Gases Flashcards
1
Q
Kinetic theory
A
- Gases consist of large # of tiny particles
- Particles in constant, random motion
- Collisions between particles and walls are elastic
- No forces of attraction between molecules
- Avg kinetic energy proportional to temp
2
Q
Diffusion
A
Spontaneous mixing due to random motion (molecules moving from H-L concentration)
3
Q
Effusion
A
Gas moving through a small hole
4
Q
Real gas
A
Gas that doesn’t completely behave accoding to kinetic theory due to
- Molecules occupy space
- Exert attractive forces on each other
5
Q
Pressure
A
Force that gas exerts on given area
Force/area
6
Q
Volume
A
Space occupied by gas
7
Q
Temperature
A
Measure of avg kinetic energy of gas
8
Q
Boyle’s Law
A
P1V1=P2V2 Temperature constant Inverse relationship (1 up 1 down)
9
Q
Charles’s Law
A
V1/T1=V2/T2 Pressure constant Direct relationship (1 up 1 up)
10
Q
Gay-Lussac’s Law
A
P1/T1=P2/T2 Volume is constant Direct relationship (1 up 1 up) Higher temp=more collisions
11
Q
STP
A
Standard temp and pressure
1 atm, 0^C
12
Q
Ideal Gas Law
A
PV=nRT
13
Q
Combines Gas Law
A
P1V1/T1=P2V2/T2
14
Q
Dalton’s Law of Partial Pressure
A
P total=P1 + P2 + P3 + …
15
Q
Vapor pressure
A
Pressure exerted by liquid in equilibrium with its liquid state
