Two identical containers hold equal moles of two different ideal gases, A and B, at the same temperature. The molecular mass of gas A is twice that of gas B. What is the ratio of the average kinetic energy of the molecules of gas A to gas B?

As the speed of molecules increases, the number of collisions per second:

If the rms speed of a gaseous molecule is $x\,\,{\rm{m}}{{\rm{s}}^{ - 1}}$ at a pressure $p$ atm, then what will be the rms speed at a pressure $2p$ atm and constant temperature

Two vessels having equal volume contain molecular hydrogen at one atmospheric and helium at two atmospheric pressure respectively. If both samples area at the same temperature the mean velocity of hydrogen molecular is:

The ratio between root mean square speed of ${{\rm{H}}_2}$ at $50{\rm{K}}$ and that of ${{\rm{O}}_2}$ at 800 K is:

At room temperature the rms speed of the molecules of a certain diatomic gas is found to be $1930{\rm{m}}/{\rm{s}}$. The gas is

The average Velocity of an ideal gas molecule at ${27^0}C$ is $0.3\,\,m/s$. The average velocity at ${927^0}C$ will be

Ratio of average to most probable velocity is

Among the given gases, the value of van der Waal’s constant `a’ is maximum for

The root mean square speed of the molecules of diatomic gas is $u$. When the temperature is doubled, the molecules dissociates into two atoms. The new speed of the atom is:

A sample of gas is at 0\,^\circ C. The temperature at which its ${\rm{rms}}$ speed of the molecules will be doubled is: