Chapt. 15: Chemical Kinetics

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

2. Reaction Energy Diagram

3. k=AExp(-Ea/RT)

4. Catalysis

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

6. A Model for Chemical Kinetics

7. The Steady-State Approximation

8. At equilibrium: Keq=kforward/kreverse

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

10. Reaction Mechanisms

11. Reaction mechanisms can't be proven

12. Rate Laws: A Summary

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

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

15. Thermo: IF Kinetics: WHEN & HOW

16. Rate=Change in Concentration/Time interval

17. Rate Laws: An Introduction

18. Reaction Rates

19. Avoid complex kinetics by measuring initial rates

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

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

22. Order=Sum of Exponents of Rate Law

23. 1st order half-life is independent of time or reactant concentration, 2nd order is not

24. Determining the Form of the Rate Law

25. The Integrated Rate Law