The root mean square velocity of an ideal gas at constant pressure varies with density $(d)$ as:

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

The temperature at which oxygen molecules have the same root mean square speed as helium atoms have at $300 \ K$ is (Atomic masses: $He = 4 \ u$,$O = 16 \ u$) (in $K$)

The ratio of most probable velocity $(u_{mp})$,average velocity $(u_{av})$,and root mean square velocity $(u_{rms})$ is:

At $T(K)$,the root mean square (rms) velocity of argon (molar mass $40 \ g \ mol^{-1}$) is $20 \ ms^{-1}$. The average kinetic energy of the same gas at $T(K)$ (in $J \ mol^{-1}$) is:

Which of the following equations does not represent the root mean square velocity $(u_{rms})$?