2. Consider this reaction: N 2 (g) + 3H 2 (g) ----> 2 NH 3 (g) + 92 kJ  G 298K = -16.8 kJ What does this equation tell us?

3. The reaction is spontaneous at 298K It is exothermic entropy is decreasing enthalpy is decreasing the names and states of reactants and products are given for every 3 mol of H 2 (g) and 1 mol of N 2 (g) consumed 2 mol of NH 3 (g) is produced 92 kJ of energy is produced N 2 (g) + 3H 2 (g) ----> 2 NH 3 (g) + 92 kJ  G 298K = -16.8 kJ

4. N 2 (g) + 3H 2 (g) ----> 2 NH 3 (g) + 92 kJ  G 298K = -16.8 kJ What does this equation NOT tell us? How much of each substance we started with how much of each substance is consumed How fast the reaction is Whether or not the reaction proceeds directly as shown in the equation or if intermediate steps occur (reaction mechanism)

5. Consider this reaction: 4 HBr(g) + O 2 (g) --> 2 H 2 O + 2 Br 2 (g) This reaction proceeds through these steps HBr + O 2 ---> HOOBr (slow) HOOBr + HBr ---> 2 HOBr (fast) 2 HOBr + 2 HBr --> 2 H 2 O + 2 Br 2 (g) (fast) In this case the equation simply tells us the reactants and products. It doesn’t tell us the series of steps by which the reaction goes.

6. When we refer to reaction rates we are referring to how fast a reaction goes. Rates can be expressed both qualitatively and quantitatively. In a qualitative way one would describe a reaction as fast or slow. H 2 (g) + O 2 (g) ----> H 2 O (g) fast Fe + 1/2O 2 + H 2 O ---> Fe(OH) 2 slow Quantitatively rates are expressed by observing the rate at which a reactant disappears or a product appears.

7. It may be expressed as the change in mol/unit time or the change in concentration/unit time Mg(s) + 2 HCl(aq) ---> MgCl 2 (aq) + H 2 (g) Rate = # mol of Mg consumed Time required to disappear = 2.4 g/24 g/mol 45 s = 2.2 x 10 -3 mol/s

8. See Saunders - Chapter 15- Lesson 2 For Measuring Rates then conduct an exercise using burettes

10. Chemical reactions only occur when reacting particles collide with sufficient energy, and at a favourable geometry. H2H2 Cl 2 H2H2 H2H2

11. Fast enough, but the wrong geometry

18. Right Geometry, too slow

39. Right Geometry, sufficient speed Activation energy reached

40. Right Geometry, sufficient speed Activation energy reached

41. Right Geometry, sufficient speed Activation energy reached

42. Right Geometry, sufficient speed Activation energy reached

43. Right Geometry, sufficient speed Activation energy reached

44. Right Geometry, sufficient speed Activation energy reached

45. Potential Energy Reaction Coordinate 1 - The reacting molecules are sufficiently far apart so they have no influence on one another 2 - As the reacting molecules approach their electrons start to repel so the H-H and Cl-Cl bonds stretch, Ek decreases and Ep increases. 3 - At the same time new bonds are starting to form between H and Cl as H nuclei attract Cl electrons and Cl nuclei attract H electrons 4 -If the molecules have sufficient energy to react a short lived activated complex is formed. At this point no bond breaking or bond making is occuring. 5 -If the reaction proceeds the bonds between H-Cl continue to shrink until they reach a stable state

46. Potential Energy (kJ) Reaction Coordinate 1. 2. 3. 2.0 4.0 7.6  H = 2.0 kJ - 4.0 kJ = - 2.0 kJ Eaf= 7.6 kJ - 4.0 kJ = 3.6 kJ Ear= 7.6 kJ - 2.0 kJ = 5.6 kJ Eaf = energy of activation, forward

47. Construct a potential energy vs. reaction coordinate curve for an endothermic reaction

48. Potential Energy (kJ) Reaction Coordinate 1. 2. 3. 1.0 3.0 5.6  H = 3.0 kJ - 1.0 kJ = 2.0 kJ Eaf= 5.6 kJ - 1.0 kJ = 4.6 kJ Ear= 5.6 kJ - 3.0 kJ = 2.6 kJ Eaf = energy of activation, forward