CHEM 1002 Lecture Notes - Lecture 1: Reaction Rate, Activation Energy, Equilibrium Constant

• School: Carleton University
• Department: Chemistry
• Course: CHEM 1002
• Professor: Monica Patterson

Document Summary

Note here that since the stoichiometric coefficient for i- is 3, whereas its order is 1, the reaction does not occur as written, but must occur via some series of steps. The slowest step in the series, the rate limiting step, is the one which is first order in [h2o2] and first order in [i-]. The same is true for h+ in that the rate law does not appear to follow directly from the reaction stoichiometry. Determining the orders experimentally: e. g. take the reaction 2 no + o2 2 no2. The following data were collected in the lab: Find the rate equation and the value of the rate constant. Looking at the results of experiments 1 and 2, we see that if [no] is unchanged, but [o2] is doubled, the rate doubles. Looking at the results of experiments 1 and 3, we see that if [no] is doubled but [o2] is unchanged, the rate quadruples.