CHE 102 Lecture Notes - Lecture 1: Kinetic Theory Of Gases, Rate Equation, Chemical Kinetics
Document Summary
Today: determination of rate law by integration, activation energy. Chemical kinetics is the study of rates of chemical processes, including chemical reactions and physical changes. reaction rate: the change in concentration of a reactant or product per unit time. For a given chemical, a positive sign means production of that chemical. A negative sign means consumption of that chemical. Kinetic molecular theory fits the observation of a reaction rate depending on the concentration of reactants: more reactants (higher concentration), faster rate, fewer reactants (lower concentration), slower rate. A rate law summarizes the relationship between reactant concentration and reaction rate. Cv+(aq) + oh-(aq) cvoh(aq) rate = k[cv+] 2 no2(g) + f2(g) 2 no2f(g) rate = k[no2][f2] The most common experimental methods: initial rates, integrated rate laws. Using calculus, we can derive mathematical expressions that can be graphed and that visually help us determine the rate law for a chemical process. 1st order rate law: rate = k[a] = [a] = d[a]
