The compressibility factor $(Z)$ of a gas is less than unity at $STP$. Therefore:

Given van der Waals constant $a$ for $NH_{3}$,$H_{2}$,$O_{2}$ and $CO_{2}$ are respectively $4.17$,$0.244$,$1.36$ and $3.59$,which one of the following gases is most easily liquefied?

The given graph represents the variation of $Z$ (compressibility factor = $\frac{PV}{nRT}$) versus $P$,for three real gases $A, B$ and $C$. Identify the only incorrect statement.

The Van der Waals equation reduces itself to the ideal gas equation at

Which of the following gas samples shows real gas behavior?

If $Z$ is the compressibility factor,then for $1 \, \text{mole}$ of a real gas,the van der Waals equation at low pressure can be written as: