Uranium has two isotopes of masses $235$ and $238$ units. If both of them are present in uranium hexafluoride gas, find the percentage ratio of the difference in rms velocities of the two isotopes to the rms velocity of the heavier isotope.

The root mean square speed of hydrogen molecules of an ideal hydrogen gas kept in a gas chamber at $0^{\circ}C$ is $3180 \ m/s$. The pressure on the hydrogen gas is ..... $atm$ (Density of hydrogen gas is $8.99 \times 10^{-2} \ kg/m^3$,$1 \ atm = 1.01 \times 10^5 \ N/m^2$).

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

The rms speed of oxygen at room temperature is about $500 \,m/s$. The rms speed of hydrogen at the same temperature is about (in $\,m/s$)

At a temperature of $27^{\circ}C$ and a pressure of $1 \, atm$,the ratio of the root mean square velocities $(\nu_{rms})_{H_2} / (\nu_{rms})_{O_2}$ for hydrogen and oxygen molecules is:

At room temperature,the $rms$ speed of a gas is $V_1$. If the pressure of the gas is doubled at the same room temperature,the $rms$ speed becomes $V_2$. Then: