Real gases behave ideally at:
Correct answer: C. High temperature and low pressure
- A. Low temperature and low pressure
- B. Moderate temperature and low pressure
- C. High temperature and low pressure
- D. High temperature and high pressure
Explanation
Generally gas behaves more like an ideal gas at higher temperature and low pressure, as P.E due to intermolecular forces become less significant compared with particle kinetic energy. Real gas behaves like an ideal gas at high temperatures and low pressure.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
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.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Real and Ideal Gases questions
When does a gas deviate the most from its ideal behavior?
Under what conditions of density and pressure does a real gas approximate to an ideal gas?
Under which conditions, does a real gas approximate to an ideal gas?
The actual volume of gas molecules is considered negligible at following pressures:
Which of the following gases is more ideal at STP?
Real gas is converted to ideal gas at: