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 $RMS$ velocity $(u_{rms})$ of one mole of an ideal gas was measured at different temperatures and the following graph is obtained. What is the slope $(m)$ of the straight line?
($x$-axis $= T$ $(K)$; $y$-axis $= (u_{rms})^2$; $M =$ molar mass; $R =$ gas constant)

The temperature of an ideal gas increases from $120 \ K$ to $480 \ K$. If the root mean square velocity of the gas molecules at $120 \ K$ is $v$,then at $480 \ K$ it will be .......

The $rms$ speed of $N_2$ molecules in a gas is $u$. If the temperature is doubled and the nitrogen molecules dissociate into nitrogen atoms,what will be the new $rms$ speed?

The ratio between the most probable speed of $N_2$ at $400 \ K$ and $CO$ at $800 \ K$ is (molar mass of $N_2 = 28 \ g \ mol^{-1}$, molar mass of $CO = 28 \ g \ mol^{-1}$)

At what temperature will the $RMS$ velocity of sulphur dioxide $(SO_2)$ molecules at $400 \ K$ be the same as the most probable velocity of oxygen $(O_2)$ molecules (in $K$)?