Gas Laws
Physics · 50 practice questions
Boyle's law (isothermal process); Charles' law (isobaric process); Pressure law (volumetric process); absolute zero of temperature; general gas equation (PV/T = constant); ideal gas equation (PV = nRT); Van der Waals gas.
- Interpret the gas laws and use their expressions to solve numerical problems.
- Interpret the Van der Waals equation for one mole of a real gas.
Try a few questions
- Practice question 1
A pressure gauge attached to a sealed gas container can be used to experimentally verify the pressure law by measuring pressure at
- A.different fixed volumes, at constant temperature
- B.a single fixed temperature only, with no variation at all
- C.different fixed masses of gas, at constant temperature and volume
- D.different fixed temperatures, at constant volume
Show the answer
D. different fixed temperatures, at constant volume
Varying only temperature, while keeping volume fixed, directly tests the pressure law's predicted relationship.
- Practice question 2
An ideal gas is best described as a
- A.real gas that only obeys the gas laws at very high pressure
- B.gas that never actually exists under any laboratory conditions
- C.gas that only obeys the gas laws at extremely low temperature
- D.hypothetical gas that perfectly obeys the gas laws under all conditions
Show the answer
D. hypothetical gas that perfectly obeys the gas laws under all conditions
The "ideal gas" concept is a useful simplification, since no real gas obeys the gas laws perfectly in every condition.
- Practice question 3
Real gases behave more like ideal gases at low pressure mainly because
- A.the average distance between molecules becomes large, making intermolecular forces and molecular volume comparatively negligible
- B.molecules are packed extremely close together under low pressure
- C.intermolecular forces become extremely strong under low pressure
- D.gas molecules cease moving entirely under low pressure
Show the answer
A. the average distance between molecules becomes large, making intermolecular forces and molecular volume comparatively negligible
Greater molecular spacing at low pressure minimizes the real-gas effects that cause deviation from ideal behaviour.
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