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
Which one of the following gases possesses the largest internal energy?
1. | 2 moles of helium occupying 1m3 at 300 K |
2. | 56 kg of nitrogen at \(10^5 \mathrm{Nm}^{-2}\) 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 mean free path of molecules of a gas, (radius r) is inversely proportional to :
(1) r3
(2) r2
(3) r
(4) √r
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
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