What will be the minimum pressure required to compress $500 \, dm^{3}$ of air at $1 \, bar$ to $200 \, dm^{3}$ at $30^{\circ} C$ (in $, bar$)?

Calculate the temperature of $2 \text{ moles}$ of gas occupying a volume of $5.0 \text{ L}$ at a pressure of $24.6 \text{ atm}$. (Given: $R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1}$) (in $^\circ \text{C}$)

The correct combined gas law equation is:

$A$ and $B$ are ideal gases. At $T(K)$,$2 \ L$ of $A$ with a pressure of $1 \ bar$ is mixed with $4 \ L$ of $B$ with a pressure $p_B \ bar$ in a $100 \ L$ flask. The pressure exerted by the gaseous mixture is $0.1 \ bar$. What is the value of $p_B$ in $bar$?

At the same temperature,gas $A$ is taken in a $0.5 \, dm^3$ flask and gas $B$ is taken in a $1 \, dm^3$ flask. If the density of $A$ is $3.0 \, g \, dm^{-3}$ and that of $B$ is $1.5 \, g \, dm^{-3}$,and the molar mass of $A$ is $1/2$ of $B$,what is the ratio of the pressures exerted by the gases?

The volume of a given mass of a gas is directly proportional to its Kelvin temperature at constant pressure. The above statement is known as . . . . . .