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 gas which always shows predominative repulsive forces .

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 .

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 ratio of Z at Boyle's temperature and at critical conditions for 1 mole of a given gas is .

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 numerical value of Z is greater than 1 for gases usually at .

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 numerical value of 'Z' for gases within Boyle's temperature range is .

Gas deviates from ideal gas nature because molecules

Establish ideal gas equations (PV=nRT).