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Review Test: Chapter 12 and 13 - Concentration Units, Henry's Law, Colligative Properties, Kinetics

This review test covers topics such as concentration units, Henry's Law, colligative properties, and kinetics. It includes multiple-choice and show-work problems. Scantron required.

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Review Test: Chapter 12 and 13 - Concentration Units, Henry's Law, Colligative Properties, Kinetics

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  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 x 100% moles of solute liters of solution moles of solute m = mass of solvent (kg) M = mass of solute mass of solute + mass of solvent Molarity(M) Mole Fraction (X) Molality(m) moles solute (i) Mole % of A = mole fraction A*100 Xi = Total moles in solution • Percent by volume: milliliters of solute/millilitersof solution (then multiplied by 100%) • Mass/volume percent: gramsof solute/milliliters of solution (then multiplied by 100%) Weight (mass) % % 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. Boiling-Point Elevation DTb = iKbm Freezing-Point Depression DTf = i Kfm Vapor-Pressure Lowering p = iMRT Osmotic Pressure (p) Boiling-Point Elevation DTb = Kbm 0 P1 = X1 P 1 Freezing-Point Depression DTf = Kfm p = MRT Osmotic Pressure (p) 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. Electrolyte/IONIC Substance Solutions (i is Vant Hoff factor) 4

  5. Chapter 12 Kinetics Average Rate aA + bBcC + dD In general for the reaction: (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. 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) Eais 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

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