Kinetic Molecular Theory of Gases This is the six point model that is used to explain the behavior of gases Points of the Kinetic Molecular Theory 1 Gases are composed of atoms or molecules that have mass ID: 815050
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Slide1
The Nature of Gases
Slide2List 5 Properties of Gases
Slide3Kinetic Molecular Theory of Gases
This is the six point model that is used to explain the behavior of gases
Slide4Points of the Kinetic Molecular Theory
1. Gases are composed of atoms or molecules that have mass
2. Gases are in constant, random, straight line motion
3. The particles that make up a sample of a gas are separated from each other by great distances
This is why the volume is NOT FIXED
Slide5Continuing the points
4. Gas particles collide with each other and the container that they are in
All of these collisions result in a transfer of energy from particle to particle
Or from particle to surroundings
No energy is ever lost completely and these are called ELASTIC COLLISIONS.
Slide6Continuing
5. Gas particles have no attraction for each other
6. Gases are highly sensitive to changes in temperature and pressure
Slide7How is an “ideal” gas different from a “Real’ Gas?
Ideal gases follow all of the rules for gas behavior
Hydrogen and Helium are the two most ideal gases that exist
Real Gases do not always follow each of the six points of KMT.
Slide8Exceptions to the KMT
1. Sometimes the particles in a mixture of gases are attracted to each other because of differences between elements
This is especially true during temperature or pressure changes
Slide9Exception #2
As the pressure that is on a sample of a gas increases we begin to confine the gas to a smaller space
Once trapped in a smaller space, gases will have a volume that we can measure
Slide10What set of conditions make gases most “Ideal”
Gases are most ideal when we have:
HIGH TEMPERATURE AND LOW PRESSURE
Under these conditions they follow the points of KMT the best.
So……400 K and 0.1 atm is good
But…...3 K and 100 atm is NOT GOOD
So Low Temperature and High pressure is when they are least ideal.