1. Chapter 5
Gases

2. Pressure barometer – measures atmospheric pressure
manometer – measures gas pressure
units of pressures are: mmHg, Pa, atm and Torr
760 mmHg = 760 Torr = 1 atm = kPa
Page 235: # 37 a-c

3. Boyle’s Law PV = k where K is called Boyle’s constant P1V1 = P2V2
holds true only at low pressures
Look over example 5.3 on page 195
Page 235: #43

4. Charles’ Law V1/T1 = V2/T2 temperature must be in Kelvins
Page 236: # 44

5. Gay-Lussac’s Law
P1/T1 = P2/T2
Temperature must be in Kelvins

6. Avogadro’s Law
V1/n1 = V2/n2
Page 236: # 45 & 46

7. Combined Gas Law
P1V1/T1 = P2V2/T2
Temperature must be in Kelvins

8. Ideal Gas Law PV = nRT R = 0.8206 L atm K-1 mol-1
useful only at LOW pressure and HIGH temperatures (this will be an AP question)
Page 236: #49

9. Gas Stoichiometry
Page 237: #67

10. Gas Density & Molar Mass
MM = dRT/P
Page 237: # 77 & 79

11. Dalton’s Law …of partial pressures Ptotal = P1 + P2 + …
look over example 5.16 on page 212
Page 237: # 72

12. Kinetic Molecular Theory
All particles are in constant, random motion
All collisions between particles are elastic
The volume of the gas particles is negligible
Average kinetic energy is proportionate to it Kelvin temeperature
Average velocity of gas molecules = root mean square velocity = urms = 3RT/MM
R = 8.31 J/K mol
Page 240: # 109

13. Effusion & Diffusion diffusion – mixing of gases
effusion – passage of a gas through a tiny hole into an evacuated chamber
Graham’s law : rateA/rateB = MMB/MMA
Page 240: # 111

14. Real Gases act like ideal gases at LOW pressures and HIGH temperatures
look over van der Waals Equation on page 225