1. Drill: List five factors & explain how each affect reaction rates

2. Review Drill & Check HW

3. CHM II HW Review PP-19 & 20 Complete the attached worksheet & turn it in tomorrow Lab Thursday

4. Are there any questions on previous material?

5. Chemical Equilibria

6. Equilibrium The point at which the rate of a forward reaction = the rate of its reverse reaction

7. Equilibrium The concentration of all reactants & products become constant at equilibrium

8. Equilibrium Because concentrations become constant, equilibrium is sometimes called steady state

9. Equilibrium Reactions do not stop at equilibrium, forward & reverse reaction rates become equal

11. Reaction aA (aq) + bB (aq) pP (aq) + qQ (aq) Rate f = k f [A] a [B] b Rate r = k r [P] p [Q] q At equilibrium, Rate f = Rate r k f [A] a [B] b = k r [P] p [Q] q

12. At equilibrium, Rate f = Rate r k f [A] a [B] b = k r [P] p [Q] q k f / k r = ([P] p [Q] q )/ ( [A] a [B] b ) k f / k r = K c = K eq in terms of concentration K c = ([P] p [Q] q )/ ( [A] a [B] b )

13. All Aqueous aA + bB pP + qQ

15. Equilibrium Expression ( Products) p (Reactants) r K eq =

16. Drill: Solve Rate Expr: X + Y M + N fast 3M + N 2G fast 2N K fast 2G + K Prod. slow

17. Drill: Solve Rate Expr: X + Y M + N fast 3M + N 2G fast 2N K fast 2G + K Prod. slow

18. Work from the slow step up

19. Drill: Solve Rate Expr: X + Y M + N fast 3M + N 2G fast 2N K fast 2G + K Prod. slow

20. 1) Cancel K & G

21. Drill: Solve Rate Expr: X + Y M + N fast 3M + N 2G fast 2N K fast 2G + K Prod. slow

22. 1)Cancel K & G Triple rxn 1 & cancel

23. Drill: Solve Rate Expr: 3X + 3Y 3M + 3N 3M + N 2G fast 2N K fast 2G + K Prod. slow

24. Solve Rate Law A + B C + Dfast 4 C + A 2Gfast 2 K 4D + B fast G + K 2 Q + 2 Wfast Q + W Prod.slow

25. Drill: Solve Rate Law A + B C + Dfast 4 C + A 2Gfast 2 K 4D + B fast G + K 2 Q + 2 Wfast Q + W Prod.slow

26. 1) Reverse step 3

27. Drill: Solve Rate Law A + B C + Dfast 4 C + A 2Gfast 4 D + B 2K fast G + K 2 Q + 2 Wfast Q + W Prod.slow

28. 1)Reverse Rxn 3 Divide Rxn 4 by 2 & cancel

29. Drill: Solve Rate Law A + B C + Dfast 4 C + A 2Gfast 4 D + B 2K fast G/2 + K/2 Q + Wfast Q + W Prod.slow

30. 1)Reverse Rxn 3 Divide Rxn 4 by 2 & cancel Divide Rxns 2 & 3 by 4 & cancel

31. Drill: Solve Rate Law A + B C + Dfast C + A/4 G/2fast D + B/4 K/2 fast G/2 + K/2 Q + Wfast Q + W Prod.slow

32. 1)Reverse Rxn 3 Divide Rxn 4 by 2 & cancel Divide Rxns 2 & 3 by 4 & cancel Add the rxns

33. 5/4 A + 5/4 B  Product Rate = k[A] 5/4 [B] 5/4

34. Review & Collect Drill & HW

35. CHM II HW Review PP-19 & 20 Remember M. S.

36. Are there any questions on previous material?

37. Equilibrium Applications When K >1, [P] > [R] When K <1, [P] < [R]

38. Equilibrium Calculations K p = K c (RT)  n gas

39. Equilibrium Expression Reactants or products not in the same phase are not included in the equilibrium expression

40. Equilibrium Expression aA (s) + bB (aq)  cC (aq) + dD (aq) [C] c [D] d [B] b K eq =

41. Reaction Mechanism When one of the intermediates anywhere in a reaction mechanism is altered, all intermediates are affected

