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Drill:

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prescott-houston
121 diapositives · 1.4K Views · Nov 08, 2014

This educational resource guides students through the essential concepts of chemical equilibrium, including five key factors that influence reaction rates. Students will learn how to establish and interpret equilibrium expressions and determine the equilibrium constant (K). The material includes practical drills on rate laws, calculations involving equilibrium conditions, and the impact of concentration changes on reaction shifts. The content is essential for mastering equilibria in chemical reactions, fostering a deeper understanding of the subjects discussed in chapters PP-19 and PP-20.

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  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. Chemical Equilibria

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

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

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

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

  9. Reaction • aA(aq)+ bB(aq) pP(aq)+ qQ(aq) • Ratef = kf[A]a[B]b • Rater = kr[P]p[Q]q • At equilibrium, Ratef = Rater • kf[A]a[B]b = kr[P]p[Q]q

  10. At equilibrium, Ratef = Rater kf[A]a[B]b = kr[P]p[Q]q kf /kr = ([P]p[Q]q)/ ( [A]a[B]b) kf /kr = Kc = Keq in terms of concentration Kc = ([P]p[Q]q)/ ( [A]a[B]b)

  11. All Aqueous aA + bB pP+ qQ

  12. Equilibrium Expression ( Products)p (Reactants)r Keq=

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

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

  15. Work from the slow step up

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

  17. 1) Cancel K & G

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

  19. Cancel K & GTriple rxn 1 & cancel

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

  21. Solve Rate Law A + B C + D fast 4 C + A 2G fast 2 K 4D + B fast G + K 2 Q + 2 W fast Q + W Prod. slow

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

  23. 1) Reverse step 3

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

  25. Reverse Rxn 3Divide Rxn 4 by 2 & cancel

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

  27. Reverse Rxn 3Divide Rxn 4 by 2 & cancelDivide Rxns 2 & 3 by 4 & cancel

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

  29. Reverse Rxn 3Divide Rxn 4 by 2 & cancelDivide Rxns 2 & 3 by 4 & cancelAdd the rxns

  30. 5/4 A + 5/4 B  ProductRate = k[A]5/4[B]5/4

  31. Review & Collect Drill & HW

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

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

  34. Equilibrium Calculations • Kp = Kc(RT)Dngas

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

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

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

  38. Reaction Mechanism • 1) A + B <---> C + D • 2) C + D <---> E + K • 3) E + K <---> H + M • 4) H + M <----> P

  39. Lab Results • % 100 80 60 40 • RT 5.21 8.42 11.9 21.7 • WR 2.75 4.23 7.96 11.2

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

  41. Drill: NH3 H2 + N2 At a certain temperature at equilibrium Pammonia = 4.0 Atm, Phydrogen = 2.0 Atm, & Pnitrogen = 5.0 Atm. Calculate Keq:

  42. Review & Collect Drill & HW

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

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

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

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

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

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