Equal amounts of two gases of molecular weights $4$ and $40$ are mixed. The pressure of the mixture is $1.1 \ atm$. What will be the partial pressure of the lighter gas in the mixture (in $atm$)?

The atomic masses of carbon,nitrogen,and oxygen are $12, 14$,and $16$ respectively. Which of the following pairs of gases will diffuse at the same rate?

Which of the following is true about the gaseous state?

$A$ container consists of a mixture of $28 \ g \ N_2$,$8 \ g \ He$,and $40 \ g \ Ne$ at $25^{\circ} C$. If the total pressure exerted by the gaseous mixture is $20 \ bar$,what is the partial pressure exerted by $N_2$ (in $bar$)?

The ratio of densities of two gases is $1:16$. What will be the ratio of their rates of diffusion?

Provide the mathematical expression for Dalton's law of partial pressure.