If the rms speed of the molecules of a diatomic gas at a temperature of $322 \ K$ is $2000 \ m \ s^{-1}$,then the gas is

The $r.m.s.$ speed of the molecules of a gas at a pressure $10^5 \ Pa$ and temperature $0^\circ C$ is $0.5 \ km \ sec^{-1}.$ If the pressure is kept constant but temperature is raised to $819^\circ C,$ the velocity will become ........ $km \ sec^{-1}.$

For a gas at room temperature of $27^{\circ}C$,the value of $\nu_{rms}$ is $1930 \, m/s$. The gas is.......... $(R = 8.3 \, J/mol \cdot K)$.

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?

At what temperature $(^oC)$ will the $rms$ speed of hydrogen be double its value at $S.T.P.$? The pressure remains constant.

The molecules of a given mass of a gas have a $r.m.s.$ velocity of $200 \, m/s$ at $27^{\circ}C$ and $1.0 \times 10^5 \, N/m^2$ pressure. When the temperature is $127^{\circ}C$ and pressure is $0.5 \times 10^5 \, N/m^2$,the $r.m.s.$ velocity in $m/s$ will be