Kinetic Theory of Gases

Chemistry

Kinetic Theory of Gases (1)

1. Gas particle volume - particles have negligible volume compared to space between particles.

Kinetic Theory of Gases (2)

2. Particle Non-Attraction - particles are not attracted to one another.

Kinetic Theory of Gases (3)

3. Particle linear motion - Gas particles are in constant motion and move in straight lines until they collide.

Kinetic Theory of Gases (4)

4. Particle collisions - particle collisions are elastic (Kinetic energy is conserved. No energy is lost)

Kinetic Theory of Gases (5)

5. Average Kinetic Energy - kinetic energy of the particles is related to the temperature. *At absolute zero, all motion stops.

Ideal Gases

Name for gas if it follows all of the above assumptions.

Boyle's Law

(P1V1=P2V2) At a constant temp. the pressure and volume are inversely proportional.

-If one goes up, the other goes down (Compression of gas)

Charles' Law

(V1/T1=V2/T2) temperature and volume are directly proportional (with a constant pressure)

-As V increases, T increases, as v decreases, t decreases.

Gay - Lussac's Law

(P1/T1=P2/T2) temperature and pressure are directly proportional (at a constant volume) as t increases, p increases, as t decreases, p decreases. As temperature increases, collisions increase.

The Combined Gas Law

(P1V1/T1 = P2V2/T2) All 3 variables have the same relationship as the separate gas laws. P inversely proportional to V and directly proportional to T, V is directly proportional to T. Temp must be in K.