Unit 6 Flashcards
(24 cards)
Liquid
Particles move by sliding past each other
Indefinite shape
Definite volume
Gas
Particles spread out throughout container
Indefinite shape
Indefinite volume
Highest KE
Melting
Solid–liquid
Freezing
Liquid–solid
Boiling (vaporization)
Liquid–gas
Condensation
Gas–liquid
Sublimation
Solid–gas
Deposition
Gas–solid
How to convert to kelvin
K=degrees Celsius + 273
Atm to psi
1 atm=14.7 psi
Atm to kPa
1 atm = 101 kPa
Atm to mmHg
1 atm = 760 mm Hg
STP
Standard temperature and pressure
1 atm
Properties of gases
- Gases are fluids (substance that flows)
- Gases are highly compressible-can change its volume
- Gases completely fill their container (indefinite shape and volume)
- Gases have lower densities than liquids and solids
KMT
Describes the motion of particles
Main assumptions of KMT
- Gas molecules are in constant random motion
- Gas molecules are separated by large distances
- No attractive or repulsive forces
- Gases are made of molecules that have mass
- Molecules undergo elastic collisions (when they collide, no energy is lost, only transferred)
Relationship between temperature and kinetic energy
Directly proportional
Solid
Particles vibrate but don’t move past each other
Definite shape
Definite volume
Lowest KE
Boyle’s Law
P1V1=P2V2
Volume and pressure of a gas are inversely proportional
Charles’ Law
V1/T1=V2/T2
For a fixed amount of gas at a constant pressure, the volume of a gas is directly proportional to the temperature
Gay-Lussac Law
P1/T1=P2/T2
For a fized amount of gas at a constant volume, the pressure of a gas is directly proportional to the temperature
Combined Gas Law
P1V1/T1=P2V2/T2
Ideal Gas Law
PV=nRT
Dalton’s Law of Partial Pressure
The total pressure of a mizture of gases is equal to the sum of the pressure of the individual gases
