Chapter 14: Chemical kinetics

Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: Reactant concentration, temperature, action of catalysts, and surface area. Invite you to consult. | Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Chapter 14 David P. White University of North Carolina, Wilmington 1 1 1 1 Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: reactant concentration, temperature, action of catalysts, and surface area. Goal: to understand chemical reactions at the molecular level. Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates Speed of a reaction is measured by the change in concentration with time. For a reaction A B Suppose A reacts to form B. Let us begin with mol A. Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates At t = 0 (time zero) there is mol A (100 red spheres) and no B present. At t = 20 min, there is mol A and mol B. At t = 40 min, . | Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Chapter 14 David P. White University of North Carolina, Wilmington 1 1 1 1 Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: reactant concentration, temperature, action of catalysts, and surface area. Goal: to understand chemical reactions at the molecular level. Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates Speed of a reaction is measured by the change in concentration with time. For a reaction A B Suppose A reacts to form B. Let us begin with mol A. Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates At t = 0 (time zero) there is mol A (100 red spheres) and no B present. At t = 20 min, there is mol A and mol B. At t = 40 min, there is mol A and mol B. Calculating, Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates For the reaction A B there are two ways of measuring rate: the speed at which the products appear (. change in moles of B per unit time), or the speed at which the reactants disappear (. the change in moles of A per unit time). A plot of number of moles versus time shows that as the reactants (red A) disappear, the products (blue B) appear. Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Reaction Rates Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Rates in Terms of Concentrations For the reaction A B there are two ways of Most useful units for rates are to look at molarity. Since volume is constant, molarity and moles are directly proportional. Consider: C4H9Cl(aq) + H2O(l) C4H9OH(aq) + HCl(aq) Copyright 1999, PRENTICE HALL Chapter 14 Chemical Kinetics Rates in Terms of Concentrations C4H9Cl(aq) + H2O(l) .