kinetic theory of gases. overview assume atomic picture of gases –simpler than solids/liquids, as...
TRANSCRIPT
Kinetic Theory of Gases
Overview
• Assume atomic picture of gases– Simpler than solids/liquids, as interactions
can be neglected
• Predict behavior– E.g., relations between P and V, P and T…
• Test in lab experiments
Basic Picture
• Gas consists of noninteracting particles
• They move around randomly
• Temperature corresponds to (average) speed of particles– Hotter faster
• Pressure a manifestation of collisions with container walls
Basic Processes
• Thermal expansion
• Evaporation– A cooling process
• Dissolving solids in liquids
• Reaction rates
• …
More on Temperature
• Prediction of kinetic theory:
v is the average speed
T is the temperature (in Kelvins)
m is the mass of a gas particle
kB is Boltzmann’s constant
• Note that
Tkmv B2
3
2
1 2
2vT
More on Pressure
• Canonical example: container wih movable piston
• P is the average force per unit area due to collisions with walls– Average because it fluctuates
• Weight on piston balances this force, in equilibrium– W tells us P of gas
Weight W
Now change something…
• E.g. add weight to the piston (T = const)• Forces out of equilibrium; piston drops• Collision rate increases until forces again
balance• P has increased, V decreased• In fact,
VP 1 (Boyle)
Computer Simulation
• Allows changing N, W, v
• Replaces tedious mathematical analysis
• Explore all relations encoded in the Ideal Gas Law: PV = NkBT
• Most of these relations are qualitatively obvious, some even quantitatively so!
Another Example
• Increase T keeping P fixed– Note: doubling T means increasing v by
• Faster particles means harder collisions and more rapid
• Piston rises, reducing collision rate• Equilibrium is restored• Model gives
TV (constant P)
2
Another Example
• Increase N with P and T held fixed• More particles means more collisions, piston
rises• Reduced collision rate restores equilibrium• In detail:
NV (constant T, P)
A slightly more complicated one…
• Increase T with V and N held constant
• Do it in two steps:– Increase T with P unchanged– Increase W to return V to its original value
• Result: TP (constant V, N)
Verifying the Predictions
• These relations are simple predictions of atomic/kinetic theory
• If they are found to hold in experiments, we gain confidence that the atomic picture is correct!
• Several of them are easily checked in lab exercises
Sample Exercises
• Calculate v for gas at room temperature
• It may take a few seconds for a smell to reach you from across a room, e.g. from a perfume bottle. What does this suggest about the path taken by the perfume particles?
Reference
• R. P. Feynman, et al., The Feynman Lectures on Physics, v. I (Addison Wesley, 1970)