If the pressure and temperature of $4 \, dm^3$ of carbon dioxide are doubled,what will be the volume of the carbon dioxide gas in $dm^3$?

If $20 \ cm^3$ of gas at $1 \ atm$ is expanded to $50 \ cm^3$ at constant $T$,what is the final pressure?

At what temperature will the volume of a gas be halved if the initial temperature is $17^{\circ}C$ and the pressure remains constant (in $^{\circ}C$)?

The volume occupied by $1.8 \; g$ of water vapour at $374^{\circ} C$ and $1 \; bar$ pressure will be $....... \; L$ : [Use $R=0.083 \; bar \; L \; K^{-1} \; mol^{-1}$]

At $300 \, K$ constant temperature,a gas having $20 \, cm^3$ volume and $1 \, bar$ pressure is converted into $50 \, cm^3$. Calculate the final pressure. (in $, bar$)

The density of air is higher at sea level. This fact is a practical application of which law?