CHEM 1050 Lecture Notes - Lecture 35: Rate-Determining Step, Rate Equation, Molecularity
24 Dec 2016
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No + o3 no2 + o2. When there"s only one step, that step is now the slow step" rate determining step is the slowest step. Multistep reactions reaction of no2 and co. No2 + no2 no3 + no. No3 + co no2 + co2 [need to get rid of no3, since it"s an intermediate!] Overall: no2 + co no + co2. 2o3 + o 3o2 + o. = [o2] / t rate laws of multistep reactions recall: for unimolecular, a products if [a] goes up, its decomposition speed increases. 1st order rate = k[a] for bimolecular. A + b products or a + a products rate = k[a][b] or rate = k[a]2. Note: 2nd order follows from the fact that the rate of collision between a and b is proportional to [a] and [b] concentrations rate laws of multistep mechanisms. Overall rate of reaction cannot exceed the rate of the slowest step (rate- determining step)
