The compressibility factor Z equals PV over nRT. For an ideal gas its value is
Correct answer: B. exactly 1 at all pressures
- A. zero
- B. exactly 1 at all pressures
- C. always greater than 1
- D. always less than 1
Explanation
By definition an ideal gas satisfies PV equal to nRT exactly, so Z is one under every condition. For a real gas Z falls below one where attractive forces dominate and rises above one at high pressure where molecular volume dominates. Plotting Z against pressure is the standard way of displaying how far a gas departs from ideality.
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About Real and Ideal Gases
An ideal gas is modelled as particles with negligible volume and no intermolecular attraction, obeying Boyle's, Charles's and Avogadro's laws through PV = nRT. Real gases deviate from this behaviour, especially at high pressure and low temperature, because particle volume and attractive forces matter; the van der Waals equation explains these corrections.
Practise Gases
443 free Gases MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
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