CH353 - Physical Chemistry I
Spring 2012, Unique 52135

Lecture Summary, 23 April 2012

Unimolecular Reactions: Unimolecular reactions proceed through the Lindemann mechanism:

  1) R + R --> R* + R
  2) R* --> P

where the first elementary step is rate determining and the steady-state approximation is valid.  Depending on the concentration of the reactant R, this reaction will either be first order in [R] or second order in [R].   

Homogeneously Catalyzed Reactions:  Catalyzed reactions proceed at a faster rate than an uncatalyzed reaction because of the addition of a molecule which is neither made nor consumed in the reaction and does not appear in the reaction stoichiometry.  The catalyst changes the mechanism of the reaction versus the uncatalyzed version (i.e. results in a different series of elementary steps) and does appear in the expression for the rate law of the reaction.  The process of solving an analytical rate law using elementary reactions, the SSA, or FE is the same for catalyzed reactions as we have already seen for uncatalyzed reactions.