At room temperature,the $r.m.s.$ speed of the molecules of a certain diatomic gas is found to be $1920\, m/s$. The gas is

Derive the equation of $v_{rms}$ in terms of the mass of a molecule.

The relation between root mean square speed $(v_{rms})$ and most probable speed $(v_{p})$ for the molar mass $M$ of oxygen gas molecule at the temperature of $300\, K$ is:

The root mean square $(r.m.s.)$ velocity of a gas particle is $v$ at pressure $P$. If the pressure is increased to $2P$ while keeping the temperature constant,the $r.m.s.$ velocity becomes:

In two vessels of the same volume,atomic hydrogen and helium at pressures of $1\, atm$ and $2\, atm$ are filled,respectively. If the temperature of both samples is the same,then the average speed of hydrogen atoms $\langle C_H \rangle$ will be related to that of helium $\langle C_{He} \rangle$ as:

For a gas at room temperature of $27^{\circ}C$,the value of $\nu_{rms}$ is $1930 \, m/s$. The gas is.......... $(R = 8.3 \, J/mol \cdot K)$.