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 mean free path of molecules of a gas, (radius r) is inversely proportional to :
(1) r3
(2) r2
(3) r
(4) √r
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 the value of the density of a fixed mass of an ideal gas divided by its pressure is x. At this ratio is
1. x
2.
3.
4.
The ratio of two specific heats of gas for argon is 1.6 and for hydrogen is 1.4. Adiabatic elasticity of argon at pressure P is E. Adiabatic elasticity of hydrogen will also be equal to E at the pressure :
1. P
2.
3.
4. 1.4P
One mole of a perfect gas in a cylinder fitted with a piston has a pressure P, volume V and temperature 273 K. If the temperature is increased by 1 K keeping pressure constant, the increase in volume is
(1)
(2)
(3)
(4) V
If 300 ml of a gas at 27°C is cooled to 7°C at constant pressure, then its final volume will be -
(1) 540 ml
(2) 350 ml
(3) 280 ml
(4) 135 ml
1. | \(2\) moles of helium occupying \(1 ~\text m^3\) at \(300 ~\text K\) |
2. | \(56~\text{kg}\) of nitrogen at \(10^5 ~\text{Nm}^{-2}\) and \(300 ~\text K\) |
3. | \(8\) grams of oxygen at \(8~\text{atm}\) and \(300 ~\text K\) |
4. | \(6 \times 10^{26}\) molecules of argon occupying \(40 ~\text m^3\) at \(900 ~\text K\) |
Two vessels separately contain two ideal gases A and B at the same temperature, the pressure of A being twice that of B. Under such conditions, the density of A is found to be 1.5 times the density of B. The ratio of molecular weight of A and B is:
(a)2/3
(b)3/4
(c)2
(d)1/2