At $300 \ K$ the average velocity of a gas is $3 \times 10^2 \ cm / s$. The average velocity (in $cm / s$) of it at $1200 \ K$ is

The ratio of the root mean square velocity of $H_2$ at $50 \ K$ to that of $O_2$ at $800 \ K$ is .......

If the average velocity of $N_2$ molecule is $0.3 \, m/s$ at $27 \, ^\circ C$,then the velocity will be $0.6 \, m/s$ at ........... $K$.

The following graph is obtained for a gas at different temperatures $T_1$,$T_2$,$T_3$. What is the correct order of temperature? ($x$-axis $=$ velocity; $y$-axis $=$ number of molecules)

The $rms$ speed of $N_2$ molecules in a gas is $v$. If the temperature is doubled and the nitrogen molecules dissociate into nitrogen atoms,the $rms$ speed becomes

$A$ gas bulb of $1 \ L$ capacity contains $2.0 \times 10^{21}$ molecules of nitrogen gas at a pressure of $7.57 \times 10^3 \ N \ m^{-2}$. Calculate the root mean square speed in $cm \ sec^{-1}$. (in $.5$)