42. Reaction Mechanism 1) A + B C + D 2) C + D E + K 3) E + K H + M 4) H + M P

43. Lab Results %100806040 RT5.218.4211.9 21.7 WR2.754.237.96 11.2

44. Reaction Quotient where [A], [B], [P], and [Q] are molarities at any time. Q = K only at equilibrium. aA (aq) + bB (aq)  pP (aq) + qQ (aq)

45. Drill: NH 3 H 2 + N 2 At a certain temperature at equilibrium P ammonia = 4.0 Atm, P hydrogen = 2.0 Atm, & P nitrogen = 5.0 Atm. Calculate K eq :

46. Review & Collect Drill & HW

47. CHM II HW Review PP 19 & 20 Complete the attached assignment & turn it in tomorrow

48. Are there any questions on previous material?

49. Reaction Quotient where [A], [B], [P], and [Q] are molarities at any time. Q = K only at equilibrium. aA (aq) + bB (aq)  pP (aq) + qQ (aq)

50. Equilibrium Applications When K > Q, the reaction goes forward When K < Q, the reaction goes in reverse

51. Equilibrium Calculations aA + bB  pP + qQ Stoichiometry is used to calculate the theoretical yield in a one directional rxn

52. Equilibrium Calculations aA + bB  pP + qQ In equilibrium rxns, no reactant gets used up; so, calculations are different

53. Equilibrium Calculations Set & balance rxn Assign amounts with x Write eq expression Substitute amounts Solve for x

54. Equilibrium Calculations CO + H 2 O CO 2 + H 2 Calculate the partial pressure of each portion at eq.when 100.0 kPa CO & 50.0 kPa H 2 O are combined: K p = 3.4 x 10 -2

55. Equilibrium Calculations COH 2 OCO 2 H 2 100 -x 50 - x x x P CO2 P H2 x 2 P CO P H2O (100-x) (50-x) K p = 3.4 x 10 -2 =KP=KP= Send to the next page

56. Equilibrium Calculations x 2 (100 -x)(50 - x) x 2 5000 -150x + x 2 x 2 = 170 - 5.1x + 0.034x 2 0.966x 2 + 5.1x - 170 = 0 = = 3.4 x 10 -2

57. Equilibrium Calculations 0.966x 2 + 5.1x - 170 = 0 Use the quadratic equation to solve for x x = 11 x = -16 Substitute 11 back into the originally assigned #

58. Equilibrium Calculations COH 2 OCO 2 H 2 100 -x 50 - x x x 100-11 50-11 11 11 P CO = 89 kPa P H2O = 39 kPa P CO2 = 11 kPa P H2 = 11 kPa

59. Equilibrium Calculations Xe (g) + F 2(g) XeF 2(g) Calculate the partial pressure of each portion when 50.0 kPa Xe & 100.0 kPa F 2 are combined: K p = 4.0 x 10 -1

60. Equilibrium Calculations XeF 2 XeF 2 50 -x 100 - x x P XeF2 x P Xe P F2 (50-x) (100-x) K p = 4.0 x 10 -1 =KP=KP= Send to the next page

61. Equilibrium Calculations x (50 -x)(100 - x) x 5000 -150x + x 2 x = 2000 - 60x + 0.40x 2 0.40x 2 -61x + 2000 = 0 = = 4.0 x 10 -1

62. Equilibrium Calculations 0.40x 2 - 61x + 2000 = 0 Use the quadratic equation to solve for x x = 48 x = 105 Substitute 48 back into the original assignmented #

63. Equilibrium Calculations XeF 2 XeF 2 50 -x 100 - x x 50-48 100-48 48 P Xe = 2 kPa P F2 = 52 kPa P XeF2 = 48 kPa

64. SO 2 + O 2 SO 3 Determine the magnitude of the equilibrium constant if the partial pressure of each gas is 0.667 Atm.

