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Understanding Chemical Kinetics: Reaction Rates, Temperature Effects, and Mechanisms

This chapter explores the fundamentals of chemical kinetics, emphasizing the rates of chemical reactions and the influence of various factors, particularly temperature. It covers key concepts such as rate expressions, initial rates, slope analyses, and integrated rate equations for zero, first, and second-order reactions. Additionally, the chapter delves into the effects of catalysts, activation energy, and the Arrhenius equation. Through exercises and graphical methods, students gain insights into reaction mechanisms, molecularity, and the importance of kinetic data in supporting or disproving proposed mechanisms.

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Understanding Chemical Kinetics: Reaction Rates, Temperature Effects, and Mechanisms

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Presentation Transcript

  1. Chapter 15 Chemical Kinetics

  2. Rates of Chemical Reactions

  3. The Effect of Temperature on Reaction

  4. Other Factors Affecting the Rates of reactions

  5. Rate Expression Initial Rate Slope of the tangent line

  6. Exercise 1

  7. Exercise 1

  8. Exercise 2 2 NO(g) + 2 H2(g)  N2(g) + 2 H2O(g)

  9. Integrated Rate Expressions Plot for shape of rate response Use in graphical methods

  10. Zero Order Rate Expression

  11. First Order Rate Expression Conc Vs Time

  12. Half Life

  13. Second Order Rate Expression Conc VS Time

  14. Effect of Temperature on the Rate Constant Increasing Concentration

  15. The Reaction Coordinate dAB AB A + B A A A B B B

  16. Temperature and Activation Energy

  17. Arrhenius Pre-exponential Factor

  18. Exercise 3

  19. Exercise 3

  20. Effect of Catalyst on the Rate Constant

  21. Catalytic Hydrogenation CH2=CH2 + H2 CH3-CH3

  22. Reaction Mechanisms

  23. The Bimolecular Substitution Reaction [Br····CH3····Cl]- BrCH3

  24. The Unimolecular Substitution Reaction [CH3]+ BLOCK + Br- + [CH3]+ BrCH3

  25. The Unimolecular Mechanism Requires an Intermediate This reaction has two transition states

  26. Exercise 4

  27. Exercise 4

  28. Exercise 4 Slope=-k = -1.244 min-1

  29. Concepts from Chapter 15 • Rate constants • Rate laws • Integrated rate equations • Zero-order, first-order and second-order reactions • Half life, t1/2 • Collision theory • Activation energy and the Arrhenius equation(s) • Catalysts • Reaction co-ordinates, intermediates and transition states • Reaction mechanisms and elementary steps • Molecularity - rate equations for elementary steps • Rate determining steps • Supporting/disproving a proposed mechanism using kinetic data

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