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2 cards from this section. Quick, good the night before a test.
Define the kinetic theory of gases.
Think about what the particles in a gas do.
What does pressure depend on in a gas?
It's about how hard and how often particles hit the walls.
What describes the pressure in a gas?
Think about how particles interact with their surroundings.
True or False: The temperature of a gas is directly proportional to the average kinetic energy of its particles.
Consider the connection between heat and motion in gases.
A 2.0 L gas sample is maintained at 300 K and exerts a pressure of 1.5 atm. If the temperature is increased to 450 K with a constant volume, what will the new pressure be?
Make sure to convert all units properly and remember to maintain consistent temperature units.
Explain why the ideal gas equation may not apply to real gases at very high pressures and low temperatures.
Consider the assumptions of the ideal gas law.
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