Unit 5 – Gases
11.1
- states of matter and motion: solid – vibrate, liquid – rotate, gas – translate
- attractions between the particles
- kinetic molecular theory of gases
11.2, 11.4, 11.5
- components of the atmosphere
- greenhouse effect and global warming
- air quality, smog, pollutants; AQHI
- indoor air quality and factors that compromise it
11.7
- air pressure, evidence of atmospheric pressure, measuring air pressure
- history: changes in atmospheric pressure and the barometer
- units: 101.3 kPa = 1 atm = 760 torr = 760 mmHg
- STP and SATP
11.8
- temperature, Celsius and the Kelvin (absolute) scale, absolute zero
- Charles’ Law: V1/T1 = V2/T2 (T is in Kelvin), balloon
11.9
- Boyle’s Law: P1V1 = P2V2, piston
- Gay-Lussac’s Law: P1/T1 = P2/T2 (T is in Kelvin), scuba tank
- combined gas law: P1V1/T1 = P2V2/T2 (T is in Kelvin)
12.1
- Gay-Lussac’s Law of Combining Volumes: gases combine in small, whole number ratios
- Avogadro’s Law V1/n1 = V2/n2
- Avogadro’s Law V1/n1 = V2/n2
- molar volume is 22.4 L/mol, calculate  #L = n x 22.4L/mol at STP
- density, D = MM/MV
- Avogadro’s Hypothesis: equal volumes of gases contain an equal number of particles
12.2
- real vs. ideal gases - why a real gas deviates from an ideal gas
- ideal gas law: PV = nRT, R is the universal gas constant
12.4
- Dalton’s Law of partial pressures: P1 + P2 + P3 = PTotal
- collecting a gas over water: Pgas  Ptotal - PH2O (Dalton Law of PP)
12.5
- stoichiometry, n may be calculated in 4 equations (12.1 and 12.2)
- MM = m/n, to determine the MM of a gas