Compressibility factor, Z, of a gas is given as `Z=(pV)/(nRT)`
(i) What is the value of Z for an ideal gas ?
For real gas what will be the effect on value of Z above Boyle.s temperature ?

Explanation

(i) For ideal gas, compressibility factor, Z = 1.
(ii) Above Boyle.s temperature, real gases show positive deviation.
So, `Z gt 1`
Note : Following important points come out from the compressibility factor, `Z=(pV)/(nRT)`
(i) For ideal Z = 1 at all temperatures and pressure because pV = nRT.
(ii) At very low pressure all gases shown have `Z ~=1` and behave as ideal gas.
(iii) At high pressure, all the gases have `Z gt 1` These are more difficult to compress.
(iv) At intermediate pressures most gases have `Z lt 1`.