The rate of diffusion of a gas (molar mass = $128$) compared to oxygen is:

During the evaporation of a liquid:

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 $atm$)?

Gas $A$ diffuses $6$ times faster than hydrogen gas. What is the molar mass of $A$?

$A$ mixture of $0.5 \text{ mol}$ $N_2$ gas, $1.0 \text{ mol}$ $O_2$ gas and $1.5 \text{ mol}$ $H_2$ gas exerts a total pressure of $18 \text{ bar}$. Find the partial pressure of $O_2(g)$. (in $\text{ bar}$)

What is the ratio of kinetic energy of $7 \ g$ of nitrogen and $4 \ g$ of oxygen at $T \ K$?