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

2. Reaction Pathways
Figure 4 Page 564:

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

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

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

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

7. Exothermic vs. Endothermic

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

9. 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

10. 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?

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

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