1. EQUILIBRIUM 2 REACTION YIELDS

2. Equilibrium Very few reactions proceed unhindered to completion. Some begin reversing as soon as products are present. Examples of reversible reactions –Melting ice block H 2 O (s) H 2 O (l) –Ni-Cad rechargeable batteries

3. Equilibrium Chemical reactions that consist of two opposing processes (forward and reverse reactions) will eventually reach an equilibrium. The state of equilibrium is characterized by the forward and reverse reactions proceeding at the same rate i.e. reactions do not stop ‑ we have a dynamic situation

4. Dynamic Equilibrium Characterized by the following criteria 1.amounts and concentrations of substances remain constant 2.total gas pressure remains constant 3.temperature remains constant 4.the reaction is incomplete (all substances involved in the reaction are present)

5. Equilibrium rate time Equilibrium first established N 2 + 3H 2  2NH 3 2NH 3  N 2 + 3H 2 Variation of the rates of the forward and reverse reactions with time

6. The Equilibrium Law For the general equilibrium xA + yB  pC + qD It can be stated = constant = K [C] p [D] q [A] x [B] y

7. Equilibrium Law K allows for the evaluation of the concentration fraction at any time. When the system is at equilibrium the concentration fraction is constant ‑ so called the equilibrium constant (K). For a particular reaction, K is constant for all equilibrium mixtures (provided temperature remains constant)

8. Information From The Equilibrium Constant If K is about 10 4 to 10 –4 there will be significant amounts of both reactants and products present at equilibrium If K is very large (> 10 4 ) the equilibrium mixture consists mostly of products If K is very small (< 10 –4 ) the equilibrium mixture consists mostly of reactants

9. Le Chatelier's Principle Whenever a change is made to a system at equilibrium, the equilibrium position will shift to partially oppose the change

10. Disturbing Equilibrium There are 4 major means of disturbing a system at equilibrium 1.Adding or removing a reactant or product 2.Changing the pressure by changing the volume (gases only) 3.Dilution (for solutions only) 4.Changing the temperature

11. Disturbing Equilibrium Addition of a catalyst will increase both the rate of the forward and reverse reactions equally It will simply reduced the time taken to reach equilibrium.

12. Effect of Temperature on Equilibria As temperature INCREASES –For exothermic reactions, value of K decreases and amounts of products decrease –For endothermic reactions, value of K increases and amounts of products increase

13. Effect of Temperature on Equilibria The value of K depends on temperature When stating a value of K, the temperature at which the constant was calculated must also be stated Temperature is the only change that can be made to a system at equilibrium that will actually change the equilibrium constant (ie K is temperature dependant)

14. Consider the Reaction N 2 (g) + 3H 2 (g) 2NH 3 (g)

15. Effect on Equilibrium of Adding / Removing Reactant or Product N 2 (g) + 3H 2 (g) 2NH 3 (g)

16. Effect of Adding Nitrogen Causes the rate of the forward reaction to increase More ammonia is formed [NH 3 ] increases This causes the rate of the back reaction to increase to re form more N 2 and H 2

17. Effect of Adding Nitrogen concentration time [NH 3 ] [N 2 ] [H 2 ] Initial equilibrium

18. Effect of Adding Nitrogen time Initial equilibrium Nitrogen added [NH 3 ] [N 2 ] [H 2 ] concentration

19. Effect of Adding Nitrogen time Initial equilibrium Nitrogen added System returns to equilibrium [NH 3 ] [N 2 ] [H 2 ] concentration

20. Effect of Adding Nitrogen time Initial equilibrium Nitrogen added System returns to equilibrium New equilibrium established [NH 3 ] [N 2 ] [H 2 ] concentration

21. Effect of Adding Hydrogen time Initial equilibrium Hydrogen added [NH 3 ] [N 2 ] [H 2 ] concentration

22. Effect of Adding Hydrogen time Initial equilibrium Hydrogen added [NH 3 ] [N 2 ] [H 2 ] concentration

23. Effect of Adding Hydrogen time Initial equilibrium Hydrogen added System returns to equilibrium [NH 3 ] [N 2 ] [H 2 ] concentration

24. Effect of Adding Hydrogen time Initial equilibrium Hydrogen added System returns to equilibrium New equilibrium established [NH 3 ] [N 2 ] [H 2 ] concentration

25. Effect of Adding Product Leads to Formation of more Reactants A nett back reaction occurs

26. Effect of Adding Ammonia time Initial equilibrium [NH 3 ] [N 2 ] [H 2 ] concentration

27. Effect of Adding Ammonia concentratio n time Initial equilibrium Ammonia added [NH 3 ] [N 2 ] [H 2 ]

28. Effect of Adding Ammonia concentratio n time Initial equilibrium Ammonia added System returns to equilibrium [NH 3 ] [N 2 ] [H 2 ]

