Chemical Equilibrium

1. Chemical Equilibrium I. A State of Dynamic Balance

2. Chemical Equilibrium I. A State of Dynamic Balance -when a ________ results in the almost ________ conversion of ________ to ________, the ________ is said to go to __________, but _____ _________ ___ ____ go to __________, most _________ are __________

3. Chemical Equilibrium I. A State of Dynamic Balance -as soon as the ________ ________ begins, the ____________ of the _________ go _____, and the _________ _____ goes _____ as the number of __________ per unit ____ goes _____

4. Chemical Equilibrium I. A State of Dynamic Balance -as the _________ proceeds, the ____ of the ________ _________ continues to ________ and the ____ of the ________ ________ continues to ________ until the two _____ are _____, and the system has reached a state of ________ __________

5. Chemical Equilibrium I. A State of Dynamic Balance -at ___________, the ____________ of the ________ and ________ are not _____, but _______, because the ____ of _________ of the ________ is _____ to the ____ of _________ of the ________

6. Chemical Equilibrium II. Equilibrium Expressions and Constants -while _____ chemical systems have little tendency to _____, and _____ chemical systems _____ readily and ___ to __________, _____ chemical systems reach a _____ of __________, leaving varying amounts of ________ ____________ -in 1864, Norwegian chemists ______ and _________ proposed the _______ ___________________, which states, at a given ___________, a chemical system may reach a _____ in which a particular _____ of _______ and _______ ____________ has a _______ value

7. Chemical Equilibrium II. Equilibrium Expressions and Constants -the _______ ________ for a _______ at __________ can be written ______________________________, where __ and __ are ________, __ and __ are ________, __, __, __, and __ are the ___________ in the ________ ________, and the __________ _______ __________ is -___________ ________ with ___ values __ __ contain more ________ than ________ at ___________, while __________ ________ with ___ values __ __ contain more ________ than ________ at __________

8. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the homogeneous equilibrium for the synthesis of ammonia from nitrogen and hydrogen.

9. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the equilibrium for the synthesis of Hydrogen iodide from iodine and hydrogen.

10. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the equilibrium for the decomposition of Dinitrogen tetroxide into Nitrogen dioxide.

11. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the equilibrium for the reaction of Carbon monoxide and Hydrogen which produces methane (Tetrahydrogen monocarbide) and water.

12. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the equilibrium for the decomposition of Dihydrogen monosulfide into diatomic hydrogen and diatomic sulfur.

13. Chemical Equilibrium II. Equilibrium Expressions and Constants -_________ in which all ________ and ________ are in the same ________ _____ are ____________, but ________ with _________ and ________ in _____ than ___ ________ _____ result in _____________ _________

14. Chemical Equilibrium II. Equilibrium Expressions and Constants -since ______ and _____ ________ and ________ don’t change ___________, (which is really their ______), if the ___________ remains ________, then in the ___________ _______ __________ for a ____________ ___________, the ___________ ________ only depends on the ______________ of the ________ and ________ in the _______ state of matter

15. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the heterogeneous equilibrium for the decomposition of Sodium Hydrogen carbonate into Sodium carbonate, Carbon dioxide, and water.

16. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the heterogeneous equilibrium for the decomposition of Calcium carbonate into Calcium oxide and Carbon dioxide.

17. Chemical Equilibrium Name_________________ II. Equilibrium Expressions and Constants Write the complete, balanced thermochemical equation and equilibrium constant expression for the homogeneous equilibrium for the reaction of hydrazine (Tetrahydrogen dinitride) and Nitrogen dioxide, which produces nitrogen and water.

18. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the complete, balanced thermochemical equation and equilibrium constant expression for the homogeneous equilibrium for the reaction of Sulfur trioxide and Carbon dioxide, which produces Carbon disulfide and oxygen.

19. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the complete, balanced thermochemical equation and equilibrium constant expression for the heterogeneous equilibrium for the reaction of monatomic Sulfur and fluorine gas, which produces Sulfur tetrafluoride gas and Sulfur hexafluoride gas.

20. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the complete, balanced thermochemical equation and equilibrium constant expression for the heterogeneous equilibrium for the reaction of magnatite (Fe3O4) and hydrogen gas, which produces iron and water vapor.

21. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the homogeneous equilibrium for the synthesis of ammonia and calculate the value of Keq when [NH3] = 0.933 M, [N2] = 0.533 M, and [H2] = 1.600 M.

22. Chemical Equilibrium II. Equilibrium Expressions and Constants Write the equilibrium constant expression for the homogeneous equilibrium for the decomposition of Sulfur trioxide into Sulfur dioxide and oxygen gas, and calculate the value of Keq when [SO3] = 0.0160 M, [SO2] = 0.00560 M, and [O2] = 0.00210 M.

23. Chemical Equilibrium III. Le Châtelier’s Principle 1. Hypothesis: 2. Prediction: 3. Gather Data: A. Safety: B. Procedure:

24. Chemical Equilibrium III. Le Châtelier’s Principle 3. Gather Data: B. Procedure:

25. Chemical Equilibrium III. Le Châtelier’s Principle 4. Analyze Data: 5. Draw Conclusions:

26. Chemical Equilibrium III. Le Châtelier’s Principle -________ that reach __________ instead of going to __________ do not ________ as much -in 1888, ________________________ discovered that there are ways to _______ _________ in order to make _________ more __________ -____________________ states that if a ______ (like a ______ in __________) is applied to a system at __________, the system _____ in the ________ that _______ the _____

27. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium A. Changes in Concentration Write the equilibrium constant expression for the equilibrium for the reaction of Carbon monoxide and Hydrogen to produce methane and water. Then, calculate the Keq value when [CO] = 0.30000 M, [H2] = 0.10000 M, and [CH4] = 0.05900 M, and [H2O] = 0.02000 M.

