The molecular mass of a gas having $r.m.s.$ speed four times as that of another gas having molecular mass $32$ is

$A$ vessel is partitioned into two equal halves by a fixed diathermic separator. Two different ideal gases are filled in the left $(L)$ and right $(R)$ halves. The rms speed of the molecules in the $L$ part is equal to the mean speed of the molecules in the $R$ part. Then the ratio of the mass of a molecule in the $L$ part to that of a molecule in the $R$ part is

The $rms$ speed of an ideal diatomic gas at temperature $T$ is $v$. When the gas dissociates into atoms,its new $rms$ speed becomes double. At what temperature does the dissociation of the gas occur?

The respective speeds of five molecules are $2, 1.5, 1.6, 1.6$ and $1.2 \, km/s$. The most probable speed in $km/s$ is:

At what temperature is the $rms$ speed of hydrogen molecules equal to the $rms$ speed of oxygen molecules at $47^{\circ}C$ (in $K$)?

The $v_{rms}$ value for a hydrogen molecule at $300 \ K$ is $1930 \ m/s$. Then the $v_{rms}$ for an oxygen molecule at $900 \ K$ is . . . . . . $m/s$.