Which among the following statements is/are incorrect regarding real gases?
(i) Their compressibility factor is never equal to unity 
.
(ii) The deviations from ideal behaviour are less at low pressure and high temperatures.
(iii) Intermolecular forces among gas molecules are equal to zero.
(iv) They obey van der Waal's equation, 
Text Solution
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(i) For real gases compressibility factor (Z) cannot be unity, while compressibility factor for an ideal gas is one.
(ii) A gas can behave like an ideal gas at very high temperature and low pressure. Hence, show very less deviation.
(iii) Intermolecular forces among gas molecules are weak as compare to liquid and solid but, these forces cannot be zero.
(iv) Ideal gas follows van der Waal's equation 
Gases which do not follow this equation are real gases
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