At the same temperature,which of the following gases will have the highest root mean square speed?

Initially,the root mean square $(rms)$ velocity of $N_2$ molecules at a certain temperature is $u$. If this temperature is doubled and all the nitrogen molecules dissociate into nitrogen atoms,then the new $rms$ velocity will be:

The average velocity of ideal gas molecules at $27\,^oC$ is $0.3\,m/s$. The average velocity at $927\,^oC$ is .......... $m/s$.

The average speed of $CH_4$ molecules at $300 \ K$ is equal to the average speed of $O_2$ molecules at ............ $K$.

For a gaseous state,if the most probable speed is denoted by $C^*$,average speed by $\overline{C}$,and root mean square speed by $C$,then for a large number of molecules,the ratio of these speeds is:

At a temperature of $27\,^{\circ}C$,$0.5 \, mol$ of $O_2$ gas is filled in a $50 \, L$ container at a pressure of $2 \, atm$. If half of the $O_2$ molecules are removed from the container,the $rms$ speed of the $O_2$ molecules will........