Chapt. 15: Chemical Kinetics
von Terrence Oas
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