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JEOPARDY!

JEOPARDY!. Click Once to Begin. Chemistry Final Review Chapter 8: Equilibrium. JEOPARDY!. Equilibrium. Equilibrium Constants. LeChatelier’s Principle and Reaction Quotients. LeChatelier’s Principle and Reaction Quotients, Part II. Calculations with Q and K. Misc. 100. 100. 100. 100.

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JEOPARDY!

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  1. JEOPARDY! Click Once to Begin Chemistry Final Review Chapter 8: Equilibrium

  2. JEOPARDY! Equilibrium Equilibrium Constants LeChatelier’s Principle and Reaction Quotients LeChatelier’s Principle and Reaction Quotients, Part II Calculations with Q and K Misc. 100 100 100 100 100 100 200 200 200 200 200 200 300 300 300 300 300 300 400 400 400 400 400 400 500 500 500 500 500 500

  3. What type of reaction occurs when reactants can form products and products can form reactants? Equilibrium - 100

  4. Equilibrium - 100 Reversible Reactions

  5. Equilibrium - 200 When is chemical equilibrium achieved?

  6. Equilibrium - 200 When the rate of forward reaction equals the rate of reverse reaction.

  7. Equilibrium - 300 At which point is equilibrium achieved?

  8. Equilibrium - 300 B!!

  9. Equilibrium - 400 Has a system at equilibrium stopped reacting? Why or why not?

  10. Equilibrium - 400 No. The system has reached dynamic equilibrium. The reaction keeps occurring, but the rates of forward and reverse reaction are equal.

  11. Equilibrium - 500 Does a Keq of 1 mean the reactant concentration equals the product concentration?

  12. Equilibrium - 500 No, not necessarily. The powers to which concentrations are raised have a large effect on the value of Keq. Ex. 2 A B; 2 M=[A], 4 M = [B] Keq = 4/(2)2 = 4/4 = 1

  13. What is the general form of an equilibrium constant given: a A + b B  c C + d D? Equilibrium Constants - 100

  14. Keq = [C]cD]d [A]a[B]b Equilibrium Constants - 100

  15. Which of the following can be included in an equilibrium expression: Solid Liquid Gas Aqueous solution Equilibrium Constants - 200

  16. Gas and Aqueous solution Equilibrium Constants - 200

  17. True or false: Equilibrium constants do NOT depend on temperature. Equilibrium Constants - 300

  18. False. All equilibrium constants are dependent on temperature Equilibrium Constants - 300

  19. An equilibrium constant much greater than 1 is a _____ favored reaction. Conversely, an equilibrium constant that is much smaller than 1 is _____ favored. Equilibrium Constants - 400

  20. 1st blank: Product 2nd blank: Reactant Equilibrium Constants - 400

  21. What are the units of an equilibrium constant? Equilibrium Constants - 500

  22. There are none!! Equilibrium Constants - 500

  23. LeChatelier’s Principle & Reaction Quotients - 100 Define LeChatelier’s Principle.

  24. LeChatelier’s Principle & Reaction Quotients - 100 When a system at equilibrium is disturbed, the reaction will counteract that shift in order to re-establish equilibrium.

  25. LeChatelier’s Principle & Reaction Quotients - 200 Which side of the reaction will a system shift towards when reactants are added or products are removed?

  26. LeChatelier’s Principle & Reaction Quotients - 200 To the right. (The products)

  27. LeChatelier’s Principle & Reaction Quotients - 300 What is the difference between the reaction quotient (Q) and equilibrium constant (K)?

  28. LeChatelier’s Principle & Reaction Quotients - 300 Reaction quotients are used at any concentrations while equilibrium constants are only used for equilibrium concentrations.

  29. LeChatelier’s Principle & Reaction Quotients - 400 N2(g) + 3 H2(g)  2 NH3 (g) A system of the above reaction is at equilibrium. Which way will the reaction shift if the volume decreases?

  30. LeChatelier’s Principle & Reaction Quotients - 400 To the right. (The products side)

  31. LeChatelier’s Principle & Reaction Quotients - 500 2 SO2 (g) + O2 (g) 2 SO3 (g) H = -197.8 kJ/mol If heat is added to a system with the above reaction at equilibrium, which direction will the reaction proceed?

  32. LeChatelier’s Principle & Reaction Quotients - 500 To the left. (The reactants side)

  33. LeChatelier’s Principle & Reaction Quotients II - 100 Q = K The system is at ________.

  34. LeChatelier’s Principle & Reaction Quotients II - 100 Equilibrium!!

  35. LeChatelier’s Principle & Reaction Quotients II - 200 Q < K Which direction will the system shift?

  36. LeChatelier’s Principle & Reaction Quotients II - 200 To the right. (The prodcuts side)

  37. LeChatelier’s Principle & Reaction Quotients II - 300 The addition of an inert gas or pure solids to a system at equilibrium results in a shift in which direction?

  38. LeChatelier’s Principle & Reaction Quotients II - 300 No change will occur since neither are included in the equilibrium constant expression.

  39. LeChatelier’s Principle & Reaction Quotients II - 400 When Q > K, the reaction shifts left. Why? Daily Double!!!

  40. LeChatelier’s Principle & Reaction Quotients II - 400 The ratio of products to reactants is too high. Shifting left makes more reactants and increases the value of the denominator in the equilibrium expression, thus lowering the value of Keq

  41. LeChatelier’s Principle & Reaction Quotients II - 500 When will changing the volume of a gas container have no effect on the system?

  42. LeChatelier’s Principle & Reaction Quotients II - 500 When equal number of moles of gas are on each side of the balanced equation.

  43. Calculations with Q and K- 100 Write the equilibrium expression for the given reaction: 2 NOCl (g)  2 NO (g) + Cl(g)

  44. Calculations with Q and K- 100 Keq = [NO]2[Cl] [NOCl]

  45. Calculations with Q and K- 200 Calculate Keq. N2 (g) + O2 (g) 2 NO (g) When [N2] = .48 M; [O2] = .75 M and [NO] = .030 M

  46. Calculations with Q and K- 200 Keq = [NO]2 [N2] [O2] = (.030)2 / (.48) (.75) = .0025

  47. Calculations with Q and K- 300 Calculate Q and determine if the system is at equilibrium or not. COCl2 CO (g) + Cl2(g) & Keq = 170 [CO]=[Cl2]=.15M and [COCl2] = .0011

  48. Calculations with Q and K- 300 Q = [CO][Cl2] [COCl2] =(.15)(.15) / .0011 = 20. The system is not at equilibrium

  49. Calculations with Q and K- 400 Calculate Q and determine which direction the system will shift. H2 (g) + I2(g)  2 HI (g) [H2]= .150 M; [I2]= .175 M; and [HI]= .950 M Keq = 50.5

  50. Calculations with Q and K- 400 Q = [HI]2 [H2][I2] = (.950)2 / (.175)(.150) = 34.4 The system will shift right.

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