29. Effect of Adding Ammonia concentratio n time Initial equilibrium Ammonia added System returns to equilibrium New equilibrium established [NH 3 ] [N 2 ] [H 2 ]

30. Effect of Changing Reactant / Product Addition of Reactant leads to more Products being formed (Nett Forward Reaction) Addition of Product leads to more Reactants being formed (Nett Back Reaction) Removal of Reactant leads to less Products being formed (Nett Back Reaction) Removal of Product leads to less Reactants being formed (Nett Forward Reaction)

31. Changing Pressure Pressure can be changed by increasing or decreasing the volume of the container while keeping the temperature constant. Need to examine 2 examples

32. Changing Pressure 2SO 2(g) + O 2(g) 2SO 3(g) – 3 gas particles 2 gas particles A nett forward reaction –involves a reduction in the number of gas particles, –so a reduction in pressure A nett back reaction –Involves an increase in the number of gas particles –So an increase in pressure

33. Changing Pressure 2SO 2(g) + O 2(g) 2SO 3(g) – 3 gas particles 2 gas particles Using Le Chatelier’s Principle An increase in pressure will lead to –Be adjusted by a reduction in pressure –A nett forward reaction will occur increasing the amount of sulphur trioxide present at equilibrium

34. Changing Pressure 2SO 2(g) + O 2(g) 2SO 3(g) SO 2 5 O 2 3 SO 3 1 TOTAL 9

35. Changing Pressure 2SO 2(g) + O 2(g) 2SO 3(g) SO 2 1 O 2 1 SO 3 5 TOTAL 7 Increased pressure Nett forward reaction

36. Changing Pressure N 2 O 4(g) 2NO 2(g) –1 gas particles 2 gas particles –Colourless Brown A nett forward reaction –involves an increase in the number of gas particles, –so an increase in pressure A nett back reaction –Involves a decrease in the number of gas particles –So a decrease in pressure

37. Changing Pressure N 2 O 4(g) 2NO 2(g) An equilibrium mixture of the gases was compressed Initially darkened - [NO 2 ] increases Then colour of gas mixture fades –Nett backward reaction

38. Changing Pressure N 2 O 4(g) 2NO 2(g) concentration Initial equilibrium [N 2 O 4 ] [NO 2 ] time

39. Changing Pressure N 2 O 4(g) 2NO 2(g) concentration Increase of pressure Initial equilibrium time [N 2 O 4 ] [NO 2 ]

40. Changing Pressure N 2 O 4(g) 2NO 2(g) concentration Increase of pressure Initial equilibrium System returns to equilibrium time [N 2 O 4 ] [NO 2 ]

41. Changing Pressure N 2 O 4(g) 2NO 2(g) concentration time Increase of pressure Initial equilibrium System returns to equilibrium New equilibrium established [N 2 O 4 ] [NO 2 ]

42. Adding an inert gas Total pressure of equilibrium system can be changed without changing the volume of the container by adding an inert gas There is no increase in concentrations of reactants or products No change in equilibrium

43. Dilution When dilution occurs, a net reaction results which produces the greater number of particles The effect of diluting the solution by adding water is –A net reaction in the direction that produces more particles

44. Dilution Fe 3+ (aq) + SCN – (aq) Fe(SCN) 2+ (aq) –2 particles in soln 1 particle in soln Dilution of this equilibrium will result in a nett back reaction Results in an increase of [Fe 3+ ] and [SCN – ]

45. Change in Temperature Using Le Chatelier’s Principle Exothermic reaction can be written as –Reactants Products + energy –Heating increases the energy of the substances –Principle says the reaction will oppose an increase in energy by removing energy –A nett back reaction occurs –Less product and more reactants now present

46. Change in Temperature Exothermic A + B C + D concentration [A] [B] [C] [D] Initial equilibrium time

47. Change in Temperature Exothermic A + B C + D concentration [A] [B] [C] [D] Initial equilibrium Temperature increases System returns to equilibrium time

48. Change in Temperature Exothermic A + B C + D time concentration [A] [B] [C] [D] Initial equilibrium Temperature increases System returns to equilibrium New equilibrium established

49. Change in Temperature Endothermic A + B C + D concentration [A] [B] [C] [D] Initial equilibrium time

50. Change in Temperature Endothermic A + B C + D concentration [A] [B] [C] [D] Initial equilibrium Temperature increases System returns to equilibrium time

51. Change in Temperature Endothermic A + B C + D concentration [A] [B] [C] [D] Initial equilibrium Temperature increases System returns to equilibrium time New equilibrium established

52. Adding a Catalyst Catalysts increase the rate of the reaction They affect both forward and back reaction equally Do NOT change the position of the equilibrium Do NOT change the equilibrium constant