The temperature of a gas is $-68^{\circ} C$. To what temperature should it be heated,so that the r.m.s. velocity of the molecules be doubled (in $^{\circ} C$)?

The rms speed of a gas molecule is $V$ at pressure $P$. If the pressure is increased by two times,then the rms speed of the gas molecule at the same temperature will be

In Maxwell's speed distribution curve,for $N_2$ gas,the average relative velocity (in $m/s$) between two molecules at $300 \, K$ is:

The curve between absolute temperature $T$ and $v_{rms}^2$ is

Nitrogen gas is at $300^{\circ} C$ temperature. The temperature (in $K$) at which the $rms$ speed of a $H_{2}$ molecule would be equal to the $rms$ speed of a nitrogen molecule is........ (Molar mass of $N_{2}$ gas = $28 \ g/mol$,Molar mass of $H_{2}$ gas = $2 \ g/mol$)

Six molecules of a gas in a container have speeds $2 \,m/s, 5 \,m/s, 3 \,m/s, 6 \,m/s, 3 \,m/s$ and $5 \,m/s$. The root mean square (r.m.s.) speed is: (in $\,m/s$)