1. Chemical Kinetics
Chapter 14

4. TRANSITION STATE

5. Activated Complex

6. Kinetics vs Thermodynamics

7. Catalysts

8. Collision Theory Particles must collide before they can react
The collision must be properly oriented for the necessary arrangement of atoms and electrons
Forceful enough – possessing enough energy to form products

9. Collision Theory Particles must collide before they can react
The collision must be properly oriented for the necessary arrangement of atoms and electrons
Forceful enough – possessing enough energy to form products

10. Rates of Reactions
Reaction rates tell how fast reactants change into products
Nature of reactants
Concentration
Temperature
Surface Area
Presence of a Catalyst

11. Elementary Steps Step 1: X + Y  M (slow) Step 2: X + M  Z (fast)
What is the rate determining step?
What are the intermediates?
Is there a catalyst present?
What is the net reaction?

12. Elementary Steps Step 1: 2NO  N2O2
Step 2: N2O2 + H2  N2O + H2O (slow)
Step 3: N2O + H2  N2 + H2O
What is the rate determining step?
What are the intermediates?
Is there a catalyst present?
What is the net reaction?

13. Elementary Steps Step 1: Ce4+ + Mn2+  Ce3+ + Mn3+
Step 3: Tl+ + Mn4+  Tl3+ + Mn2+
What are the intermediates?
Is there a catalyst present?
What is the net reaction?

14. Rate Laws must be determined experimentally.
Rate = k[A]x[B]y
Rate Laws must be determined experimentally.
The ONLY time you do NOT need to use the experimental trial is for a one step reaction.

15. Reaction Order xA(aq) + yB(aq)  AB(s) Rate = k[A]x[B]y
It is order x with respect to A.
It is order y with respect to B
*The net reaction order = x + y.

16. What is the reaction order?
Rate = k[A][B]2
What is the reaction order?
Rate = k[A]3[B]2

17. Reaction Order
Determine the rate law for the following one step reactions:
2NO + O2  2NO2
2NO + Br2  2NOBr

18. Determining Rate Laws Experimentally

19. Determining Rate Laws Experientially

20. Determining Rate Laws Experimentally
Initial Rate Method: Rate1 [A]x1[B]y1 [A]1 x [B]1 y
Rate2 [A]x2[B]y2 [A]2 [B]2