At very low pressure,if the molar volume of $CO_2$ is constant,its compressibility factor is ..........

The pressure of a van der Waals gas is less than the pressure of an ideal gas because of

The relation between pressure exerted by an ideal gas $(P_{ideal})$ and observed pressure $(P_{real})$ is given by the equation
$P_{ideal} = P_{real} + \frac{an^2}{V^2}$
$(i)$ If pressure is taken in $N \ m^{-2}$,number of moles in $mol$,and volume in $m^3$,calculate the unit of $a$.
$(ii)$ What will be the unit of $a$ when pressure is in atmosphere and volume in $dm^3$?

What is the pressure of $2 \, mol$ of $NH_3$ at $27 \, ^oC$ when its volume is $5 \, L$ using the van der Waals equation (in $, atm$)? ($a = 4.17 \, L^2 \, bar \, mol^{-2}$,$b = 0.03711 \, L \, mol^{-1}$)

For $NH_3$ gas,the $Z$ vs pressure $(P)$ curve at different temperatures is shown. What is the correct order of temperatures? (Given $T_B$ = Boyle temperature)

The van der Waals equation reduces to the ideal gas equation under which of the following conditions?