In the $Vander$ $Waals$ equation,the constant $'b'$ is a measure of $......$.

Under what conditions do real gases behave as ideal gases?

Consider the following gases and their corresponding $ 'a'$ values given in parentheses: $CH_4 (2.25), N_2 (1.35), O_2 (1.36)$,and $CO (1.46)$. Which of these gases will be the most difficult to liquefy?

If $Z$ is the compressibility factor,then for $1 \, \text{mole}$ of a real gas,the van der Waals equation at low pressure can be written as:

Which of the following can be most easily liquefied? (Value of $a$ for $NH_3 = 4.17, CO_2 = 3.59, SO_2 = 6.71, Cl_2 = 6.49$)

Which of the curves $(Z \ vs \ p)$ will be followed by a real gas?