$A$ certain sample of gas has a volume of $0.2 \ L$ at one atmosphere pressure and $273.15 \ K$. What is the volume of gas at $273.15 \ ^{\circ}C$ at the same pressure (in $L$)?

$A$ dry gas occupied $127.4 \, mL$ at $STP$. If the same mass of the gas is collected over water at $27 \, ^\circ C$ and at a total pressure of $725 \, torr$,what volume does it occupy? The vapour pressure of water at $27 \, ^\circ C$ is $25 \, torr$. (Note: $1 \, bar = 750 \, torr$)

$4 \ g$ of an ideal gas occupies $5.6035 \ L$ of volume at $546 \ K$ and $2 \ atm$ pressure. What is its molecular weight?

What is the relationship between the molecular mass,density,and volume of a gas?

What is the volume in $litre$ occupied by $7 \, g$ of $N_2$ gas at $27 \, ^oC$ temperature and $750 \, mm \, Hg$ pressure?

$n$ moles of an ideal gas at temperature $T$ (in kelvin) occupy $V \ L$ of volume, exerting a pressure of $P$ atmospheres. What is the concentration (in $mol / L$)?