Chapt. 15: Chemical Kinetics

1. Reaction Rates

2. Catalysis

3. Rate Laws: A Summary

4. Rate Laws: An Introduction

5. Reaction Mechanisms

6. A Model for Chemical Kinetics

7. Determining the Form of the Rate Law

8. The Steady-State Approximation

9. The Integrated Rate Law

10. Rate=Change in Concentration/Time interval

11. Thermo: IF Kinetics: WHEN & HOW

12. Avoid complex kinetics by measuring initial rates

13. Rate Law: Rate=k[R]^n k & n must be determined experimentally

14. The rate law can provide information about the elementary steps of a reaction

15. Order=Sum of Exponents of Rate Law

16. 1st order half-life is independent of time or reactant concentration, 2nd order is not

17. Pseudo-first-order: make one reactant in a multireactant rxn rate-limiting

18. To test a proposed mechanism, compare the rate law of its slowest step with the experimentally determined rate law

19. Key Terms: elementary step, intermediate, molecularity & rate determining step

20. Reaction mechanisms can't be proven

21. At equilibrium: Keq=kforward/kreverse

22. Steady state: Rate of I production = Rate of I consumption

23. k=AExp(-Ea/RT)

24. Reaction Energy Diagram

25. Catalysts create a new reaction pathway with a lower activation energy