I keep getting “Real vs ideal gas behaviour” questions wrong in States of Matter: Gases. What's the trap?
assuming every gas obeys the ideal equation under all conditions.
The usual trap: assuming every gas obeys the ideal equation under all conditions. How to avoid it: ideal-gas law works best at low pressure and high temperature. Go back to the definition — real gases deviate from PV = nRT at high pressure and low temperature, when molecular size and attractions can't be ignored.
Key point
Real vs ideal gas behaviour
Common mistake
assuming every gas obeys the ideal equation under all conditions.
Memory tip
ideal-gas law works best at low pressure and high temperature.
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