At $740 \ torr$ pressure,the volume of $N_2$ gas is $800 \ mL$. If the volume becomes $540 \ mL$ at constant temperature,calculate the pressure of the gas. (in $torr$)

The value of the compressibility factor for an ideal gas is ........ .

Calculate the pressure of $HCl$ gas having a density of $8 \, kg \, m^{-3}$ at a temperature of $-40 \, ^oC$. (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,Molar mass of $HCl = 36.5 \, g \, mol^{-1} = 0.0365 \, kg \, mol^{-1}$)

At what new pressure will $100 \ mL$ of a gas at a pressure of $720 \ mm$ occupy a volume of $84 \ mL$,keeping the temperature constant (in $mm$)?

At a constant pressure $p$,the plot of volume $(V)$ as a function of temperature $(T)$ for $2 \, mol$ of an ideal gas gives a straight line with a slope $0.328 \, L \, K^{-1}$. The value of $p$ (in $atm$) is closest to
[Gas constant,$R=0.0821 \, L \, atm \, mol^{-1} \, K^{-1}$ ]

Which one of the following is the correct $PV$ vs $P$ plot at constant temperature for an ideal gas? ($P$ and $V$ stand for pressure and volume of the gas respectively)