The ideal gas behaviour has been expressed in terms of ideal gas equation `PV =nRT` Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor `Z = (Z =(PV)/(nRT))` Usually when `Z gt1` repulsive forces among molecules predominates and when `Z lt1` attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of `Z` for 1 mole of gas at critical conditions is `(3)/(8)`
The compressibility factor `SO_(20` is `0.711` then .
A. `SO_(2)` is more compressible than ideal gas
B. `SO_(2)` is less compressible than ideal gas
C. `SO_(2)` is less equally compressible
D. `SO_(2)` can not be compressed
