1. Chapter 15 Chemical Kinetics

2. Rates of Chemical Reactions

3. The Effect of Temperature on Reaction

4. Other Factors Affecting the Rates of reactions

5. Rate Expression Slope of the tangent line Initial Rate

6. Exercise 1 Time(min)[CH 3 COOPh] (mol/L) 00.55 0.250.42 0.50.31 0.750.23 10.17 1.250.12 1.50.085

7. Time(min)[CH 3 COOPh] (mol/L) 00.55 0.250.42 0.50.31 0.750.23 10.17 1.250.12 1.50.085 Exercise 1

8. Exercise 2 2 NO(g) + 2 H 2 (g)  N 2 (g) + 2 H 2 O(g) Reactant Concentration (mol/L)Rate of Appearance of N 2 (mol/L·s) [NO][H 2 ] Run 1:0.4200.1220.136 Run 2:0.2100.1220.0339 Run 3:0.2100.2440.0678 Run 4:0.1050.4880.0339

9. Use in graphical methods Plot for shape of rate response Integrated Rate Expressions

10. Zero Order Rate Expression

11. First Order Rate Expression Conc Vs Time

12. Half Life

13. Second Order Rate Expression Conc VS Time

14. Effect of Temperature on the Rate Constant Increasing Concentration

15. The Reaction Coordinate A + B AB A B d AB A B A B

16. Temperature and Activation Energy

17. Arrhenius Pre-exponential Factor

18. Exercise 3 Temp( o C)K(1/Ms) 2833.52*10 -7 3563.02*10 -5 3932.19*10 -4 4271.16*10 -3 5083.95*10 -2

19. Exercise 3 T( o C)T(K)k1/Tln k 2835563.52E-070.001799-14.8596 3566293.02E-050.00159-10.4077 3936662.19E-040.001502-8.42644 4277001.16E-030.001429-6.75934 5087813.95E-020.00128-3.23145

20. Effect of Catalyst on the Rate Constant

21. Catalytic Hydrogenation CH 2 =CH 2 + H 2 CH 3 -CH 3

22. Elementary StepMolecularityRate Equation A  prod. UnimolecularRate = k[A] A + B  prod. BimolecularRate = k[A]·[B] A + A  prod. BimolecularRate = k[A] 2 2 A + B  prod. TermolecularRate = k[A] 2 ·[B] Reaction Mechanisms

23. The Bimolecular Substitution Reaction [Br····CH 3 ····Cl] - BrCH 3

24. The Unimolecular Substitution Reaction Br - + [CH 3 ] + BrCH 3 + BLOCK [CH 3 ] +

25. This reaction has two transition states The Unimolecular Mechanism Requires an Intermediate

26. Exercise 4

27. Time (min)[PhAc] (mol/L)ln[PhAc]1/[PhAc] 0.000.55-0.597837001.81818182 0.250.42-0.867500572.38095238 0.500.31-1.171182983.22580645 0.750.23-1.469675974.34782609 1.000.17-1.771956845.88235294 1.250.12-2.120263548.33333333 1.500.085-2.4651040211.7647059

28. Slope=-k = -1.244 min -1 Exercise 4

29. Concepts from Chapter 15 Rate constants Rate laws Integrated rate equations Zero-order, first-order and second-order reactions Half life, t 1/2 Collision theory Activation energy and the Arrhenius equation(s) Catalysts Reaction co-ordinates, intermediates and transition states Reaction mechanisms and elementary steps Molecularity - rate equations for elementary steps Rate determining steps Supporting/disproving a proposed mechanism using kinetic data