CHEM 104 1st EditionExam # 2 Study Guide Chapters: 14 - 15 Topics- Chemical kinetics (chapter 14)o Definition of chemical kinetics o Factors that influence reaction rates o Definition of reaction rateo Equation for reaction rateso Generalized graph for reaction rates o Definition of the rate law o Equation for rate laws o Reaction order for each reactant, overall reaction order o Initial rates method for determining rate law (determine order of each reactant and rate constant k)o Integrated rate law method (deriving information from equations given)o Definition of integrated rate law method o Half life of different orders of reactions o Requirements that need to be met for a reaction to happen o Definition of elementary reaction o Definition of molecularity, typeso Definition of activation energy, transition state/activated complexo Activation energy graph (decoding information from the graph) o Relationship between temperature and reaction rate, cause of relationship o Arrhenius equation, how to manipulate it o Graph of ln(k) vs. 1/To Definition of reaction mechanisms o Requirements for a valid mechanism o Difference and meaning of slow steps (i.e. rate-determining) compared to fast steps within a reaction mechanism These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.o How to derive the rate law given the reaction mechanism (both when the first step is theslow step, and when the slow step is following a fast equilibrium step) o Definition of catalysis o How catalysts affect reaction mechanisms and activation energies o Differences between homogeneous and heterogeneous catalysis o Definition of enzymes, characteristics o Definition of substrate and active site o Processes through which enzymes can become inactiveo Generalized reaction mechanism for enzymes/substrates/enzyme-substrate complexes - Chemical equilibrium (chapter 15) o Characteristics of chemical equilibriumo Relationship between rates and chemical equilibrium (and generalized graph to visualize) o Law of mass action o Difference between law of mass action for homogeneous equilibrium systems and heterogeneous equilibrium systems o Equilibrium constants kc and kp (concentration and pressure) o Equation for the relationship between partial pressure and concentration o How equilibrium constants show whether reaction is reactant or product favored (depending on whether k is much larger than, equal to, or much smaller than 1) o Relationship of equilibrium constants and temperature o Definition of Le Chatelier’s principle o Different system changes that Le Chatelier’s principle can be applied to (changes in concentration, pressure, or temperature) o Definition and equation for reaction quotient, relationship of Q and K o Effect of catalysts in relation to Le Chatelier’s principleo Application of Le Chatelier’s principle: Haber-Bosch process (i.e. ammonia symthesis)o Manipulating k (reversed reaction, adding chemical equations, different ways to balance equations)Using ICE (stands for initial concentration, change in concentration, equilibrium concentration) tables to determine