The ratio of densities of $O_2$ and $H_2$ is $16 : 1$. The ratio of their $rms$ velocities will be:

$RMS$ velocity of one mole of an ideal gas was measured at different temperatures. $A$ graph of $(u_{rms})^2$ (on y-axis) and $T(K)$ (on x-axis) gave a straight line passing through the origin and its slope is $249 \ m^2 \ s^{-2} \ K^{-1}$. What is the molar mass (in $kg \ mol^{-1}$) of the ideal gas? $(R=8.3 \ J \ mol^{-1} \ K^{-1})$

The rms velocity of oxygen molecules at $27^{\circ} C$ is around $800 \ m/s$. The rms velocity of methane molecules at $600 \ K$ temperature is around ...... (in $m/s$)

The most probable speed $(u_{mp})$ of $8 \ g$ of $H_2$ is $2 \times 10^2 \ ms^{-1}$. The kinetic energy (in $J$) of the same amount of $H_2$ gas is:

What is the approximate most probable velocity of oxygen, if the kinetic energy of one mole of oxygen is $3741.3 \ J$?

The relationship among most probable velocity,average velocity,and root mean square velocity is respectively: