CHEM 104 1st Edition Exam 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 rate o Equation for reaction rates o 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 types o Definition of activation energy transition state activated complex o 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 T o 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 the slow 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 inactive o Generalized reaction mechanism for enzymes substrates enzyme substrate complexes Chemical equilibrium chapter 15 o Characteristics of chemical equilibrium o 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 principle o 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 unknowns
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