1. Chemical Kinetics or Reaction Rates

2. You have 6 ball bearings with identical magnetic strength but different diameters where A > B > C > D > E > K. Which two will hold together the most & the least.

3. Reaction Rate The speed at which reactants become products in a chemical reaction M/s

4. Kinetic Theory All matter is made up of tiny particles The particles are in constant motion All collisions are elastic ?

5. Elastic Collisions Collisions in which there is no energy change

6. Particles Reacting For particles to react, they must collide Reaction rate is dependent on collision rate

7. Particles Reacting When a reaction takes place, an energy change occurs Collision in which reactions occur are not elastic

10. Reaction Rate Rate = - d[Reactant]/dt Rate = +d[Product]/dt M/s

13. Factors Affecting Rxn Rate Concentration, Temperature, Agitation, Process, Orientation, Catalyst, SA of Solid, Pressure of Gas, Reaction Mechanism

14. List & describe all of the factors affecting rxn rates.

16. Drill: List at least 5 factors that will affect reaction rates

17. Rate Expression An equation showing how rate depends on the amount of reactants in a rate determining reaction

18. Rate Expression Rxn: aA (aq) + bB (aq) P Expr: Rate = k[A] a [B] b [A] = molarity of A

19. Rate Expression Rxn: aA (g) + bB (g) Product Exp: Rate = kP A a P B b

20. Write Rate Expressions for: H 2(g) + N 2(g) NH 3(g) HCl (aq) + Ba(OH) 2(aq) BaCl 2(aq) + H 2 O (l)

21. Write Rate Expressions for: Cl 2(g) + HOOH (aq) P (aq)

22. Reaction Order The total number of reactants Equals total of all of the coeffecients of R in the rxn Equals total exponents in rate expression

23. Determining Rxn Rate Find rate expression ratios (Ratio of concentrations) x = rate ratio x = exponent

24. Experimental Results Exp [A] [B] [C] Rate 1 1.0 1.0 1.0 2 2 2.0 1.0 1.0 4 3 1.0 2.0 1.0 8 4 1.0 1.0 2.0 4

25. Experimental Results Exp # [A] [B] [C] Rate 1 0.1 0.1 0.1 3 2 0.3 0.1 0.1 9 3 0.1 0.3 0.1 27 4 0.1 0.1 0.3 3

26. Half-Life The time required for one half of a reactant to be decomposed in a reaction

28. Useful Relationships Rxn OrderRate Exp 0 R=k 1 R=k[A] 2 R=k[A] 2

29. Useful Relationships Rxn OrderHalf Life 0 [A o ]/2k 1 0.693/k 2 1/k[A]

30. Useful Relationships Rxn OrderLin Plot 0[A] vs k 1 ln[A] vs k 2 1/[A] vs k

31. Useful Relationships Rxn OrderCalc R E 0 -d[A]/dt = k 1 -d[A]/dt = k[A] 2 -d[A]/dt = k[A] 2

32. Experimental Results Exp # [R] [S] [T] Rate 1) 0.25 0.20 0.10 2 2) 0.25 0.60 0.10 18 3) 0.50 0.20 0.10 4 4) 0.25 0.20 0.40 32

34. Clausius-Claperon Eq E a = R ln (T 2 )(T 1 ) k 2 (T 2 – T 1 ) k 1

36. Calculate the activation energy of a reaction whose rate constant is 2.0 x 10 3 at 27 o C and is 2.0 x 10 6 at 77 o C:

37. Experimental Results Exp # T [A] [B] Rate 1) 27 o C 0.10 0.10 2 2) 27 o C 0.30 0.10 18 3) 27 o C 0.10 0.20 4 4) 77 o C 0.10 0.10 20

38. Reaction Mechanism The sequence of steps that make up the reaction process

40. Reaction Mechanism Step 1A Bfast Step 2B ---> Cslow Step 3C Dfast Total A ---> D

41. Reaction Mechanism The rate determining step in a reaction mechanism is the slowest step

42. Reaction Mechanism To solve the rate expression, you must use the slowest step

43. Solve Rate Expression A + B C + D fast 2C + A G fast 2D + B K fast 2G + 2K Prod. slow

44. Solve Rate Expression X + Y M + N fast M + N 2G slow 2N + G K fast 2G + 2K Prod. fast

45. Solve Rate Expression X + Y M + N fast 3M + N 2G fast 2N K fast 4G + 2K Prod. slow

46. Solve Rate Expression A + B C + Dfast 4C + A 2Gfast 4D + B 2Kfast G + K Q + Wslow Q + WProd.fast

47. Review

48. Experimental Results Exp # T [A] [B] Rate 1) 27 o C 0.10 0.10 2 2) 27 o C 0.30 0.10 18 3) 27 o C 0.10 0.20 8 4) 77 o C 0.10 0.10 20

49. Solve Rate Expression A + B C + Dfast 4 C + A 2Gfast 2 K 4D + B fast G + K Q + Wfast 2Q + 2W Prod.slow