# 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

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