1. Gas Laws
The work of Boyles, Charles, Avogadro, Dalton and Graham explains the behavior of ideal gases.

2. Kinetic Molecular Theory
How gas particles behave under ideal conditions (Ideal gases)
Constantly moving in straight-line motion
undergo “elastic” collisions never losing energy
Particles are volumeless in relation to the space between them (the measurement of the space is the volume of the gas.)
no intermolecular attractions between particles

3. Ideal gases love summer!

4. Gases Deviate from Ideal Behavior a.k.a. “real gases”
low temperatures COLD
and high pressures SQUEEZED

5. 3 variables affect the behavior of gases
(P)ressure
Standard pressure measured at sea level = 1 atm = 101.3kPa = 760mmHg = 14.6psi
(T)emperature in Kelvin
Standard temp = 0oC = 273K
(V)olume in Liters
1 mol = 22.4L only if at STP

6. Boyle’s Law P1V1 = P2V2
…as temperature stays constant.

7. Inverse relationship between P & V …. When T stays the same

8. Charles’ Law

9. As pressure stays constant… what is the relationship between V & T?

10. V is directly proportional to T in Kelvin
V  T
V is directly proportional to T in Kelvin
Temperature K
Volume

12. constant volume
As heat energy is added, temperature increases and increases the average KE of the gas particles.
When the particles move faster they have more collisions with their container & collide with more force……therefore increasing pressure.

13. COMBINED Gas Laws

14. Practice
A sample of oxygen gas has a volume of 205mL when its temperature is 22.0oC and its pressure is 30.8kPa. What volume will the gas occupy at STP?

15. A sample of gas under a pressure of 8. 11atm has a volume of 312ml
A sample of gas under a pressure of 8.11atm has a volume of 312ml. The pressure is increased to 948kPa. What volume (in liters) will the gas occupy?

16. Practice
At a temperature of -33.0oC, a sample of confined gas exerts a pressure of 53.3kPa. If volume remains constant, at what temperature will the pressure reach 1.31kPa?

17. The End