2. Video 9.1

3. Rate: A measure of the speed of any change.

4. Collision Theory: When two chemicals react, their molecules have to collide with each other with proper energy and orientation.

5. When temperature increases, the molecules move ___________ and collide ________. So the rate of reaction ____________, or the reaction moves _____________. Temperature faster more increases faster

6. When concentration increases, the molecules collide ________. So the rate of reaction ____________, or the reaction moves _____________. Concentration more increases faster

7. When the surface area increases, the molecules collide ________. So the rate of reaction ____________, or the reaction moves _____________. Surface Area more increases faster

8. When catalysts are added, the make the reaction ___________ and collide ________. So the rate of reaction ___________. Catalysts faster more increases

9. Ionic substances react faster than covalent substances because the easily break into ions when you dissolve them. Nature of Reactants

10. When the pressure on a gas increases, the gas has __________ volume. Therefore, there are _________ collisions and the rate __________, or moves _____________. Pressure less more increases faster

11. Video 9.2

12. If heat is absorbed, the reaction is endothermic and the enthalpy increases (+). If heat is released the reaction is exothermic and the enthalpy decreases (-). Enthalpy: Heat

13. Reactions with negative enthalpy values are exothermic. The heat can be added to the reaction on the products side. CH 4 + 2O 2  CO 2 + 2H 2 O + 890.4KJ Reactions with positive enthalpy values are endothermic. The heat can be added to the reaction on the reactant side. 182.6KJ + N 2 + O 2  2 NO Reference Table I

14. More stable Spontaneous The reactants in the reaction have more energy than the products. Exothermic Reactions

15. 1.Endothermic or exothermic? a.Formation of NO 2 b.Synthesis of C 2 H 6 c.Formation of CO 2 from elements d.Dissolving LiBr 2.Which is more stable? a.H 2 O (g) or H 2 O (l) b.C 2 H 2 or Al 2 O 3 Review with Table I ENDO EXO H 2 O (l) Al 2 O 3

16. Use mole ratios to calculate how much heat is evolved in a reaction: 89.3KJ + C + 2S  CS 2 1.How much heat is absorbed when 5.00 moles of C are used? 2.How much heat is needed to produce 3.00 moles of CS 2 ? Enthalpy in reactions 447KJ 268KJ 5(89.3) = 3(89.3) =

17. Video 9.3

18. Activation Energy There is a minimum amount of energy required for reaction: the activation energy, E a. Just as a ball cannot get over a hill if it does not roll up the hill with enough energy, a reaction cannot occur unless the molecules possess sufficient energy to get over the activation energy barrier.

19. A + B C + D Exothermic Reaction Endothermic Reaction The activation energy (E a ) is the minimum amount of energy required to initiate a chemical reaction. 13.4

20. The activated complex is the highest part of the graph where the reaction can go to completion or revert back to reactants. Enthalpy, or heat, can be measured on the graph by subtracting reactants from products.

21. Energy Diagrams ExothermicEndothermic

22. Catalysts Catalysts increase the rate of a reaction by decreasing the activation energy of the reaction. Catalysts change the mechanism by which the process occurs.

23. Video 9.4

24. The more disorder, the higher the entropy. The entropy of a gas is _______ than a liquid or solid. The more substances, the __________ the entropy. As temperature increases, entropy _____________. Entropy = Disorder More higher increases

25. If a reaction is exothermic and is disorderly, the reaction will be spontaneous. Think about Spontaneous combustion! Spontaneous Reactions

26. 1.Contrast enthalpy and entropy. 2.As a system becomes more random, entropy _________. 3.What phase changes increase entropy? 4.On a heating curve, which point has the most entropy? Review

27. Video 9.5

28. Equilibrium

29. N 2 O 4 NO 2 N 2 + 3H 2 2NH 3

30. A reaction at equilibrium means the forward and reverse reaction occur at the same rate. If any change happens, the equilibrium will shift in a direction that reduces that change. Le Châtelier’s Principle N 2 O 4 NO 2

31. If a substance is taken, the reaction will shift toward that substance to restore equilibrium. If a substance is added, the reaction will shift away from that substance to restore equilibrium. 2H 2 + O 2  2H 2 O The Effects of Changes in Concentration

32. Concentration

33. The Effect of Changes in Temperature Endothermic Reactants + Heat  Products ExothermicReactants  Heat + Products Heat is considered a reactant and product

34. An increase in volume decreases the pressure and causes a shift that favors more moles of gas A decrease in volume increases the pressure and causes a shift that favors less moles of gas N 2 O 4(g) 2NO 2(g) The Effects of Changes in Volume

35. Volume/Pressure 2Red  1Gray

36. Catalysts Catalysts increase the rate of both the forward and reverse reactions. Equilibrium is achieved faster, but the reactants and products do not change.

37. 1.Consider the following equation: N 2 + 3H 2  2NH 3 + 92KJ Predict how the H 2 will be affected by: a.Ammonia being added b.Nitrogen being added c.Heat being added d.Pressure decreasing e.Ammonia being removed f.Nitrogen being removed g.Decreasing the volume LeChatelier Problems increases decreases increases decreases increases decreases