1. Equilibrium Calculations Example 4—Using Trial K eq to Predict Which Way a Reaction Will Move to Reach Equilibrium

2. What we do in this type of problem is:

3. 1.Write the K eq expression.

4. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression.

5. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression

6. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression and find the Trial K eq

7. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression and find the Trial K eq (or Trial Quotient “ Q ”).

8. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression and find the Trial K eq (or Trial Quotient “Q ”). 4.Compare Trial K eq with the Actual K eq :

9. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression and find the Trial K eq (or Trial Quotient “Q ”). 4.Compare Trial K eq with the Actual K eq :

10. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression and find the Trial K eq (or Trial Quotient “Q ”). 4.Compare Trial K eq with the Actual K eq : If Trial K eq < Actual K eq, the reaction will move to the right.

11. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression and find the Trial K eq (or Trial Quotient “Q ”). 4.Compare Trial K eq with the Actual K eq : If Trial K eq < Actual K eq, the reaction will move to the right. If Trial K eq > Actual K eq, the reaction will move to the left.

12. What we do in this type of problem is: 1.Write the K eq expression. 2.Insert initial concentrations of all species in the K eq expression. 3.Evaluate the expression and find the Trial K eq (or Trial Quotient “Q ”). 4.Compare Trial K eq with the Actual K eq : If Trial K eq < Actual K eq, the reaction will move to the right. If Trial K eq > Actual K eq, the reaction will move to the left. If Trial K eq = Actual K eq, the reaction is already at equilibrium and will not move.

13. Here’s an example:

14. At 35°C, K eq for the reaction

15. Here’s an example: At 35°C, K eq for the reaction 2NO (g) + Cl 2(g)  2NOCl (g)

16. Here’s an example: At 35°C, K eq for the reaction 2NO (g) + Cl 2(g)  2NOCl (g) is 6.25 × 10 4

17. Here’s an example: At 35°C, K eq for the reaction 2NO (g) + Cl 2(g)  2NOCl (g) is 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask

18. Here’s an example: At 35°C, K eq for the reaction 2NO (g) + Cl 2(g)  2NOCl (g) is 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C.

19. Here’s an example: At 35°C, K eq for the reaction 2NO (g) + Cl 2(g)  2NOCl (g) is 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a)Will the reaction move to the left or right in order to establish equilibrium?

20. Here’s an example: At 35°C, K eq for the reaction 2NO (g) + Cl 2(g)  2NOCl (g) is 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a)Will the reaction move to the left or right in order to establish equilibrium? b)Will the [NOCl] increase or decrease as equilibrium is being established?

21. Here’s an example: At 35°C, K eq for the reaction 2NO (g) + Cl 2(g)  2NOCl (g) is 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a)Will the reaction move to the left or right in order to establish equilibrium? b)Will the [NOCl] increase or decrease as equilibrium is being established? c)Will the total pressure in the container increase or decrease as equilibrium is being established?

22. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

23. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

24. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

25. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

26. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

27. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species: Initial [NO]

28. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

29. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

30. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

31. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species: Initial [Cl 2 ]

32. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

33. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

34. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species:

35. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? First we find initial concentrations of all the species: Initial [NOCl]

36. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Initial [NO]

37. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

38. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Initial [Cl 2 ]

39. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

40. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Initial [NOCl]

41. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

42. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

43. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

44. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

45. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

46. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

47. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

48. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

49. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

50. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

51. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

52. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Evaluate this to find the Trial K eq

53. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 Initial [NO] = 0.0200 M Initial [Cl 2 ] = 0.0400 M Initial [NOCl] = 0.900 M 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq

54. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq Actual K eq

55. 2NO (g) + Cl 2(g)  2NOCl (g) K eq = 6.25 × 10 4 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq Actual K eq Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < The Trial K eq is smaller than the Actual K eq

56. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 <

57. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < If Trial K eq < Actual K eq

58. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < If Trial K eq < Actual K eq The product/reactant ratio is lower than it is at equilibrium

59. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < If Trial K eq < Actual K eq The product/reactant ratio is lower than it is at equilibrium The reaction will move to the RIGHT

60. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < If Trial K eq < Actual K eq The product/reactant ratio is lower than it is at equilibrium The reaction will move to the RIGHT As the reaction moves right, reactants form products,

61. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < If Trial K eq < Actual K eq The product/reactant ratio is lower than it is at equilibrium The reaction will move to the RIGHT As the reaction moves right, reactants form products, so the RATIO of products to reactants (which began as 5.06 × 10 4 ), is going up.

62. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < If Trial K eq < Actual K eq The product/reactant ratio is lower than it is at equilibrium The reaction will move to the RIGHT As the reaction moves right, reactants form products, so the RATIO of products to reactants (which began as 5.06 × 10 4 ), is going up. When it reaches 6.25 × 10 4, equilibrium will be established!

63. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium?

64. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. a) Will the reaction move to the left or right in order to establish equilibrium? Trial K eq 5.06 × 10 4 Actual K eq 6.25 × 10 4 < Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium.

65. 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. b)Will the [NOCl] increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. 2NO (g) + Cl 2(g)  2NOCl (g)

66. 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. b)Will the [NOCl] increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. 2NO (g) + Cl 2(g)  2NOCl (g)

67. 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. b)Will the [NOCl] increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium

68. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. b)Will the [NOCl] increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium DECREASE The amount of reactants will DECREASE

69. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. b)Will the [NOCl] increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium INCREASE The amount of product will INCREASE The amount of reactants will DECREASE

70. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. b)Will the [NOCl] increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium The amount of product will INCREASE The [NOCl] will increase as equilibrium is being established.

71. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium

72. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 3 mol of gas

73. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 1 3 mol of gas

74. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 1 3 mol of gas 2 mol of gas

75. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 1 3 mol of gas 2 mol of gas

76. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 1 3 mol of gas 2 mol of gas

77. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 3 mol of gas 2 mol of gas 1

78. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 3 mol of gas 2 mol of gas 1 DECREASES The number of moles of gas DECREASES

79. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? Because Trial K eq < Actual K eq The reaction will move to the RIGHT in order to establish equilibrium. Moves to the Right to Achieve Equilibrium 3 mol of gas 2 mol of gas 1 DECREASES The number of moles of gas DECREASES decreases The total pressure decreases

80. 2NO (g) + Cl 2(g)  2NOCl (g) 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C. c)Will the total pressure in the container increase or decrease as equilibrium is being established? When 0.100 mol NO, 0.200 mol Cl 2, and 4.50 mol NOCl are added to an empty 5.00 L flask and the temperature is maintained at 35°C, as equilibrium is being established the total pressure decreases.