At which temperature will the average velocity of ammonia $(NH_3)$ molecules be identical to the average velocity of nitric oxide $(NO)$ molecules at $327\,^oC$?

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:

If the kinetic energy and $RMS$ speed of a gas at a certain temperature are $4.0 \ kJ \ mol^{-1}$ and $5.0 \times 10^4 \ cm \ s^{-1}$,respectively,the molecular weight of the gas is:

The $rms$ velocity at $NTP$ of the species can be calculated from the expression

In the Maxwell-Boltzmann distribution of molecular speeds shown below,which of the following is correct regarding the most probable speed $(U_{M.P.})$ at temperatures $T_1$ and $T_2$?

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 ........... $K$.