A mixture of three gases X (density 1.0), Y (density 0.2), and Z (density 0.4) is enclosed in a vessel at constant temperature. When the equilibrium is established, the gas/gases:

When an ideal gas undergoes unrestricted expansion, no cooling occurs because the molecules:

Which of the following mixture of gases at room temperature would not follow Dalton's law of partial pressures?

The root mean square velocity of an ideal gas at constant pressure, varies with density (d) as :

Equal masses of methane and oxygen are mixed in an empty container at $25^{\circ }C25^\backslash circ\; C$. The fraction of the total pressure exerted by oxygen is :

The molecular velocity of any gas is :

Under critical state of a gas, for one mole of a gas, compressibility factor is :

A 100 mL flask contained $H_{2}H\_2$, at 200 Torr and a 200 mL flask contained He at 100 Torr. The two 2 flask were then connected so that each gas filled their combined volume. Assuming no change in temperature, total pressure is :

The temperature at which $N_{2}N\_2$ molecules would have the same average speed as that of helium atoms at 300K is :

At $0^{\circ }C0^\backslash circ\; C$ and one atm pressure, a gas occupies 100 cc. If the pressure is increased to one and a half-time and temperature is increased by one-third of given temperature, then final volume of the gas will be