The respective speeds of the five molecules are $1, 2, 3, 4$ and $5 \ km/s$. The ratio of their root mean square (rms) velocity to their average velocity is:

$A$ mixture of $2$ moles of helium gas (atomic mass $= 4 \ amu$) and $1$ mole of argon gas (atomic mass $= 40 \ amu$) is kept at $300 \ K$ in a container. The ratio of the rms speeds $\left(\frac{v_{\text{rms}} \text{ (helium)}}{v_{\text{rms}} \text{ (argon)}}\right)$ is:

The given diagram shows isotherms for a fixed mass of an ideal gas at temperatures $T_1$ and $T_2$. What is the value of the ratio $\frac{\text{r.m.s. speed of the molecules at temperature } T_2}{\text{r.m.s. speed of the molecules at temperature } T_1}$?

The rms speed of a gas molecule is $V$ at pressure $P$. If the pressure is increased by two times,then the rms speed of the gas molecule at the same temperature will be

The $v_{rms}$ of gas molecules in a container is $400 \ ms^{-1}$. If half of the gas leaks out of the container at a constant temperature,the $v_{rms}$ of the remaining gas molecules will be . . . . . . $ms^{-1}$.

If the rms velocity of hydrogen gas at a certain temperature is $c,$ then the rms velocity of oxygen gas at the same temperature is