Compressibility factor, Z of a gas is given as `Z=(pV)/(nRT)`
(i) What is the value of Z for an ideal gas ?
(ii) 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,
Note Following imapotant points come out from the compressibility factor, `Z=(pV)/(nRT)`.
(i) For ideal `Z=1` at all temperatures and pressures because `pV=nRT`.
(ii) At very low pressure all gases shown have `Z cong 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 pressure most gases have `Z lt 1`.