Consider the following figure. Which of the following gases show negative as well as positive deviation from the ideal gas behaviour?

In the van der Waals equation,which of the following will have the highest value of '$a$'?

Which gas shows real behavior?

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 $dm^3$)?

The compressibility factor $(Z)$ of one mole of a van der Waals' gas of negligible '$a$' value is

Which among the following statements is/are incorrect regarding real gases?
$(i)$ Their compressibility factor is never equal to unity $(Z \neq 1)$.
$(ii)$ The deviations from ideal behavior are less at low pressures and high temperatures.
$(iii)$ Intermolecular forces among gas molecules are equal to zero.
$(iv)$ They obey Van der Waals equation,$PV = nRT$.