Kinetic theory of gases

A closed vessel contains $10\,\mathrm{g}$ of an ideal gas X at $300\,\mathrm{K}$, which exerts $2\,\mathrm{atm}$ pressure. At the same temperature, $80\,\mathrm{g}$ of another ideal gas Y is added to it and the pressure becomes $6\,\mathrm{atm}$. The ratio of root mean square velocities of X and Y at $300\,\mathrm{K}$ is

If the distribution of molecular speeds of a gas is as per the figure shown below, then the ratio of the most probable, the average, and the root mean square speeds, respectively, is

Which of the following statement(s) is(are) correct regarding the root mean square speed $(u_{rms})$ and average translational kinetic energy $(\varepsilon_{av})$ of a molecule in a gas at equilibrium?

The diffusion coefficient of an ideal gas is proportional to its mean free path and mean speed. The absolute temperature of an ideal gas is increased 4 times and its pressure is increased 2 times. As a result, the diffusion coefficient of this gas increases $x$ times. The value of $x$ is

Initially, the root mean square (rms) velocity of $\ce{N2}$ molecules at certain temperature is u. If this temperature is doubled and all the nitrogen molecules dissociate into nitrogen atoms, then the new rms velocity will be :

Which of the following is not an assumption of the kinetic theory of gases ?

The value of d in cm (shown in the figure), as estimated from Graham's law, is

The experimental value of d is found to be smaller than the estimate obtained using Graham's law. This is due to

The temperature at which oxygen molecules have the same root mean square speed as helium atoms have at 300 K is : (Atomic masses : He = 4 u, O = 16 u)

Sulphur dioxide and oxygen were allowed to diffuse through a porous partition. 20 dm$^3$ of $\ce{SO2}$ diffuses through the porous partition in 60 seconds. The volume of $\ce{O2}$ in dm$^3$ which diffuses under the similar condition in 30 seconds will be (atomic mass of sulphur = 32 u) :

According to kinetic theory of gases

At 400 K, the root mean square (rms) speed of a gas X (molecular weight = 40) is equal to the most probable speed of gas Y at 60 K. The molecular weight of the gas Y is