac{2}{3}\) | 2. | \(\frac{3}{4}\) |
3. | \(2\) | 4. | \(\frac{1}{2}\) |