CHEM 1212 1nd EditionExam # 2 Study Guide Lectures: 7-16Chapter 15 - If the concentration of a reactant is increased, the reaction rate will often increase as well- Chemical reactions occur more rapidly at higher temperatures- Rate law equation: k[A]m[B]n- Homogeneous catalyst is included in rate equations- In zero order reactions, the reaction rate is independent of the reactant concentration- 1st order integrated rate equation: ln[R]t/[R]0 = -kt- 2nd order integrated rate equation: 1/[R]t – 1/[R]0 = kt- 0 order integrated rate equation: [R]0 – [R]t = kt- Orders determined from graphso Find one with straight lineo If straight line is on graph of [R]t vs. t, then it is 0 ordero If straight line is on ln[R]t vs. t, the it is 1st ordero If straight line is on 1/[R]t vs. t, then it is 2nd order- Half lifeo Longer half life = slower reactiono Usually involving 1st order processeso Half life and 1st order k t1/2 = .693/K t1/2 is independent of concentration- The Arrhenius Equationo K = rate constant = Ae-Ea/RTo Frequency factor (A) is temperature independento Ln(K2/K1) = -Ea/R[(1/T2) – (1/T1)]Chapter 16- Equilibrium constant, Ko K = [C]c[D]d/[A]a[B]b- Solids not included in equilibrium (K) equation- Water is not included in equilibrium (K) equation- Kp = PcPd/PaPbo Kp = concentrations in partial pressure- K > 1 = product favored- K < 1 = reactant favored- Reaction quotient, Q (used when reaction is not at equilibrium)o Q = [C]c[D]d/[A]a[B]b- If Q < K then reactants must be converted to products to reach equilibrium- If Q > K then products much be converted to reactants to reach equilibrium- When stoichiometric coefficients of a balanced equation are multiplied by some factor, the Knew is the Kold raised to the power of the multiplication factor- The equilibrium constants for a reaction and its reverse are the reciprocals of one another- When two or more chemical equations are added to produce a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants for the added equationsChapter 17- In a neutral solution, [H3O+] = [OH] = 1.0x10-7o Together = 1.0x10-14- In acidic solution, hydronium concentration is greater than OH concentration- In basic solution, hydronium concentration is less than the OH concentration- pH scaleo pH = -log[H3O+]o pH 7 = neutralo pOH = -log[OH-]o pKw = 14.00 = pH + pOHo pH < 7 = acidico pH > 7 = basic- Ionization constanto Ka = [H3O+][A-]/[HA]o Ka < 1 = weak acido Kb = [BH+][OH-]/[B]o The weaker the acid, the stronger the conjugate baseo pKa = -logKao As Ka increases, acid strength increaseso As pKa decreases, acid strength increaseso Ka x Kb = Kw Kw = 1.0x10-14- Acid base reactionso Mixing equal amounts (moles) of a strong base and strong acid produces a neutral