Which is incorrect about ideal gas?
Correct answer: C. Can be liquefied easily
- A. No force of attraction between molecules
- B. No example in nature
- C. Can be liquefied easily
- D. Obey gas laws at all conditions of temperature and pressure
Explanation
Ideal gases cannot be liquefied easily. This is because ideal gases have no intermolecular forces, which are the forces that hold molecules together in a liquid. Without intermolecular forces, the molecules of an ideal gas would simply fly apart when the pressure is increased. An ideal gas cannot be liquefied easily because forces between its molecules are negligible, as a result the molecules do not come closer enough together.
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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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