At $300 \ K$,the compressibility factor of $1 \ mole$ of a gas is $1.1$. Its pressure is $2.706 \ atm$. What is its volume in $L$? (Given $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$).

In the given $pV \to V$ graph for gases at constant temperature,what kind of deviation will be observed for $H_2, He, CO, CH_4$?

Calculate the compressibility factor $(Z)$ of $1 \text{ mole}$ of a certain real gas if it occupies $0.4 \text{ dm}^3$ at $300 \text{ K}$ and $40 \text{ atm}$. [Given: $R = 0.082 \text{ dm}^3 \text{ atm K}^{-1} \text{ mol}^{-1}$]

When helium gas is allowed to expand into vacuum, a heating effect is observed. The reason for this is (assume $He$ as a non-ideal gas):

The figure represents $PV$ vs $P$ relation for $CO$, $CH_4$, $H_2$ and $He$ gases under identical conditions. Which curve, shown in the figure, represents $He$ gas?

$A$ gas that follows Boyle's law,Charle's law and Avogadro's law is called an ideal gas. Under what conditions does a real gas behave ideally?