If ${V_H}$,${V_N}$,and ${V_O}$ denote the root-mean-square velocities of molecules of hydrogen,nitrogen,and oxygen respectively at a given temperature,then:

The gas having an average speed four times that of $SO_2$ (molecular mass $64$) is

At what temperature is the $rms$ speed of air molecules doubled compared to its value at $NTP$?

If the molecular weights of two gases are $M_1$ and $M_2$,then at a constant temperature,the ratio of their root mean square velocities $v_1$ and $v_2$ will be:

Let $\bar{v}$,${v_{rms}}$ and ${v_p}$ respectively denote the mean speed,root mean square speed,and most probable speed of the molecules in an ideal monoatomic gas at absolute temperature $T$. The mass of a molecule is $m$. Then

$A$ tube is divided into two parts,containing two different ideal gases,$L$ and $R$. If the $rms$ velocity of the gas on the left side is equal to the average velocity of the gas on the right side,what is the ratio of the masses of the molecules in $L$ and $R$?