Chemical Kinetics

35 lessons, pages 2096–2130.

  1. What Reaction Rate Measures — Concentration change per time and stoichiometric normalization
  2. Average and Instantaneous Rates — Secant slopes, tangent slopes and concentration-time graphs
  3. Rate Units and Measurement — Concentration, time and experimental signals
  4. Factors Affecting Rate — Concentration, temperature, surface area and catalyst effects
  5. Rate Laws from Experiments — Empirical concentration dependence and rate constants
  6. Initial-Rates Method — Finding orders by controlled comparisons of initial rates
  7. Reaction Order and Units of k — Overall order and dimensional consistency of rate constants
  8. Molecularity Versus Reaction Order — Elementary-step particle count compared with measured overall order
  9. Zero-Order Integrated Rate Law — Linear concentration decline and zero-order half-life
  10. First-Order Integrated Rate Law — Exponential decay, ln concentration plot and half-life
  11. Second-Order Integrated Rate Law — Reciprocal-concentration plot and concentration-dependent half-life
  12. Using Graphs to Identify Order — Comparing concentration, log and reciprocal plots
  13. Half-Life Across Reaction Orders — Contrasting zero-, first- and second-order half-life formulas
  14. Pseudo-First-Order Conditions — Excess reactant approximation and observed rate constants
  15. Temperature and Rate Constants — Rate change with temperature without confusing equilibrium
  16. Arrhenius Equation — Activation energy, pre-exponential factor and exponential temperature dependence
  17. Arrhenius Plots — Extracting activation energy from ln k versus inverse temperature
  18. Two-Temperature Arrhenius Calculations — Estimating k ratios and activation energy from two temperatures
  19. Collision Theory — Effective collisions, orientation and energy thresholds
  20. Activation Energy and Energy Profiles — Forward and reverse barriers on reaction-coordinate diagrams
  21. Catalysts and Alternative Pathways — Lower barriers, unchanged equilibrium and catalyst regeneration
  22. Homogeneous and Heterogeneous Catalysis — Same-phase pathways versus surface adsorption steps
  23. Elementary Steps and Mechanisms — Writing mechanisms whose steps sum to an overall reaction
  24. Intermediates and Catalysts in Mechanisms — Species formed and consumed versus species regenerated
  25. Rate-Determining Steps — Slow-step approximations and their limitations
  26. Pre-Equilibrium Approximation — Deriving a rate law from a fast initial equilibrium
  27. Steady-State Approximation — Estimating low intermediate concentrations from production and consumption
  28. Parallel and Consecutive Reactions — Competing pathways, intermediates and product distributions
  29. Reversible Reaction Rates — Forward and reverse rates approaching dynamic equilibrium
  30. Gas-Phase Kinetics — Partial pressures, concentration conversion and gas reaction rates
  31. Solution Kinetics and Ionic Strength — Solvent, mixing and ionic-environment effects on observed rates
  32. Photochemical Reaction Rates — Photon absorption, light intensity and quantum yield
  33. Experimental Kinetics Design — Controlling variables, repeat measurements and uncertainty
  34. Kinetics Problem-Solving Workshop — Choosing rate-law, integrated-law and Arrhenius methods from data
  35. Chemical Kinetics: Unit Review — Connecting rates, mechanisms, temperature and catalysis