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Name: Date: Period: ACADEMIC Chapter 16 Review Sheet Vocabulary reversible reaction chemical equilibrium law of mass action equilibrium constant equilibrium expression law of chemical equilibrium equilibrium position homogeneous equilibria heterogeneous equilibria reaction quotient Le Chatelier’s principle Haber process Section 16-1 1. 2. 3. 4. 5. What is the relationship between concentration and rate? True or False. At equilibrium, the concentrations of reactants and products remain constant which means that the reaction has stopped. What are three factors that control the rate of reaction? Can all reversible reactions be observed in the laboratory? Why or why not? Why is chemical equilibrium referred to as a dynamic equilibrium? Section 16-2 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. What do the brackets mean in the equilibrium expression? If the Keq for the forward reaction is 5, what is the Keq’ for the reverse reaction? Write the equilibrium expression for 2 NO2(g) N2O4(g). Make sure you write “Keq =” and there is no plus sign in the equilibrium constant expression. Write the equilibrium expression for 2 CO(g) + O 2(g) 2 CO2(g). What does it mean if the Keq is much greater than 1? What does it mean if the Keq is much smaller than 1 (like 0.001)? What does it mean if the Keq is around 1? Write the equilibrium expression for KCl(l) + Na(l) NaCl(l) + K(g). NOTE: liquids and solids are not included in the equilibrium expression. Write the equilibrium expression for 2 NO(g) + 2 H 2(g) N2(g) + 2 H2O(l). At 340C, Keq = 0.064 for the reaction Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O(g). Given the [H2] = 0.45 M and [H2O] = 0.37 M, find Q and predict how the reaction will proceed. Ammonia is synthesized from nitrogen and hydrogen in the reaction N 2(g) + 3H2(g) 2NH3(g). At 500C, the equilibrium constant for this reaction is 0.080. Given that [NH3] = 0.0596 M, [N2] = 0.600 M, and [H2] = 0.420 M, find Q and predict how the reaction will proceed. How is the reaction quotient related to the equilibrium constant? In other words, how are they different, the same? Section 16-3 18. How does the reaction shift to reestablish equilibrium if you add more CO to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? 19. How does the reaction shift to reestablish equilibrium if you take away CO to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? 20. How does the reaction shift to reestablish equilibrium if you add more CO 2 to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? 21. How does the reaction shift to reestablish equilibrium if you take away CO2 to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? 22. How does the reaction shift to reestablish equilibrium if you increase the pressure in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? 23. How does the reaction shift to reestablish equilibrium if you increase the temperature in the following reaction: NH4Cl(s) NH3(g) + HCl(g) where the H is negative.? 24. Describe Le Chatelier’s principle. 25. What factors alter the equilibrium position in chemical reactions? Name: Date: Period: ACADEMIC Chapter 16 Review Sheet Vocabulary reversible reaction chemical equilibrium law of mass action equilibrium constant equilibrium expression law of chemical equilibrium equilibrium position homogeneous equilibria heterogeneous equilibria reaction quotient Le Chatelier’s principle Haber process Section 16-1 1. 2. 3. 4. 5. What is the relationship between concentration and rate? (ANS: The greater the concentration, the faster the rate.) True or False. At equilibrium, the concentrations of reactants and products remain constant which means that the reaction has stopped. (ANS: False) What are three factors that control the rate of reaction? (ANS: Concentration, temperature and pressure) Can all reversible reactions be observed in the laboratory? Why or why not? (ANS: Sometimes the reverse reaction is so small that it cannot be observed.) Why is chemical equilibrium referred to as a dynamic equilibrium? (ANS: Dynamic means changing; it means that even at equilibrium, the reaction continues to proceed.) Section 16-2 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. What do the brackets mean in the equilibrium expression? (ANS: molarity) If the Keq for the forward reaction is 5, what is the Keq’ for the reverse reaction? (ANS: 1/5) Write the equilibrium expression for 2 NO2(g) N2O4(g). Make sure you write “Keq =” and there is no plus sign in the equilibrium constant expression. (ANS: Keq = [N2O4]/[NO2]2) Write the equilibrium expression for 2 CO(g) + O 2(g) 2 CO2(g). (ANS: Keq = [CO2]2/([CO]2[O2])) What does it mean if the Keq is much greater than 1? (ANS: The equilibrium favors products.) What does it mean if the Keq is much smaller than 1 (like 0.001)? (ANS: The equilibrium favors reactants) What does it mean if the Keq is around 1? (ANS: There is a lot of both reactants and products.) Write the equilibrium expression for KCl(l) + Na(l) NaCl(l) + K(g). NOTE: liquids and solids are not included in the equilibrium expression. (ANS: Keq = [K]) Write the equilibrium expression for 2 NO(g) + 2 H 2(g) N2(g) + 2 H2O(l). (ANS: Keq = [N2]/([NO]2[H2]2)) At 340C, Keq = 0.064 for the reaction Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O(g). Given the [H2] = 0.45 M and [H2O] = 0.37 M, find Q and predict how the reaction will proceed. (ANS: Q = 0.556 which is greater than Keq therefore the reaction will shift to the REACTANTS to reach equilibrium.) Ammonia is synthesized from nitrogen and hydrogen in the reaction N 2(g) + 3H2(g) 2NH3(g). At 500C, the equilibrium constant for this reaction is 0.080. Given that [NH 3] = 0.0596 M, [N2] = 0.600 M, and [H2] = 0.420 M, find Q and predict how the reaction will proceed. (ANS: Q = 0.0800 which is equal to the Keq therefore it is already at equilibiurm.) How is the reaction quotient related to the equilibrium constant? In other words, how are they different, the same? (ANS: They differ in the time they are measured; K is measured at equilibrium only and Q is measured at anytime. They are the same with respect to their equation; they have the same equation.) Section 16-3 18. How does the reaction shift to reestablish equilibrium if you add more CO to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? (ANS: It will shift to PRODUCTS.) 19. How does the reaction shift to reestablish equilibrium if you take away CO to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? (ANS: It will shift to REACTANTS.) 20. How does the reaction shift to reestablish equilibrium if you add more CO 2 to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? (ANS: It will shift to REACTANTS.) 21. How does the reaction shift to reestablish equilibrium if you take away CO2 to the system in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? (ANS: It will shift to PRODUCTS.) 22. How does the reaction shift to reestablish equilibrium if you increase the pressure in the following reaction: 2 CO(g) + O2(g) 2 CO2(g)? (ANS: It will shift to the PRODUCTS.) 23. How does the reaction shift to reestablish equilibrium if you increase the temperature in the following reaction: NH4Cl(s) NH3(g) + HCl(g) where the H is negative? (ANS: It will shift to the REACTANTS.) 24. Describe Le Chatelier’s principle. (ANS: The reaction will shift to minimize the disturbance to reestablish equilibrium.) 25. What factors alter the equilibrium position in chemical reactions? (ANS: Concentration, Pressure and temperature)