At $300 \ K$,one mole of a gas present in a $10 \ L$ flask exerted a pressure of $2.706 \ atm$. What is its compressibility factor $(Z)$? (Given $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$).

Under what conditions do real gases behave as ideal gases?

Dominance of strong repulsive forces among the molecules of the gas ($Z =$ compressibility factor)

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: $R = 0.082 \text{ dm}^3 \text{ atm K}^{-1} \text{ mol}^{-1}$]

The units of constant $a$ in the Van der Waals equation are:

The temperature at which a real gas obeys ideal gas laws over an appreciable range of pressure is called ..........