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,$R=0.0821 \, L \, atm \, mol^{-1} \, K^{-1}$ ]

To an evacuated vessel with a movable piston under an external pressure of $1 \ atm$,$0.1 \ mol$ of $He$ and $1.0 \ mol$ of an unknown compound (vapour pressure $0.68 \ atm$ at $0^{\circ} C$) are introduced. Considering ideal gas behaviour,the total volume (in litres) of the gases at $0^{\circ} C$ is close to:

At what pressure will a quantity of gas occupy a volume of $60 \, mL$,if it occupies a volume of $100 \, mL$ at a pressure of $720 \, mm$ (assuming temperature is constant)?

Which effect is observed when the pressure of a gas increases?

At $N.T.P.$,the density of a gas is $0.00356 \ g/mL$. What is the molecular mass of the gas?

An open vessel at $27\,^{\circ}C$ is heated until two-fifths of the air (assumed as an ideal gas) in it has escaped from the vessel. Assuming that the volume of the vessel remains constant,the temperature to which the vessel has been heated is: