Real gases deviate from ideal behaviour because the molecules

Identify the correct graph for an ideal gas ($y$-axis $= Z$; $x$-axis $= p$).

The $P$ vs $V$ graph is plotted for $1$ $mole$ of a hypothetical gas. Based on the given isotherms at $200 \ K$ and $300 \ K$,determine the range of $\frac{a}{b}$ for this gas in $atm-L \ mole^{-1}$. [Given: $R = 0.08 \ atm-L \ mole^{-1} \ K^{-1}$]

What is the compressibility factor $(Z)$ for the deviation of real gases from ideal behavior?

Which intermolecular force is most responsible for the liquefaction of inert gases?

For a non-ideal gas,identify the term in the van der Waals equation that represents the intermolecular forces.