The average kinetic energy of gas molecules is directly proportional to:

Molecules of a gas behave like

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

At ${0^ \circ }C$ the density of a fixed mass of a gas divided by pressure is $x.$ At ${100^ \circ }C,$ the ratio will be

If the molecular diameter of a gas is doubled, while the number density remains constant, its mean free path will:

A monoatomic gas is kept at room temperature 300K. Calculate the average kinetic energy of gas molecule (Use $k = 1.38 imes {10^{ - 23}}MKS$ units)

Vessel $A$ is filled with hydrogen while vessel $B,$ whose volume is twice that of $A,$ is filled with the same mass of oxygen at the same temperature. The ratio of the mean kinetic energies of hydrogen and oxygen is

The pressure and temperature of an ideal gas in a closed vessel are $720\;kPa$ and ${40^ \circ }C$ respectively. If $\frac{1}{4}$ th of the gas is released from the vessel and the temperature of the remaining gas is raised to ${353^ \circ }C,$, the final pressure of the gas is

If the mean free path of atoms is doubled then the pressure of gas will become

If masses of all molecules of a gas are halved and their speeds are doubles, then the ratio of initial and final pressures is

In a certain region of space there are only 5 molecules per ${\rm{c}}{{\rm{m}}^2}$ on an average. The temperature there is 3 K. The pressure of this dilute gas is ($k = 1.38 imes {10^{ - 23}}\;{\rm{J}}{{\rm{K}}^{ - 1}})$)