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Similaire à Ch17 hrw rxn kinetics
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Ch17 hrw rxn kinetics
- 1. Chapter 17 pp Reaction Kinetics
- 4. A Molecular Representation of the Elementary Steps in the Reaction of NO 2 and CO Overall: NO 2 + CO NO + CO 2 Step 1: NO 2 + NO 2 NO 3 + NO (k 1 ) Step 2: NO 3 + CO NO 2 + CO 2 (k 2 ) NO 3 is an intermediate
- 11. Definition of Rate. 2NO 2 2NO + O 2
- 13. Tr96 Fig. 17-9 p. 533 Possible Collision Patterns
- 14. Several Possible Orientations for a Collision Between Two BrNO Molecules. (a) & (b) can lead to a collision, (c) cannot.
- 15. No Reaction O N Br O N Br O N Br O N Br O N Br O N Br O N Br O N Br O N Br O N Br
- 18. Energy Reaction coordinate Reactants Products
- 19. Energy Reaction coordinate Reactants Products Activation Energy - Minimum energy to make the reaction happen
- 20. Energy Reaction coordinate Reactants Products Activated Complex or Transition State
- 21. Energy Reaction coordinate Reactants Products Overall energy change
- 63. Energy Reaction coordinate Reactants Products
- 65. Energy Plots for a Catalyzed and an Uncatalyzed Pathway for a Given Reaction. ∆ E is the same in both cases!
- 69. Catalysts Pt surface H H H H C H H C H H
- 72. Catalysts Pt surface H C H H C H H H H H
- 81. Definition of Rate. 2NO 2 2NO + O 2
- 95. A Molecular Representation of the Elementary Steps in the Reaction of NO 2 and CO Overall: NO 2 + CO NO + CO 2 Step 1: NO 2 + NO 2 NO 3 + NO (k 1 ) Step 2: NO 3 + CO NO 2 + CO 2 (k 2 ) NO 3 is an intermediate
- 108. Second step is slow High activation energy E a
- 109. E a Third step is fast Low activation energy
- 110. Second step is rate determining
- 112. Activated Complexes or Transition States
- 114. Nuclear Review for Star Test
Notes de l'éditeur
- Hrw 511
- Hrw 531
- Hrw 531; z53 Section 12.6 Reaction Mechanisms Z5e 583
- Fig. 12.9 Z5e 584 NO 2 + NO 2 ---> NO 3 + NO (k 1 ) NO 3 + CO ---> NO 2 + CO 2 (k 2 ) NO 3 is an intermediate Each rx called an elementary step ; I.e., its rate law can be written from its molecularity Molecularity is defined as the # of species that must collide to produce the rxn indicated by that step.
- Z5e 584
- Z5e 585.
- i.e., 3 moles of H 2 are being consumed for every 1 mole of N 2
- Z5e Fig. 12.1 Definition of Rate Z5e 562
- Hrw 532
- Fig. 12.13 Z5e 589 (a) and (b) lead to a reaction, but (c) cannot.
- Hrw 534
- Hrw 534
- Hrw 562-563
- Vonderbrink PL 17
- Hrw 705-707; z5e 1024-1025
- Hrw 706; z5e 1024
- Hrw 706; z5e 1024-1025
- Hrw 707; z5e 1024-1025
- Hrw 686; z5e 1083
- Hrw 686
- Hrw 538
- Z5e 559
- Hrw 538
- Hrw 539
- Hrw 539
- Hrw 540
- Hrw 540
- Hrw 540 Section 12.8 Catalysis Z5e 592
- Fig. 12.15 Z5e 593
- Hrw 541
- Hwr 541
- Z5e 594
- Z5e 598
- Hrw 541 Section 12.2 Rate Laws Z5e 564 When fwd & rev rxn rates are equal then no change in conc. of either --> equilibrium Rate = k [H 2 ] m [NH 3 ] n Note: “m” and “n” are not coefficients of the balanced equation
- Hrw 541
- Hrw 541
- “ n” is not the coefficient of the balanced reaction. Rf. Z5e 566
- Z5e Fig. 12.1 Definition of Rate Z5e 562
- Section 12.3 Determining the Form of the Rate Law Z5e 567
- Z5e 568
- Hrw 541-542 Z5e 570 SE 1.
- Rf. SE 12.1 Z5e 570 Be able to write the rate law (using variables) from the reaction !
- See SE 12.1 Z5e 570
- See SE 12.1 Z5e 570
- See SE 12.1 Z5e 570
- See SE 12.1 Z5e 570
- Hrw 542
- Hrw 542 Z5e Section 12.6 Reaction Mechanisms Z5e 583
- Hrw 542-543 Fig. 12.9 Z5e 584 NO 2 + NO 2 ---> NO 3 + NO (k 1 ) NO 3 + CO ---> NO 2 + CO 2 (k 2 ) NO 3 is an intermediate Each rx called an elementary step ; I.e., its rate law can be written from its molecularity Molecularity is defined as the # of species that must collide to produce the rxn indicated by that step.
- See Hrw 544 SP 17-6
- Z5e 584
- See Hrw 544 SP 17-6
- Rf. Table 12.7 Z5e 585
- Z5e 585.
- Hrw 544 SP 17-7
- Hrw 544 SP 17-7
- Hrw 544 Addl SP 17-7 #2
- Hrw 544 Addl SP 17-7 #3
- Hrw 705-707; z5e 1024-1025
- Hrw 706; z5e 1024
- Hrw 706; z5e 1024-1025
- Hrw 707; z5e 1024-1025