To what temperature should the hydrogen at room temperature $(27^{\circ}C)$ be heated at constant pressure so that the $R.M.S.$ velocity of its molecules becomes double of its previous value?

If $c$ is the $rms$ speed of molecules in a gas and $v$ is the speed of sound waves in the gas,show that $\frac{c}{v}$ is constant and independent of temperature for all diatomic gases.

The rms velocity of a gas molecule of mass $m$ at a given temperature is proportional to

The root mean square speed of molecules of nitrogen gas at $27^{\circ} C$ is approximately $.......m/s$. (Given: mass of a nitrogen molecule $= 4.6 \times 10^{-26} \, kg$ and Boltzmann constant $k_{B} = 1.4 \times 10^{-23} \, J K^{-1}$)

The $rms$ speeds of the molecules of Hydrogen,Oxygen,and Carbon dioxide at the same temperature are $V_{H}$,$V_{O}$,and $V_{C}$ respectively. Then:

The rms speed of an oxygen molecule at a certain temperature is $600 \,ms^{-1}$. If the temperature is doubled and the oxygen molecule dissociates into atomic oxygen atoms,the new rms speed is (in $\,ms^{-1}$)