Kinetic Theory Of Gases Flashcards
1
Q
Pressure x volume
A
= 1/3 (number of molecules) x mass x (root mean square speed)^2
2
Q
Kinetic gas theory assumptions
A
- identical
- large number of molecules
- negligible volume of molecules compared with volume of the gas
- random motion (direction and speed)
- attraction is negligible
- all collisions are elastic
- molecules move in straight lines
- forces acting during collisions act for a short time relative to the time between collisions
3
Q
Average velocity = 0
A
Due to particles all heading in different directions
4
Q
Pressure of the gas increases when the volume reduces because the molecules travel less distance between impacts so the impacts with the walls are more frequent.
A
Boyle’s Law
5
Q
Pressure of the gas increases as the temperature rises because the molecules have a larger average speed so the impacts with the walls are harder and more frequent.
A
Pressure law
6
Q
Pressure = force/area =
A
Change in momentum/(time x surface area)
