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 value of Z for an ideal gas?

Explanation

To find the value of the compressibility factor \( Z \) for an ideal gas, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Compressibility Factor (Z)**:
The compressibility factor \( Z \) is defined as:
\[
Z = \frac{PV}{nRT}
...