The temperature of an ideal gas is increased from $140 \,K$ to $560 \,K$. If the r.m.s. speed of gas molecules is $v$ at $140 \,K$, then at $560 \,K$, the r.m.s. speed becomes:

At a given temperature,the $rms$ velocity of a gas molecule of mass $m$ is proportional to:

The $rms$ speed of hydrogen molecules at room temperature $(300 \ K)$ will be:

At a temperature of $27^{\circ}C$ and a pressure of $1.0 \times 10^5 \, N/m^2$,the $rms$ speed of a gas is $200 \, m/s$. What is the $rms$ speed at a temperature of $127^{\circ}C$ and a pressure of $0.5 \times 10^5 \, N/m^2$?

The r.m.s. speed of gas at temperature $T$ is $2$ times the r.m.s speed at $320 \,K$. The value of the temperature $T$ is (in $\,K$)

At what temperature $(^oC)$ is the average speed of hydrogen molecules equal to the average speed of oxygen molecules at $31^oC$?