Chapter 12 Homework and Learning Objectives Honor Chemistry
Honor Chemistry Chapter 12 Learning Objectives
Chapter 12: Gases and Liquids
Chapter Opening: Ascent into the ozone
Using hot air balloons to collect data on the ever-changing ozone layer.
12.1
Kinetic Molecular Theory explains the properties of gases under ideal gas conditions.
Properties of Gases:
Gases are fluids
Gases have low density
Gases are highly compressible
Gases fill a container and exert pressure in all directions
Gas temperature determines the average kinetic energy of its particles
KE=1/2mv2
Mass=m, speed=v
Atmospheric Pressure
Pressure = Force/Area
SI unit of force = Newton (N)
SI unit of area= meters squared
SI unit of pressure = Pascal (Pa)
Barometer used to measure pressure, sealed column of mercury is used b/c of it’s high density. Density Hg=13.7g/mL.
Standard Temperature and Pressure (STP) 0 degrees Celsius and 1 atm
Units of Pressure and Equivalents
1 atm
14.7 lbs/in2
760 mmHg, (Torr)
101,325 Pascal (Pa)
101.325 KPa
Greenhouse effect:
Ozone Depletion:
12.2 Gas Laws
Review Temperature Conversions, Fahrenheit, Celsius, Kelvin
Gas law variables
P T V n
Boyle’s Law= P1V1=P2V2 Pg. 435 Sample and Practice Problems
Dalton’s Law of Partial Pressure= Ptotal=PA+PB+PC
Charles’ Law=V1/T1=V2/T2 (See graph pg. 439, direct relationship) (Unit for T = K)
Avogadro’s Law =1 mole of gas @STP=22.4L
Graham’s Law of effusion=rate of effusion for two gases are inversely proportional to the square roots of their molar masses at the same temp and pressure
Effusion=passage of a gas through a small opening
12.3
Pg. 447 Ideal Gas Law= PV=nRT
R= .0821 (L)(atm)/(mol)(K)
Pg. 448 Combined Gas Law= PV/nRT=PV/nRT (Units are important)
Complete Section Rv. Pg. 451
Gas Stoichiometry #48 pg. 463
