`1 mol` of `C Cl_(4)` vapours at `77^(@)C` occupies a volume of `35.0 L`. If van der Waals constants are `a=20.39 L^(2) atm mol^(-2)` and `b=0.1383 L mol^(-1)`, calculate compressibility factor `Z` under
(`a`) Low pressure region
(`b`) High pressure region

Explanation

To calculate the compressibility factor \( Z \) for \( 1 \, \text{mol} \) of \( \text{CCl}_4 \) vapors at \( 77^\circ C \) occupying a volume of \( 35.0 \, \text{L} \) under low and high pressure regions, we can follow these steps:

### Given Data:
- Number of moles, \( n = 1 \, \text{mol} \)
- Volume, \( V = 35.0 \, \text{L} \)
- Temperature, \( T = 77^\circ C = 350 \, \text{K} \) (convert to Kelvin by adding 273)
- Van der Waals constants:
- \( a = 20.39 \, \text{L}^2 \, \text{atm} \, \text{mol}^{-2} \)
...