1. Review 1 For test 1 Chapter 12 and 13
Test will have part 1 Multiple choice and part 2 show work problems
One can receive partial credit in Multiple choice if work is shown or concept is explained
BRING A SCANTRON

2. Concentration Units Mole Fraction (X) M = moles of solute
liters of solution
m =
mass of solvent (kg)
Molarity (M)
Molality (m)
Weight (mass) %
x 100%
mass of solute
mass of solute + mass of solvent Xi =
moles solute (i)
Total moles in solution
Mole Fraction (X)
Mole % of A = mole fraction A*100
Percent by volume: milliliters of solute/milliliters of solution (then multiplied by 100%)
Mass/volume percent: grams of solute/milliliters of solution (then multiplied by 100%)
% by mass =

3. Henry’s law for Gas solubility Sg (mol/L) Sg =KHPg
ROULT’s Law
Psolution = Xsolvent  Posolvent
Psolution = the vapor pressure of a mixture of solute and solvent
Po = the vapor pressure of the pure solvent
Xsolvent = the mole fraction of the solvent.
If 2 liquids A and B are mixed then Vapor of each of them in the mixture are
PA = XA P0A PB = XB P0B Ptotal = PA ++ PB

4. Colligative Properties of Nonelectrolyte Solutions
Colligative properties are properties that depend only on the number of solute particles in solution and not on the nature of the solute particles.
Vapor-Pressure Lowering
P1 = X1 P 1
Boiling-Point Elevation
DTb = Kb m
Freezing-Point Depression
DTf = Kf m
Osmotic Pressure (p)
p = MRT
Electrolyte/IONIC Substance Solutions (i is Vant Hoff factor)
Boiling-Point Elevation
DTb = i Kb m
Freezing-Point Depression
DTf = i Kf m
Osmotic Pressure (p)
p = iMRT 4

5. In general for the reaction:
Chapter 12 Kinetics
Average Rate
In general for the reaction:
aA + bB  cC + dD
(M/s)
Initial Rate
x and y are the reactant orders determined from experiment. x and y are NOT the stoichiometric coefficients.

6. Insert Table 13.2

7. Both A and Ea are specific to a given reaction.
The Arrhenius Equation
k is the rate constant
T is the temperature in K
R is the ideal-gas constant (8.314 J/Kmol)
Ea is the activation energy
A is known the frequency or pre–exponential factor
Both A and Ea are specific to a given reaction.

8. Uncatalyzed reaction Catalyzed reaction Catalysts
Lowers activation energy
Changes Reaction mechanism
But does not change Enthalpy
Speeds up reaction
Reaction Mechanisms, Overall Reaction, Molecularity (unimolecular, bi molecular etc for each
Step in a multistep reaction pathway)
Intermediates
Rate Detreminating step is the slowest step and makes up the overall reaction rate law.
Difference between a CATALYST vs Intermediate