1. Review 1 For test 1 Chapter 14 and 15 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

2. Concentration Units % by mass = M = moles of solute liters of solution m = moles of solute mass of solvent (kg) Molarity (M) Molality (m) Weight (mass) % x 100% mass of solute mass of solute + mass of solvent XiXi = moles solute (i) Total moles in solution Mole Fraction (X) 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%)

3. Henry’s law for Gas solubility S g (mol/L) S g =K H  P g ROULT’s Law P solution = X solvent  P o P solution = the vapor pressure of a mixture of solute and solvent P o = the vapor pressure of the pure solvent X solvent = the mole fraction of the solvent. If 2 liquids A and B are mixed then Vapor of each of them in the mixture are P A = X A P 0 A P B = X B P 0 B

4. 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 P 1 = X 1 P 1 0 Boiling-Point Elevation  T b = K b m Freezing-Point Depression  T f = K f m Osmotic Pressure (  )  = CRT Boiling-Point Elevation  T b = i K b m Freezing-Point Depression  T f = i K f m Osmotic Pressure (  )  = iCRT Electrolyte Solutions (i is Vant Hoff factor)

5. Chapter 15 Kinetics aA + bB  cC + dD In general for the reaction: (M/s) Average Rate Initial Rate x and y are the reactant orders determined from experiment. x and y are NOT the stoichiometric coefficients.

6. Integrated Rate Laws- Remember the graphs!! Zero order kinetics Rate = k [A] o Rate =k [A] t  [A] o =  kt Half life t 1/2 = [A] o /2K unit of k =?? First order kinetics Rate = k [A] 1 ln[A] t = ln[A] o  kt Half life t 1/2 = 0.693/k unit of k =?? Second order kinetics Half life t 1/2 = 1/[A] o K unit of k =?? Rate = k [A] 2

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