# Chapt. 15: Chemical Kinetics

## Chapt. 15: Chemical Kinetics

by 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

### Recommended Maps

## Create your own maps

with MindMeister

Get Started
## Create your own maps

with MindMeister

Get Started