Positive deviation from ideal behaviour.

Assertion: Helium shows only positive deviations from ideal behaviour. Reason: Helium is an inert gas.

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 For gases like H_(2) and He , which show only positive deviation from ideal behaviour, the compressibility factor is greater than 1. Is the statement true or false?

A: An azeotropic solution of two liquids has boiling point lower than either of them. R: Solution shows +ve deviation from ideal behaviour.

Which of the following gas always shows positive deviation from ideal gas behaviour ?

A solution of two liquids A and B showing a large negative deviation from ideal behaviour have