What is the volume of $1 \ mole$ of a real gas at $STP$ $(V_{ideal} = 22.4 \ dm^3)$,if the compressibility factor of the real gas is $1.1$ at $STP$ (in $dm^3$)?

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

For a real gas at $25^{\circ} C$ temperature and high pressure $(99 \ bar)$,the value of the compressibility factor is $2$. The value of the Van der Waals constant '$b$' is $\times 10^{-2} \ L \ mol^{-1}$. (Nearest integer) (Given $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)

The compressibility factor of a real gas at high pressure is

What is Boyle's temperature? Give its relation with the value of $Z$.

The compressibility factor $(z)$ is lower for $NH_3$ and $CO_2$ gases than that of $N_2$ gas, because