$A$ vessel of $2.461 \ L$ contains a mixture of $0.3 \ mol$ of $N_2$,$0.5 \ mol$ of $He$,and $6.2 \ mol$ of $O_2$ at $27 \ ^oC$. What is the partial pressure of $N_2$ in the mixture in $atm$?

$A$ certain volume of oxygen gas diffuses through a porous pot in $20 \ s$. If the same volume of another gas $(X)$ diffuses in $Y \ s$, then $(X)$ and $Y$ respectively are:

The density of a gas at $STP$ is $2.86 \, g \, L^{-1}$. Which gas is it?

Between $NH_3$ and $CO_2$,which one will diffuse faster? What will be the ratio of their rates of diffusion?

$A$ sample of air contains $N_2, O_2$ and $H_2O$. It is saturated with water vapor and the total pressure is $640 \, torr$. The vapor pressure of water is $40 \, torr$ and the molar ratio of gases ${N_2}:{O_2}$ is $3:1$. What is the partial pressure of $N_2$ in the sample in $torr$?

To which of the following gaseous mixtures is Dalton's law of partial pressures not applicable?