Real gases deviate most from ideal behaviour at
Correct answer: B. low temperature and high pressure
- A. high temperature and low pressure
- B. low temperature and high pressure
- C. high temperature and high pressure
- D. standard temperature and pressure
Explanation
At high pressure the molecules are close enough that their own volume is no longer negligible, and at low temperature they move slowly enough for intermolecular attractions to matter. Both assumptions of the ideal model fail together under those conditions, which is also why gases liquefy there. A gas behaves most ideally when it is hot and dilute.
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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
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