Chemistry Chapter 17 – Reaction Kinetics South Lake High School Ms. Sanders

Reaction Pathways Figure 4 Page 564:

Reaction Pathways Ea = activation energy ∆E = energy change in reaction ∆Eforward = Eproducts – Ereactants ∆Ereverse = Ereactants - Eproducts

Energy Diagram Practice Practice page 567 1a) Draw and label: ∆Eforward, ∆Ereverse, Ea, and Ea’

Energy Diagram Practice Continue Practice page 567 1a) Determine the values for: ∆Eforward, ∆Ereverse, Ea, and Ea’

Energy Diagram Practice Continue Practice page 567 1b)Is the forward reaction exothermic or endothermic? Explain.

Exothermic vs. Endothermic

Reaction Rate Factors Affecting Reaction Rate – Nature of reactants Surface area Temperature Concentration Presence of a catalyst

Reaction Rate Rate Law – An equation that relates reaction rate and concentration of reactants R = k[A]ⁿ[B]ᵐ R – reaction rate k – specific rate constant [A] & [B] – molar concentrations of reactants n & m – order of the reaction

Reaction Rate Practice Page 574 1) 3A C [A] = 0.2M, R = 1.0M/s; [A] is doubled = 0.4M, R = 4.0M/s; What is the rate law?

Review Reaction Rate R = k[A]ⁿ[B]ᵐ Page 574 – Sample Problem B

Review Energy Diagram Practice page 567 2) Ea = 125 kJ/mole; Ea’ = 86 kJ/mole; reactants at 0