Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is
`Z=(pV)/(nRT)`
The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at `0^(@)C` and 100 atm pressure is found to be 0.5. The van der Waals gas equation is
`(p(an^(2))/(V^(2)))(V-nb)=nRT`
What is the significance of van der Waals constant 'a'?

Explanation

To answer the question regarding the significance of the van der Waals constant 'a', we can follow these steps:

### Step 1: Understand the Van der Waals Equation
The van der Waals equation is a modification of the ideal gas law that accounts for the volume occupied by gas molecules and the intermolecular forces between them. It is given by:
\[ \left( p + \frac{a n^2}{V^2} \right)(V - nb) = nRT \]
Where:
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