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Chapter 8: Equilibrium Jeopardy Game

By: Sarah Dippelhofer. Chapter 8: Equilibrium Jeopardy Game. Jeopardy. Basic Concept of Equilibrium-100. What is the definition of Equilibrium?. Click here to return to game. Equilibrium- When the rate of the forward reaction equals the rate of the reverse reaction in a chemical reaction.

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Chapter 8: Equilibrium Jeopardy Game

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  1. By: Sarah Dippelhofer Chapter 8: EquilibriumJeopardy Game

  2. Jeopardy

  3. Basic Concept of Equilibrium-100 What is the definition of Equilibrium?

  4. Click here to return to game Equilibrium- When the rate of the forward reaction equals the rate of the reverse reaction in a chemical reaction.

  5. Basic Concept of Equilibrium-200 In order for a reaction to occur, what must happen according to the collision theory?

  6. Click here to return to game According to the collision theory, molecules must collide at the correct orientation and with the minimum amount of energy to begin the reaction in order for the reaction to occur.

  7. Basic Concept of Equilibrium-300 • In the following diagram, what do A, B, and C represent? A B C

  8. Click here to return to game A: Forward Reaction B: Point at which Equilibrium is reached C: Reverse Reaction

  9. Basic Concept of Equilibrium-400 Explain the term Dynamic Equilibrium

  10. Click here to return to game • Dynamic Equilibrium- when the reaction proceeds in both the forward and reverse directions at the same rate. At this state the products and reactants no longer change. This makes it seem as though the reaction has stopped.

  11. Basic Concept of Equilibrium-500 Which of the following glasses contains substances involved in a reaction that can achieve equilibrium? How can you tell? Once at equilibrium, do the amount of products and reactants change? A B C

  12. Click here to return to game • Glass C contains substances that can react and reach equilibrium. It is easy to identify that the reaction in glass C can reach equilibrium because it is the only reaction with a double arrow (an arrow facing toward and an arrow facing away from the reactants). This indicates that the reaction occurs in the forward and reverse directions, which is necessary for a reaction to reach equilibrium. At equilibrium, amount of products and reactants remains constant.

  13. Equilibrium Constants- 100 Define the Equilibrium Constant Expression

  14. Click here to return to game Equilibrium Constant Expression- an equation showing the ratio of the concentrations of products to reactants at equilibrium

  15. Equilibrium Constants-200 • Write the Equilibrium Expression for the following equations: • 2 • 2

  16. Click here to return to game • 2 • 2

  17. Equilibrium Constants-300 • Write the Equilibrium Expression for the following reactions:

  18. Click here to return to game

  19. Equilibrium Constants-400 • Write the Equilibrium Constant Expression for • If, at equilibrium, , what is the equilibrium constant?

  20. Click here to return to game • Equilibrium Expression: • Calculating the Constant: • In order to calculate the equilibrium constant for this reaction, you have to first write the equilibrium expression. Then you enter each concentrations in the expression and solve for K (the equilibrium constant).

  21. Equilibrium Constants-500 • Write the Equilibrium Constant Expression for: • Calculate [if the [Fe]=0.70M, [=0.330M, = 0.54M and the equilibrium constant is 0.711 • In which direction does the reaction lie? Explain your reasoning.

  22. Click here to return to game • 0.711 • .605 M • This reaction lies to the left, toward the reactants. You can conclude that the reaction lies to the left because the equilibrium constant is .711, which is less than 1. If the equilibrium constant is less than one, the reaction lies toward the left and the reaction lies to the right if the equilibrium constant is greater than 1.

  23. Reaction Quotients-100 • What is the difference between the equilibrium constant and the reaction quotient?

  24. Click here to return to game • The equilibrium constant is at equilibrium and the reaction quotient is at any point in the reaction.

  25. Reaction Quotients-200 • In the following siduations, where does the reaction lie (which reaction has the fastest rate)? • Q=K • Q>K • Q<K

  26. Click here to return to game • Q=K -System is at equilibrium • Q>K-System will make more reactants to reach equilibrium (lies to the left to make more reactants, so reverse reaction rate is faster) • Q<K-System will make more products to reach equilibrium (lies to the right to make more products, so forward reaction rate is faster)

  27. Reaction Quotients-300 • For CaCO3(s) <--> CaO(s) + CO2(g) • If the pressure of CO2 is .026 atm and the , in which direction does the equation lie?

