1. Basic Principles of Chemistry Online Southeast Missouri State University Cape Girardeau, MO Introductory Chemistry, 3 rd Edition Nivaldo Tro Chapter 15 Chemical Equilibrium 2009, Prentice Hall

2. Tro's Introductory Chemistry, Chapter 15 2 Equilibrium vs. Disequilibrium When systems are at equilibrium with their surroundings, their conditions are the same as the surroundings and they stay that way. When systems are in disequilibrium with their surroundings, their conditions are not the same as the surroundings. Systems that are in disequilibrium tend to change until they reach equilibrium with their surroundings. Living things are in controlled disequilibrium with their environment—they are not at the same conditions as the environment and do not tend to change toward those conditions.

3. Tro's Introductory Chemistry, Chapter 15 3 Reaction Rates Some chemical reactions proceed rapidly. Like the precipitation reactions studied in Chapter 7 where the products form practically the instant the two solutions are mixed. Other reactions proceed slowly. Like the decomposition of dye molecules of a sofa placed in front of a window. The rate of a reaction is measured in the amount of reactant that changes into product in a given period of time. Generally moles of reactant used per second.  Like miles per hour. Chemists study ways of controlling reaction rates.

4. Tro's Introductory Chemistry, Chapter 15 4 Reaction Rates, Continued Initially, only reactants are presentAfter 15 seconds, the left reaction is 60% complete, but the right reaction is only 20% complete After 30 seconds, the left reaction is complete, whereas the right reaction is only 40% done. After 45 seconds, the right reaction is still not complete

5. Tro's Introductory Chemistry, Chapter 15 5 2 N 2 O 5 (g) → 4 NO 2 (g) + O 2 (g) Over time, the concentrations of reactants decrease as products increase.

6. Tro's Introductory Chemistry, Chapter 15 6 2 N 2 O 5 (g) → 4 NO 2 (g) + O 2 (g): Rate vs. Time Because reactant concentrations decrease, the rates of reactions slow down over time.

7. Tro's Introductory Chemistry, Chapter 15 7 Collision Theory In order for a reaction to take place, the reacting molecules must collide with each other. Once molecules collide they may react together or they may not, depending on two factors: 1.Whether the collision has enough energy to “start to break the bonds holding reactant molecules together." 2.Whether the reacting molecules collide in the proper orientation for new bonds to form.

8. Tro's Introductory Chemistry, Chapter 15 8 Effective Collisions Collisions in which these two conditions are met (and therefore the reaction occurs) are called effective collisions. The higher the frequency of effective collisions, the faster the reaction rate. There is a minimum energy needed for a collision to be effective. We call this the activation energy. The lower the activation energy, the faster the reaction will be.

9. Tro's Introductory Chemistry, Chapter 15 9 Effective Collisions: Kinetic Energy Factor For a collision to lead to overcoming the energy barrier, the reacting molecules must have sufficient kinetic energy so that when they collide, it can form the activated complex.

10. Tro's Introductory Chemistry, Chapter 15 10 Effective Collisions: Orientation Effect

11. Tro's Introductory Chemistry, Chapter 15 11 Reaction Energy Diagram

12. Tro's Introductory Chemistry, Chapter 15 12 The higher the concentration of reactant molecules, the faster the reaction will generally go. Increases the frequency of reactant molecule collisions. Since reactants are consumed as the reaction proceeds, the speed of a reaction generally slows over time. Factors Effecting Reaction Rate: Reactant Concentration

13. Tro's Introductory Chemistry, Chapter 15 13 Effect of Concentration on Rate Low concentrations of reactant molecules leads to fewer effective collisions, therefore a slower reaction rate. High concentrations of reactant molecules lead to more effective collisions, therefore a faster reaction rate.

14. Tro's Introductory Chemistry, Chapter 15 14 Increasing the temperature increases the number of molecules in the sample with enough energy so that their collisions can overcome the activation energy. Increasing the temperature also increases the frequency of collisions. So the rate increases because the frequency of effective collisions increases. Both these mean that increasing temperature increases the reaction rate. Factors Effecting Reaction Rate: Temperature

15. Effect of Temperature on Rate Low temperatures lead to fewer molecules with enough energy to overcome the activation energy, and less frequent reactant collisions, therefore a slower reaction rate High temperatures lead to more molecules with enough energy to overcome the activation energy, and more frequent reactant collisions, therefore, a faster reaction rate.

16. Tro's Introductory Chemistry, Chapter 15 16 Reaction Dynamics If the products of a reaction are removed from the system as they are made, then a chemical reaction will proceed until the limiting reactants are used up. However, if the products are allowed to accumulate; they will start reacting together to form the original reactants. This is called the reverse reaction. Reactions that can proceed in both the forward and reverse directions are called reversible reactions.

