Unit 10 Chem- 10.1
Kinetic Theory of matter
All mastter consists of tiny particles that are in constant random motion
Kinetic Energy
energy of motion
-Depends on the mass and speed of particles
Temperature
measure of the average KE of the particles in a substance
Kinetic Theory of Gases Assumption 1
Gas particles have negligible volume and are very far apart
- Gases are mostly empty space
Kinetic Theory of Gases Assumption 2
Gas particles are in constant, random motion
- move in straight paths
Kinetic Theory of Gases Assumption 3
Gas particles have elastic collisions
- no attractive forces between them
- They exert a pressure, but do not lose any kinetic energy
Gas pressure
result of gas particles colliding
- more collisions = more pressure
What can cause more collisions?
- More particles (higher density)
- Higher temp
- Decreased Volume/Space
Vacume
has no pressure b/c there are no molecules
Atmospheric pressure
caused by the force (weight) of air due to gravity
- same idea as water pressure
Standard Atmospheric Pressure
- Air pressure at sea level
- Equal to 1atm = 760mmHg = 101.3 KPa
STP
0 C and 1atm
Conversion Factors
0 C = 273K
1atm = 760 mm Hg
1atm = 101.3 kPa