The root mean square speed of hydrogen molecules at room temperature is $2400\,\,{\rm{m}}{{\rm{s}}^{ - 1}}$. At room temperature the root mean square speed of oxygen molecules would be:

The rates of diffusion of ${{\rm{O}}_2}$ and ${{\rm{H}}_2}$ at same $P$ and $T$ are in the ratio:

For one mole of an ideal gas, increasing the temperature from $10^\circ C$ to 20\,\,^\circ C

Equal moles of nitrogen and oxygen gases are placed in a porous container. After a certain time, one-fifth of the nitrogen has escaped. What fraction of the oxygen has escaped in the same time period?

The rate of diffusion of methane at a given temperature is twice that of gas X. The molecular mass of gas X is

Two gases, A and B, have molar masses of 2 g/mol and 32 g/mol respectively. According to Graham's Law, what is the ratio of their rates of effusion?

If both oxygen and helium gases are at the same temperature, the rate of diffusion of ${{\rm{O}}_2}$ is very close to

$A$ , $B$ and $C$ are ideal gases. Their molecular weights are 2, 4 and 28 respectively. The rate of diffusion of these gases follow the order

The root mean square speed of hydrogen molecules at room temperature is $2400\,\,{\rm{m}}{{\rm{s}}^{ - 1}}$. At room temperature the root mean square speed of oxygen molecules would be:

Which pair of the gases diffuse through a small hole with the same rate of diffusion at same ‘P’ at ‘T’

Equal moles of hydrogen and oxygen gases are placed in a container with a pin-hole through which both can escape. What fraction of the oxygen escape in the time required for one-half of the hydrogen to escape?