  28. Click here to return to game • The reaction DOES NOT LIE IN ANY DIRECTION, because it is at equilibrium • If K=Q (which in this case it does) , than the system is at equilibrium and both reactions are occurring at the same rate

  29. Reaction Quotients-400 For N2 (g) + O2 (g)  2 NO (g) If [N2] = 0.71 M, [O2] = 0.78 M and [NO] = 0.120 M, is the reaction at equilibrium if K = 0.0025? If not, which direction will lie to reach equilibrium?

  30. Click here to return to game • Q= .0260 • Q>K , so the reaction is not at equilibrium because Q≠K • Because Q>K, the reaction lies to the left because more reactants need to be made (which requires the reverse reaction to occur at a faster rate)

  31. Reaction Quotients-500 Write the reaction quotient expression for the reaction If the concentration of acetate is .34 M , the concentration of hydronium is .65 M, and the concentration of acetic acid is .97 M, what is the reaction quotient? If the equilibrium constant is .3467, where does the system lie? Explain your reasoning.

  32. Click here to return to game Q =.228 The system lies to the left because Q<K. This indicates that more reactants need to be produced so the system can reach equilibrium.

  33. LeChatelier’s Principle-100 Define LeChatelier’s Principle

  34. Click here to return to game • Le Chatelier’s Principle – If a system at equilibrium is disturbed, it will shift to re-establish equilibrium • In other words, a system will do what ever it takes to adjust the system so that it establishes equilibrium

  35. LeChatelier’s Principle-200 Explain how adding concentrations and decreasing concentrations in a system can establish equilibrium.

  36. Click here to return to game • Adding more products if a reaction lies to the left (Q<K)will help the system establish equilibrium because more products would shift the system further to the left , increasing the reverse reaction rate, which leads to establishing equilibrium. Decreasing the concentration of reactants will have the same effect. • Adding more reactant if a reaction lies to the right (Q<K) will help the system establish equilibrium because it shifts the reaction lies to increase the rate of the forward reaction. Decreasing the concentration of products will have the same effect.

  37. LeChatelier’s Principle-300 • Complete the chart about changes in pressure affecting equilibrium:

  38. Click here to return to game

  39. LeChatelier’s Principle-400 Complete the missing spaces in the chart:

  40. Click here to return to game

  41. LeChatelier’s Principle-500 • Which way would the following changes cause the system to shift given the reaction: • NH4Cl (s)  NH3 (g) + HCl (g) • Add NH3 • Decrease HCl • Increase Pressure • Decrease Volume

  42. Click here to return to game • 1. shift to left because more product was added • 2. Shift to the right because product was less concentrated compared to reactants • Shift left because there are less moles on the reactants side (ratio of reactants moles to product moles is 1:2) • Shift right because increased volume means pressure decreased and a decrease and pressure shifts to what side has the least moles. In this reaction, the reactants have less moles.

  43. Miscellaneous-100 What is the difference between Homogeneous Equilibrium and Heterogeneous Equilibrium?

  44. Click here to return to game • Heterogeneous Equilibrium – There are at least 2 states of matter • Ex: • Homogeneous Equilibrium – All of the species are the same state of matter • Ex: 2 H2 (g) + O2 (g)  2 H2O (l) 2 H2 (g) + O2 (g)  2 H2O (g)

  45. Miscellaneous-200 • What are the two states of matter that are not included in an equilibrium constant expression or reaction quotient expression?

  46. Click here to return to game • Solids and Liquids are not included in wither expression • Only Gases and aqueous solutions are included in the expressions

  47. Miscellaneous-300 What is the equilibrium constant expression for this reaction? If the equilibrium constant is 1.33, what is the concentration of CO2 at equilibrium if the concentration of NaOH is .230 M and the concentration of NaHCO3 is .743 M?

  48. Click here to return to game 1.33=

  49. Miscellaneous-400 • What are the changes that have no affect in the rates of equations in a system shifting? (Explain at least 3 of the 4)

  50. Click here to return to game • Adding a pure solid or liquid will not make a difference because they are not included in equilibrium expressions. • Increasing pressure by adding an inert gas will not make a difference because they are also not in the equilibrium constant expression. • Changing the volume when there are an even number of moles on each side won’t change anything because equal moles means the pressures can not be changed. • Adding a catalyst will not make a difference because it’s not included in the reaction; it only speeds up the reaction.

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