CHEM 1050 Lecture Notes - Lecture 33: Stoichiometry, Rate Equation, Reaction Rate Constant

• School: University of Guelph
• Department: Chemistry
• Course: CHEM 1050
• Professor: Rick De Laat

Document Summary

Involves a series of steps where each step is an elementary process. Add up all steps to get the overall reacion (certain products cancel out) Elementary step: a single step with no intermediates. Once you know a reacion is elementary-through experimental determinaion- then the rate law is derived from the stoichiometry of the elementary reacion (rate law can never be determined from the stoichiometry unless an elementary reacion) Overall order of the reacion=molecularity of the reacion. Example: no + o3 no2 + o2 rate=k[no][o3] overall order=2, bimolecular. The sequence of elementary reacions should always convert reactants to products i. e. , forward direcion. Suggested reacion mechanisms should always match up with experimental rate laws for any given reacion. One molecule breaks apart/decomposes to give products. Example: no + o3 no2 + o2: termolecular reacions. Three molecules react together at the same ime in one step. This is a rare situaion and we will not deal with it oten.