For the diffusion of a gas at pressure $P$,the rate of diffusion is expressed by :

When the pressure of $1 \ mol$ of ammonia gas changes from $1 \ atm$ to $0.5 \ atm$ at constant temperature,the number of molecules will:

$A$ gaseous mixture of $3$ gases $A$, $B$ and $C$ has a pressure of $10 \,atm$. The total number of moles is $10$. If the partial pressures of gases $A$ and $B$ are $3 \,atm$ and $1 \,atm$ respectively, and the molar mass of gas $C$ is $2 \,g/mol$, calculate the weight of $C$ in the mixture. (in $\,g$)

At $27^{\circ} C$, a closed vessel contains a mixture of equal weights of helium (mol. wt. = $4$), methane (mol. wt. = $16$) and sulphur dioxide (mol. wt. = $64$). The pressure exerted by the mixture is $210 \ mm$. If the partial pressures of helium, methane and sulphur dioxide are $p_1, p_2$ and $p_3$ respectively, which one of the following is correct?

Calculate the partial pressure exerted by dioxygen from a mixture of $32 \ g$ $O_2$,$80 \ g$ $Ar$ (molar mass $40 \ g/mol$) and $4 \ g$ dihydrogen $(P_{\text{total}} = 10 \ bar)$. (in $bar$)

If $X \, mL$ of $H_2$ gas diffuses through a hole in a container in $5 \, s$,what is the time taken for the diffusion of the same volume of another gas under identical conditions?