At identical temperature and pressure, the rate of diffusion of hydrogen gas is $3\sqrt{3}$ times that of a hydrocarbon having molecular formula $C_n H_{2n-2}$. What is the value of '$n$'?

The ratio of rates of diffusion of gases $A$ and $B$ is $1 : 0.707$. If the molecular weight of $B$ is $32$,the molecular weight of $A$ is

$A$ neon-dioxygen mixture contains $70.6 \ g$ dioxygen and $167.5 \ g$ neon. If the total pressure of the mixture of gases in the cylinder is $25 \ bar$,what are the partial pressures of dioxygen and neon in the mixture?

$A$ sample of $O_2$ gas is collected over water at $23\,^oC$ at a barometric pressure of $751\, mm\, Hg$ (vapour pressure of water at $23\,^oC$ is $21\, mm\, Hg$). The partial pressure of $O_2$ gas in the sample collected is

Which of the following relationships is correct,where $r$ is the rate of diffusion of a gas and $d$ is its density?

$A$ gas diffuses $1/3$ times as fast as hydrogen. Its molecular weight is