65. Drill: Write the equilibrium expression & solve its magnitude when P NO2 & P N2O4 = 50 kPa each at eq: N 2 O 4(g) NO 2(g)

66. Review Drill & Check HW

67. CHM II HW Review PP-20 Complete the attached HW

68. CHM II Schedule: Lab: Later this week Test Early next week

69. Are there any questions on previous material?

70. Equilibrium Calculations Xe (g) + 2 F 2(g) XeF 4(g) Calculate the partial pressure of each portion when 75 kPa Xe & 20.0 kPa F 2 are combined: K p = 4.0 x 10 -8

71. Le Chatelier’s Principle If stress is applied to a system at equilibrium, the system will readjust to eliminate the stress

72. LC Eq Effects A (aq) +2 B (aq) C (aq) + D (aq) + heat Write equilibrium exp: What happens if:

73. LC Eq Effects 2 A (aq) + B (s) C (aq) +2 D (aq) + heat Write equilibrium exp: What happens if:

74. LC Eq Effects 2 A (g) + 2 B (g) 3 C (g) + 2 D (l) What happens if:

75. Equilibrium Applications  G =  H - T  S  G = - RTlnK eq

76. Drill: Solve for K A (aq) + 2 B (aq) C (s) + 2 D (aq) Calculate K eq if: [A] = 0.30 M [B] = 0.20 M C = 5.0 g [D] = 0.30 M

77. Review & Collect Drill & HW

78. Schedule Lab: Friday Test: Next week

79. CHM II HW Review PP-20 Complete the attached assignment & turn it in tomorrow.

80. Are there any questions on previous material?

81. A (aq) + B (aq) AB (aq) Calculate the equilibrium concentration of each species when equal volumes of 0.40 M A & 0.20 M B are combined. K eq = 0.50

82. Equilibrium Calculations Xe (g) + F 2(g) XeF 2(g) Calculate the partial pressure of each portion when 80.0 kPa Xe & 60.0 kPa F 2 are combined: K p = 4.0 x 10 -2

83. Drill: A + B C + D Calculate the equilibrium concentration of each species when equal volumes of 0.60 M A & 0.80 M B are combined. K eq = 5.0 x 10 -6

84. Review & Collect Drill & HW

85. CHM II HW Review PPs 19 & 20 Review both for the Test on Monday.

86. The Test on Rxn Rates & Chemical Equilibria will be on Monday

87. Are there any questions on previous material?

88. Working with Equilibrium Constants

89. When adding Reactions: Multiply Ks

90. ABK 1 B CK 2 ACK 3 K 3 = (K 1 )(K 2 )

91. Solve K for each: A + B C + D C + D P + Q A + B P + Q K1K1 K2K2 K3K3

92. When doubling Reactions: Square Ks

93. ABK 1 2 A2 B K 2 K 2 = (K 1 ) 2

94. When a rxn is multiplied by any factor, that factor becomes the exponent of K

95. ABK 1 1/3 A1/3 B K 2 K 2 = (K 1 ) 1/3

96. When reversing Reactions Take 1/Ks

97. ABK 1 B AK 2 K 2 = 1/K 1

98. Equilibrium Calculations CuCl 6 -4 (aq) + 2 NH 3(aq) [Cu(NH 3 ) 2 Cl 4 ] -2 (aq) Calculate the molarity of each portion when 0.10 M CuCl 6 -4 & 1.0 M NH 3 are combined: K formation = 0.060

99. Equilibrium Calculations Rn (g) + F 2(g) RnF 2(g) Calculate the partial pressure of each portion when 25 kPa Rn & 75 kPa F 2 are combined: K p = 4.0 x 10 -2

100. Drill: A + B P + Q Calculate the concentration of each portion at equilibrium when 100.0 mL 0.50 M A is added to 150 mL 0.50 M B: K c = 6.0 x 10 -8

101. Review Drill & Check HW

102. Next Test Monday

103. Review for the Test

104. Rate Law aA + bB pP + qQ k[A] a [B] b Rate =

105. Equilibrium Equation aA + bB pP + qQ [P] p [Q] q [A] a [B] b K c = at equilibrium

106. Reaction Quotient aA + bB pP + qQ [P] p [Q] q [A] a [B] b Q = at the other conditions

107. The data on the next slide was obtained in lab. Use that data to solve for the order with respect to each reactant, the reaction order, the rate expression, k, & E a.

