At $300 \, K$ temperature and $1 \, atm$ pressure,the volume of $7.0 \, g$ of a gas is $4.1 \, L$. What is the molar mass of the gas?

$n$ 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 $mol / L$)?

At $273\,K$,$Pd$ vs $P$ is plotted for various gases $1, 2, 3, 4$. Assuming ideal behaviour for four gases $N_2, He, CO_2$ & $H_2$. The correct combination is [$P$ denotes pressure in atmosphere & $d$ denotes density in $g/L$]

Which gas has a density of $1.24 \ g/L$ at $0^{\circ} C$ and $1 \ atm$ pressure?

At $25^{\circ} C$ and $760 \,mm \,Hg$ pressure,a gas occupies $600 \,mL$ volume. What will be its pressure at a height where the temperature is $10^{\circ} C$ and the volume of the gas is $640 \,mL$?

If the density of dioxygen gas at $STP$ is $1.43 \, g \, L^{-1}$,calculate its density at $17 \, ^\circ C$ and $800 \, torr$ pressure.