The mean free path of gas molecules depends on (d = molecular diameter)

For Boyle's law to hold the gas should be :

The kinetic energy of one mole gas at 300 K temperature, is E. At 400 K temperature kinetic energy is E'. The value of E'/E is

Consider a 1 c.c. sample of air at the absolute temperature ${\mathrm{T}}_0$ at sea level and another 1 c.c. sample of air at a height where the pressure is the one-third atmosphere. The absolute temperature T of the sample at that height is :

To double the volume of a given mass of an ideal gas at 27°C keeping the pressure constant, one must raise the temperature in degree centigrade to

Which of the following statements about kinetic theory of gases is wrong

If a Vander-Waal's gas expands freely, then final temperature is

In Vander Waal's equation $\left[\mathrm{P}+\frac{\mathrm{a}}{{\mathrm{V}}^2}\right]\left(\mathrm{V}-\mathrm{b}\right)=\mathrm{RT},$ the dimensions of a are

Which law states that effect of pressure is same for all portion

The equation for an ideal gas is PV = RT, where V represents the volume of

Under which of the following conditions is the law PV = RT obeyed most closely by a real gas

The gas equation $\frac{\mathrm{PV}}{\mathrm{T}}=$ constant is true for a constant mass of an ideal gas undergoing

That gas cannot be liquified :

At STP the mass of one litre of air is 1.293 gm. The value of the specific gas constant will be :

The pressure P, volume V and temperature T of gas in the jar A and the other gas in the jar B at pressure 2P, volume V/4 and temperature 2T, then the ratio of the number of molecules in the jar A and B will be :

A balloon contains $500 {\mathrm{m}}^3$ of helium at 27°C and 1 atmosphere pressure. The volume of the helium at – 3°C temperature and 0.5 atmosphere pressure will be :

A vessel contains 1 mole of ${\mathrm{O}}_2$ gas (molar mass 32) at a temperature T. The pressure of the gas is P. An identical vessel containing one mole of He gas (molar mass 4) at temperature 2T has a pressure of

A given mass of a gas is allowed to expand freely until its volume becomes double. If ${\mathrm{C}}_{\mathrm{b}}$ and ${\mathrm{C}}_{\mathrm{a}}$ are the velocities of sound in this gas before and after expansion respectively, then ${\mathrm{C}}_{\mathrm{a}}$ is equal to :

One litre of Helium gas at a pressure 76 cm of Hg and temperature 27°C is heated till its pressure and volume are doubled. The final temperature attained by the gas is :

The molecular weight of a gas is 44. The volume occupied by 2.2 g of this gas at $0°\mathrm{C}$ and 2 atm pressure will be-

A gas at 27°C temperature and 30 atmospheric pressure is allowed to expand to the atmospheric pressure. If the volume becomes 10 times its initial volume, then the final temperature becomes

In the relation $\mathrm{n}=\frac{\mathrm{PV}}{\mathrm{RT}}, \mathrm{n}=$

The equation of state corresponding to 8 g of ${\mathrm{O}}_2$ is :

Three containers of the same volume contain three different gases. The masses of the molecules are ${\mathrm{m}}_1, {\mathrm{m}}_2$ and ${\mathrm{m}}_3$ and the number of molecules in their respective containers are ${\mathrm{N}}_1, {\mathrm{N}}_2$ and ${\mathrm{N}}_3$ . The gas pressure in the containers are ${\mathrm{P}}_1, {\mathrm{P}}_2$ and ${\mathrm{P}}_3$ respectively. All the gases are now mixed and put in one of the containers. The pressure P of the mixture will be :

At a given volume and temperature, the pressure of a gas :

The rate of diffusion is :

At the top of a mountain a thermometer reads 7°C and a barometer reads 70 cm of Hg. At the bottom of the mountain these read 27°C and 76 cm of Hg respectively. Comparison of density of air at the top with that of bottom is

Two thermally insulated vessels 1 and 2 are filled with air at temperatures $\left({\mathrm{T}}_1, {\mathrm{T}}_2\right),$ volume $\left({\mathrm{V}}_1, {\mathrm{V}}_2\right)$ and pressure $\left({\mathrm{P}}_1, {\mathrm{P}}_2\right)$ respectively. If the valve joining the two vessels is opened, the temperature inside the vessel at equilibrium will be

For matter to exist simultaneously in gas and liquid phases :

The value of critical temperature in terms of Vander Waal’s constant a and b is