17. Tro's Introductory Chemistry, Chapter 15 17 Reaction Dynamics, Continued The forward reaction slows down as the amounts of reactants decreases. At the same time, the reverse reaction speeds up as the concentration of the products increases. Eventually, the forward reaction is using reactants and making products as fast as the reverse reaction is using products and making reactants. This is called chemical equilibrium. Dynamic equilibrium is reached when the rates of two opposite processes are the same.

18. Tro's Introductory Chemistry, Chapter 15 18 Chemical Equilibrium When a reaction reaches equilibrium, the amounts of reactants and products in the system stay constant. The forward and reverse reactions still continue. Because they go at the same rate, the amounts of materials do not change.

19. Equilibrium Initially, we only have reactant molecules in the mixture. The reaction can only proceed in the forward direction, making products. As the reaction proceeds, the forward reaction slows down as the reactants get used up. At the same time, the reverse reaction speeds up as product concentration increases. Eventually, the forward and reverse rates are equal. At this time equilibrium is established. Once equilibrium is established, the concentrations of the reactants and products in the final mixture do not change, (unless conditions are changed).

20. Tro's Introductory Chemistry, Chapter 15 20 Equilibrium, Continued Time Rate Rate forward Rate reverse Initially, only the forward reaction takes place. As the forward reaction proceeds it makes products and uses reactants. Because the reactant concentration decreases, the forward reaction slows. As the products accumulate, the reverse reaction speeds up. Eventually, the reaction proceeds in the reverse direction as fast as it proceeds in the forward direction. At this time equilibrium is established. Once equilibrium is established, the forward and reverse reactions proceed at the same rate, so the concentrations of all materials stay constant.

21. 21 Hypothetical Reaction 2 Red  Blue Time[Red][Blue] 00.4000.000 100.2080.096 200.1900.105 300.1800.110 400.1740.113 500.1700.115 600.1680.116 700.1670.117 800.1660.117 900.1650.118 1000.1650.118 1100.1640.118 1200.1640.118 1300.1640.118 1400.1640.118 1500.1640.118 The reaction slows over time, but the red molecules never run out! At some time between 100 and 110 sec, the concentrations of both the red and the blue molecules no longer change— equilibrium has been established. Notice that equilibrium does not mean that the concentrations are equal! Once equilibrium is established, the rate of red molecules turning into blue is the same as the rate of blue molecules turning into red.

22. Tro, Chemistry: A Molecular Approach 22 Hypothetical Reaction 2 Red  Blue, Continued

23. Tro's Introductory Chemistry, Chapter 15 23 Equilibrium  Equal The rates of the forward and reverse reactions are equal at equilibrium. But that does not mean the concentrations of reactants and products are equal. Some reactions reach equilibrium only after almost all the reactant molecules are consumed— we say the position of equilibrium favors the products. Other reactions reach equilibrium when only a small percentage of the reactant molecules are consumed—we say the position of equilibrium favors the reactants.

24. Tro's Introductory Chemistry, Chapter 15 24 An Analogy: Population Changes When Narnians feel overcrowded, some will emigrate to Middle Earth. However, as time passes, emigration will occur in both directions at the same rate, leading to populations in Narnia and Middle Earth that are constant, though not necessarily equal.

25. Tro's Introductory Chemistry, Chapter 15 25 Disturbing and Re-Establishing Equilibrium Once a reaction is at equilibrium, the concentrations of all the reactants and products remain the same. However, if the conditions are changed, the concentrations of all the chemicals will change until equilibrium is re-established. The new concentrations will be different, but the equilibrium constant will be the same. Unless you change the temperature.

26. Tro's Introductory Chemistry, Chapter 15 26 Le Châtelier’s Principle Le Châtelier’s principle guides us in predicting the effect on the position of equilibrium when conditions change. “When a chemical system at equilibrium is disturbed, the system shifts in a direction that will minimize the disturbance.”

27. 27 An Analogy: Population Changes When an influx of population enters Middle Earth from somewhere outside Narnia, it disturbs the equilibrium established between Narnia and Middle Earth. When the populations of Narnia and Middle Earth are in equilibrium, the emigration rates between the two states are equal so the populations stay constant. The result will be people moving from Middle Earth into Narnia faster than people moving from Narnia into Middle Earth. This will continue until a new equilibrium between the populations is established, However, the new populations will have different numbers of people than the old ones.

28. Tro's Introductory Chemistry, Chapter 15 28 The Effect of Concentration Changes on Equilibrium Adding a reactant will decrease the amounts of the other reactants and increase the amount of the products until a new position of equilibrium is found. That has the same K eq. Removing a product will increase the amounts of the other products and decrease the amounts of the reactants. You can use to this to drive a reaction to completion! Remember: Adding more of a solid or liquid does not change its concentration and, therefore, has no effect on the equilibrium.

29. Tro's Introductory Chemistry, Chapter 15 29 The Effect of Concentration Changes on Equilibrium, Continued When NO 2 is added, some of it combines to make more N 2 O 4.

30. Tro's Introductory Chemistry, Chapter 15 30 The Effect of Concentration Changes on Equilibrium, Continued When N 2 O 4 is added, some of it decomposes to make more NO 2.

