A mixture of $N_2$ and an unknown gas X effuses through a porous barrier in 5 minutes and 7 minutes respectively under identical conditions. If the molar mass of $N_2$ is 28 g/mol, what is the most likely identity of gas X given the following options?

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?

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:

Identify the pair of gases that have equal rates of diffusion

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

Equal moles of methane ($CH_4$) and sulfur dioxide ($SO_2$) are placed in a container with a pin-hole. What fraction of the sulfur dioxide escapes in the time required for one-fourth of the methane to escape?

A mixture of 0.50 mole of ${{\rm{H}}_{\rm{2}}}$ and 0.50 mole of ${\rm{S}}{{\rm{O}}_{\rm{2}}}$ is introduced into a 10.00 L container at ${\rm{2}}{{\rm{5}}^{\rm{0}}}{\rm{C}}$. The container has a pinhole leak. After a period of time, the partial pressure of ${{\rm{H}}_2}$ in the remaining mixture

What is the ratio of diffusion rate of oxygen and hydrogen?

$2{\rm{g}}$ of hydrogen diffuses from a container in 10 minute. How many gram of oxygen would diffused through the same container in the same time under similar conditions?

The density of ${\rm{CC}}{{\rm{l}}_4}$ vapour at 0\,^\circ C and 76 cm Hg in ${\rm{g}}/{\rm{litre}}$ is:

Equal moles of ${H_2}$ and ${O_2}$ gases are placed in a container with a pin hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the ${H_2}$ to escape