Define the compressibility factor $(Z)$ in terms of the molar volume of a gas.

Under which conditions will a real gas behave most like an ideal gas?

The compressibility factor for a real gas at high pressure is $:$

$A$ certain quantity of real gas occupies a volume of $0.15 \ dm^3$ at $100 \ atm$ and $500 \ K$ when its compressibility factor is $1.07$. Its volume at $300 \ atm$ and $300 \ K$ (when its compressibility factor is $1.4$) is $........ \times 10^{-4} \ dm^3$ (Nearest integer).

Under which conditions do real gases deviate most from ideal gas behavior?

The $Van \text{ der } Waals$ equation explains the behaviour of