31. Tro's Introductory Chemistry, Chapter 15 31 Practice—Predict the Effect on the Equilibrium When the Underlined Substance Is Added to the Following Systems: 2 CO 2 (g)  2 CO(g) + O 2 (g) BaSO 4 (s)  Ba 2+ (aq) + SO 4 2- (aq) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(l)

32. 32 Practice—Predict the Effect on the Equilibrium When the Underlined Substance Is Added to the Following Systems, Continued: 2 CO 2 (g)  2 CO(g) + O 2 (g) BaSO 4 (s)  Ba 2+ (aq) + SO 4 2- (aq) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(l) Shift right, removing some of the added CO 2 and increasing the concentrations of CO and O 2. Shift left, removing some of the added Ba 2+ and reducing the concentration of SO 4 2-. Shift right, removing some of the added CO 2 and decreasing the O 2, while increasing the concentration of CO 2.

33. Tro's Introductory Chemistry, Chapter 15 33 Effect of Volume Change on Equilibrium For solids, liquids, or solutions, changing the size of the container has no effect on the concentration. Changing the volume of a container changes the concentration of a gas. Same number of moles, but different number of liters, resulting in a different molarity.

34. Tro's Introductory Chemistry, Chapter 15 34 Effect of Volume Change on Equilibrium, Continued Decreasing the size of the container increases the concentration of all the gases in the container. This increases their partial pressures. If their partial pressures increase, then the total pressure in the container will increase. According to Le Châtelier’s principle, the equilibrium should shift to remove that pressure. The way to reduce the pressure is to reduce the number of molecules in the container. When the volume decreases, the equilibrium shifts to the side with fewer molecules.

35. Tro's Introductory Chemistry, Chapter 15 35 Since there are more gas molecules on the reactants side of the reaction, when the pressure is increased the position of equilibrium shifts toward the products. When the pressure is decreased by increasing the volume, the position of equilibrium shifts toward the side with the greater number of molecules—the reactant side. The Effect of Volume Change on Equilibrium, Continued

36. Tro's Introductory Chemistry, Chapter 15 36 Practice—Predict the Effect on the Equilibrium When the Volume Is Reduced. 2 CO 2 (g)  2 CO(g) + O 2 (g) BaSO 4 (s)  Ba 2+ (aq) + SO 4 2- (aq) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(l)

37. 37 Practice—Predict the Effect on the Equilibrium When the Volume Is Reduced, Continued. 2 CO 2 (g)  2 CO(g) + O 2 (g) BaSO 4 (s)  Ba 2+ (aq) + SO 4 2- (aq) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(l) Shift left because there are fewer gas molecules on the reactant side than on the product side. No effect because none of the substances are gases. Shift right because there are fewer gas molecules on the product side than on the reactant side.

38. Tro's Introductory Chemistry, Chapter 15 38 The Effect of Temperature Changes on Equilibrium Exothermic reactions release energy and endothermic reactions absorb energy. If we write heat as a product in an exothermic reaction or as a reactant in an endothermic reaction, it will help us use Le Châtelier’s principle to predict the effect of temperature changes. However, heat is not matter and not written in a proper equation.

39. Tro's Introductory Chemistry, Chapter 15 39 The Effect of Temperature Changes on Equilibrium for Exothermic Reactions For an exothermic reaction, heat is a product. Increasing the temperature is like adding heat. According to Le Châtelier’s principle, the equilibrium will shift away from the added heat. The concentrations of C and D will decrease and the concentrations of A and B will increase. The value of K eq will decrease. How will decreasing the temperature effect the system? aA + bB  cC + dD + heat

40. Tro's Introductory Chemistry, Chapter 15 40 The Effect of Temperature Changes on Equilibrium for Endothermic Reactions For an endothermic reaction, heat is a reactant. Increasing the temperature is like adding heat. According to Le Châtelier’s principle, the equilibrium will shift away from the added heat. The concentrations of C and D will increase and the concentrations of A and B will decrease. The value of K eq will increase. How will decreasing the temperature effect the system? Heat + aA + bB  cC + dD

41. Tro's Introductory Chemistry, Chapter 15 41 The Effect of Temperature Changes on Equilibrium

42. Tro's Introductory Chemistry, Chapter 15 42 Practice—Predict the Effect on the Equilibrium When the Temperature Is Reduced. Heat + 2 CO 2 (g)  2 CO(g) + O 2 (g) BaSO 4 (s)  Ba 2+ (aq) + SO 4 2- (aq)(endothermic) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(l)(exothermic)

43. 43 Practice—Predict the Effect on the Equilibrium When the Temperature Is Reduced, Continued. Heat + 2 CO 2 (g)  2 CO(g) + O 2 (g) Heat + BaSO 4 (s)  Ba 2+ (aq) + SO 4 2- (aq) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(l) + Heat Shift left, reducing the value of K eq. Shift right, increasing the value of K eq.