28. Chemical Equilibrium III. Le Châtelier’s Principle A. Changes in Concentration -_________ the ____________ of ___ _________ the _______ of _________ between ___ and ___, _________ the _____ of the _______ _______ -the system responds to the ______ of the addition of _______ by forming more _______ to bring the system back into equilbrium

29. Chemical Equilibrium III. Le Châtelier’s Principle A. Changes in Concentration

30. Chemical Equilibrium III. Le Châtelier’s Principle A. Changes in Concentration -_________ the ____________ of a ________ causes __________ to _____ to the ____ to _______ the ____ of formation of ______ -_________ the ____________ of a ________ causes __________ to _____ to the ____ to _______ the ____ of formation of ______

31. Chemical Equilibrium III. Le Châtelier’s Principle A. Changes in Concentration Predict what should happen to the following equilibrium if hydrogen bonding due to the addition of acetone binds water and effectively removes it from the products.

32. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium A. Changes in Volume -_________ the ______ of the _______ container, according to ______, ________ the ________, which in turn ________ the _____ of _________ between the ________ of the ________, _________ the _____ of the ________ _______ -the _____ in the _________ causes the _____ on the system to be _______ as for every __ _____ of _______ _______ _________, only __ _____ of _______ _______ are _________, which, according to ________, occupies __ the ______, which _________ the ________

33. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium Use Le Châtelier’s Principle to predict how each of these changes would affect the ammonia equilibrium system. a. removing hydrogen from the system __________________________ b. adding ammonia to the system _______________________________

34. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium Use Le Châtelier’s Principle to predict how each of these changes would affect the ammonia equilibrium system. 1N2 (g) + 3H2(g) 2NH3(g) c. adding hydrogen to the system _______________________________

35. Chemical Equilibrium 2SO2 (g) + 1O2(g) 2SO3(g) III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium How would decreasing the volume of the reaction container affect each of these equilibria? a. _________________________ b. _____________________________ 1H2 (g) + 1Cl2(g) 2HCl(g) c. _________________________ 2NOBr(g) 2NO(g) + 1Br2(g)

36. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium A. Changes in Temperature -while _______ in _____________ and ________ in _______ cause ______ in _________, they ___ ___ _______ the __________ _______, but a ______ in ___________ causes ______ in both the __________ ________ and the __________ _______

37. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium A. Changes in Temperature -since the _______ for making _______ has a _______ ____, the ________ _______ is _________, and the _______ _______ is __________, so ____ can be thought of as a _______ in the ________ _______ and a _______ in the _______ _______

38. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium A. Changes in Temperature -_________ the __________ is like _______ more _______ to the _______ in which _____ acts as a _______ and is _____ ___, in this case, the __________ _______ _______ -__________ shifts to the _____, _________ the ___________ of _______ because _______ is a _______ in the _______ _______

39. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium A. Changes in Temperature -_________ the __________ is like ________ _______ from the _______ in which _____ acts as a _______, in this case, the __________ _______ _______ -__________ shifts to the _____, _________ the ___________ of _______ because _______ is a _______ in the _______ _______

40. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium In the following equilibrium, would you raise or lower the temperature to get the following results? a. increase the amount of CH3CHO______________________________ b. decrease the amount of C2H2 ________________________________

41. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium In the following equilibrium, would you raise or lower the temperature to get the following results? 1C2H2 (g) + 1H2O(g) 1CH3CHO(g) ΔH0 = -151 kJ c. increase the amount of H2O _________________________________

42. Chemical Equilibrium III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium In the following equilibrium, what effect does changing the volume of the reaction vessel have? ______________________________________________________________________________________________________________________________________________________________________________ In the following equilibrium, what effect does simultaneously increasing the temperature and the pressure have? ______________________________________________________________________________________________________________________________________________________________________________

43. Chemical Equilibrium III. Le Châtelier’s Principle 1. Hypothesis: 2. Prediction: 3. Gather Data: A. Safety:

44. Chemical Equilibrium III. Le Châtelier’s Principle 3. Gather Data: B. Procedure:

45. Chemical Equilibrium III. Le Châtelier’s Principle 3. Gather Data: B. Procedure: 4. Analyze Data: A. The equation for the reversible reaction in this experiment is:

46. Chemical Equilibrium III. Le Châtelier’s Principle 4. Analyze Data: A. Use the equation to explain the colors of the solution in steps 1, 2, and 3

47. Chemical Equilibrium III. Le Châtelier’s Principle 4. Analyze Data: B. Explain how the equilibrium shifts when heat energy is added or removed. 5. Draw Conclusions:

48. Chemical Equilibrium IV. Using Equilibrium Constants -when a ________ has a _____ ___, the __________ _______ contains _____ ________ than ________ at __________ -when a ________ has a _____ ___, the __________ _______ contains _____ ________ than ________ at __________ A. Calculating Equilibrium Concentrations -__________ ________ can also be used to ________ the __________ ____________ of any ________ in the _______

49. Chemical Equilibrium IV. Using Equilibrium Constants A. Calculating Equilibrium Concentrations At 1200 K, the Keq for the following reaction equals 3.933. What is the concentration of the methane produced, if [CO] = 0.850 M, [H2] = 1.333 M, and [H2O] = 0.286 M?

50. Chemical Equilibrium IV. Using Equilibrium Constants A. Calculating Equilibrium Concentrations At 1405 K, the Keq for the following reaction equals 2.27 x 10-3. What is the concentration of the Hydrogen gas produced, if [S2] = 0.0540 M, and [H2S] = 0.184 M?