CHM 104 1st Edition Lecture 8 Outline of Last Lecture I Reaction Mechanism where rate determining step is not the first step II Homogeneous Catalysis III Heterogeneous Catalysis IV Hydrogenation of ethylene V Enzymatic catalysis Outline of Current Lecture VI Chemical Equilibria Current Lecture 2NO2 N2O4 What is happening 2NO2 N2O4 Will start FAST and slow down over time Build up of N2O4 N2O4 2NO2 Will start slow and speed up to match rate of forward reaction Rate at equilibrium forward Rate at equilibrium reverse kf NO2 2eq kr N2O4 eq f forward r reverse and eq equilibrium K equilibrium constant 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 In General Law of Mass Action aA bB cC dD All are concentrations AFTER an equilibrium has been established K unitless too many different units always positive concentrations are always 0 range 0 infinity The value of K tells us if the reaction favors products or reactants at equilibrium Example H2 Br2 2HBr K 1 9 x 1019 1 Reverse the equation inverse K 2 Multiply the coefficient in the reaction by a factor of n raise K to power of n 3 Add 2 reaction with known K values together multiply the K values together
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