Chemistry - Gas Chapter

Kinetic Molecular Theory

Kinetic Molecular Theory

Describes the motion of all molecules & atoms not matter the phase of matter

Activation energy

The minimum energy colliding particles must have in order to react

Reaction rate

The number of atoms, ions, or molecules that react in a given time to form products

How can reaction rates be increased?

Increasing the number, force, or effectiveness of collisions

What affects reaction rates?

Concentration & surface area

Gas properties

1) Gas has mass

2) Gases can be compressed

3) They are fluid

4) Gases expand

5) Diffusion

Diffusion

Gases spread out uniformly without aide of air movement

Avogardo’s Law has constant…

… temperature & pressure; direct proportion

Boyles’s Law has constant…

… temperature; inverse proportion

Charles’s Law has constant…

… pressure; direct proportion

Gay-Lussacs Law has constant…

… volume; direct proportion

Dalton’s Law of Partial Pressure

The total amount of pressure is all the different gases’ pressures added up together

Graham’s Law of Effusion

The rate of effusion for a gas is inversely proportional to the square root of its molar mass

Graham’s Law of Diffusion

The rate of diffusion for a gas is inversely proportional to the square root of its molar mass

What is the difference between diffusion and effusion?

Diffusion is when gas molecules disperse throughout a container, effusion is when a gas passes through an opening that is smaller than the mean free path of the particles