108. Experimental Results Exp # [A] [B] Rate 1 27 1.0 1.0 2.0 x 10 -2 2 27 2.0 1.0 4.0 x 10 -2 3 27 1.0 2.0 8.0 x 10 -2 4 77 1.0 1.0 2.0

109. Reaction Mechanism Step 1A Bfast Step 22 B 3Cfast Step 3C 2Dfast Step 4D  P slow

110. LC Eq Effects 2 A (aq) + B (s) C (aq) +2 D (aq) + heat Write equilibrium exp: What happens if:

111. LC Eq Effects 3 A (g) + B (g) 2 C (g) + 2 D (l) Write equilibrium exp: What happens if:

112. SO + O 2 SO 3 Calculate the equilibrium pressures if SO at 80.0 kPa is combined with O 2 at 40.0 kPa. K = 2.00

113. Equilibrium Calculations I 2 + 2 S 2 O 3 -2 S 4 O 6 -2 + 2 I - Calculate the equilibrium concentration of each portion when it’s 0.25 M I 2 & 0.50 M S 2 O 3 -2 at the start of the rxn. K c = 4.0 x 10 -8

114. Clausius-Claperon Eq E a = R ln (T 2 )(T 1 ) k 2 (T 2 – T 1 ) k 1

115. Clausius-Claperon Eq H v = R ln (T 2 )(T 1 ) P 2 (T 2 – T 1 ) P 1

116. Clausius-Claperon Eq  H = R ln (T 2 )(T 1 ) K 2 (T 2 – T 1 ) K 1

117.  G  -  S  G o = -RTlnK

118. Experimental Results Exp # [A] [B] [C] time 1 1.0 1.0 1.0 16 2 2.0 1.0 1.0 2 3 1.0 2.0 1.0 8 4 1.0 1.0 2.0 4

119. Drill: 1 A + 1 B 1 Z + 1 Y Calculate the concentration of each portion at equilibrium when 1.0 L 0.50 M A is added to 1.5 L 0.50 M B: K c = 2.0 x 10 -2

120. Drill: Calculate the heat of reaction when K = 2.5 x 10 -6 at 27 o C, & K = 2.5 x 10 -4 at 127 o C.

121. Write the Eq Expression AB (aq) A (aq) + B (aq) Calculate [A], [B], & [AB] at equilibrium when [AB] = 0.60 M at the start K eq = 6.0 x 10 -5

122. Write the Eq Expression PQ (aq) P (aq) + Q (aq) Calculate [P], [Q], & [PQ] at equilibrium when [PQ] = 0.90 M at the start K eq = 9.0 x 10 -5

123. Write the Eq Expression AB (aq) A (aq) + B (aq) Calculate [A], [B], & [AB] at equilibrium when [AB] = 0.60 M at the start K eq = 6.0 x 10 -5

124. Experimental Results Exp # [A] [B] [C] Rate 1 0.1 0.1 0.2 2 2 0.1 0.3 0.2 18 3 0.1 0.1 0.8 8 4 0.2 0.1 0.2 64

125. A + B C + D C + H M + N N + T P + Q What happens all intermediates if:

126. 1A + 1B1P + 1Q [A i ] = 0.20 MCalcu- [B i ] = 0.30 Mlate the [P i ] = 0.20 Meq con- [Q i ] = 0.30 Mcentra- K c = 0.020tion of ea.