At a temperature of $27^{\circ}C$ and a pressure of $1 \, atm$,the ratio of the root mean square velocities $(\nu_{rms})_{H_2} / (\nu_{rms})_{O_2}$ for hydrogen and oxygen molecules is:

If the root mean square velocity of a hydrogen molecule at a given temperature and pressure is $2 \,km/s$, the root mean square velocity of oxygen at the same condition in $km/s$ is:

Temperature of an ideal gas, initially at $27^{\circ} C$, is raised by $6^{\circ} C$. The rms velocity of the gas molecules will

The Maxwell distribution function for different gases is shown in the figure. Which of the following is the correct matching?

The temperature of an ideal gas is increased from $100 \ K$ to $400 \ K$. If '$x$' is the root mean square velocity of its molecules at $100 \ K$,what is the new root mean square velocity?

At what temperature will the root mean square speed $(\nu_{rms})$ of oxygen gas molecules be equal to the $\nu_{rms}$ of hydrogen gas molecules at $27 \, ^\circ C$? $(M_{O_2} = 32 \, g \, mol^{-1}, M_{H_2} = 2 \, g \, mol^{-1})$