Two gases, A and B, have molar masses of 16 g/mol and 64 g/mol respectively. If gas A takes 20 seconds to effuse through a small opening, how long will gas B take to effuse under the same conditions?

Under identical conditions of temperature and pressure, which gas will effuse fastest?

Graham's Law relates the rate of effusion of a gas to its:

Two gases, A and B, have molar masses of 16 g/mol and 64 g/mol respectively. If gas A takes 20 seconds to effuse through a small opening, how long will gas B take to effuse under the same conditions?

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

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

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

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:

Diffusion of helium gas is four times faster than