CHEM 116 Lecture Notes - Lecture 2: Rate-Determining Step, Elementary Reaction, Reaction Step
Document Summary
Chemical equation that gives the starting and ending species of a reaction reaction proceeds via a series of steps call elementary reactions. Show how bonds are broken and formed rate of elementary reaction is given by its molecularity. Number of species taking place in an elementary step. A products rate = k[a] unimolecular. A + b products rate = k[a][b] bimolecular. A + b + c products rate = k[a][b][c] trimolecular intermediate species. Short lived species that appears in the reaction mechanism but is not in the chemical equation rate determining step. No2 + o3 o2 + no3. Reaction rate and temperature rate1 = k[no2][o3] (slow step, determines rate) rate2 = k[no3][no2] (fast step) the overall rate is rate1 for a reaction event to occur two species must collide with sufficient energy (activation energy) At a particular temperature, there is a distribution of energies. A0: pre exponent term (frequency factor), units are the same as k k: rate constant.
