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## Chapter 15 Chemical Kinetics

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**Chapter 15**Chemical Kinetics**Rate Expression**Initial Rate Slope of the tangent line**Exercise 2**2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)**Integrated Rate Expressions**Plot for shape of rate response Use in graphical methods**First Order Rate Expression**Conc Vs Time**Second Order Rate Expression**Conc VS Time**Effect of Temperature on the Rate Constant**Increasing Concentration**The Reaction Coordinate**dAB AB A + B A A A B B B**Catalytic Hydrogenation**CH2=CH2 + H2 CH3-CH3**The Bimolecular Substitution Reaction**[Br····CH3····Cl]- BrCH3**The Unimolecular Substitution Reaction**[CH3]+ BLOCK + Br- + [CH3]+ BrCH3**The Unimolecular Mechanism Requires an Intermediate**This reaction has two transition states**Exercise 4**Slope=-k = -1.244 min-1**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