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Chemistry: The Central Science, 10th edition

Chemistry: The Central Science, 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten. Chapter 15 Chemical Equilibrium. Todd Austell, The University of North Carolina  2006, Pearson Prentice Hall. a. moles of reactant always equals moles of product.

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Chemistry: The Central Science, 10th edition

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  1. Chemistry: The Central Science, 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 15Chemical Equilibrium Todd Austell, The University of North Carolina  2006, Pearson Prentice Hall

  2. a. • moles of reactant always equals moles of product. • mass of reactant always equals mass of product. • the rates of opposing reactions are equal. • cannot be determined without temperature information.

  3. a. • moles of reactant always equals moles of product. • mass of reactant always equals mass of product. • the rates of opposing reactions are equal. • cannot be determined without temperature information.

  4. b. • the constant will be greater than 1. • the constant will be less than 1. • the constant will be equal to the square of the forward reaction rate. • cannot determine without temperature information.

  5. b. • the constant will be greater than 1. • the constant will be less than 1. • the constant will be equal to the square of the forward reaction rate. • cannot determine without temperature information.

  6. no bubbles are observed in the reaction mix. • the temperature of the reaction mix cools. • the concentrations of reactants and products no longer change. • the color of the reaction mix remains constant.

  7. no bubbles are observed in the reaction mix. • the temperature of the reaction mix cools. • the concentrations of reactants and products no longer change. • the color of the reaction mix remains constant.

  8. Kc is 2nd order with respect to NO2 and 1st order with respect to N2O4. • Kc is independent of the starting concentrations of reactants and products. • Kc is 2nd order with respect to NO2 and inversely related to N2O4. • Kc is directly related to NO2 and inversely related to N2O4.

  9. Kc is 2nd order with respect to NO2 and 1st order with respect to N2O4. • Kc is independent of the starting concentrations of reactants and products. • Kc is 2nd order with respect to NO2 and inversely related to N2O4. • Kc is directly related to NO2 and inversely related to N2O4.

  10. Kc represents the equil. constant when equil. conc. are expressed in molarity and Kp represents the equil. constant when equil. conc. are expressed in atm. • Kc and Kp are the rate constants expressed in M/time and atm/time respectively. • Kc and Kp are the equil. constants expressed in molarity and atmospheres respectively. • Kc and Kp are the rate contants used to determine rates of solution and gaseous reactions respectively.

  11. Kc represents the equil. constant when equil. conc. are expressed in molarity and Kp represents the equil. constant when equil. conc. are expressed in atm. • Kc and Kp are the rate constants expressed in M/time and atm/time respectively. • Kc and Kp are the equil. constants expressed in molarity and atmospheres respectively. • Kc and Kp are the rate contants used to determine rates of solution and gaseous reactions respectively.

  12. 0.00140 M • 0.00140 (no units) • 0.00140 atm • cannot determine without additional information.

  13. 0.00140 M • 0.00140 (no units) • 0.00140 atm • cannot determine without additional information.

  14. Kp does not change since all coefficients were multiplied by the same number. • the magnitude of the new Kp is 3 times the original Kp. • the magnitude of the new Kp cannot be determined without knowing the energy of reaction. • the new equilibrium constant is equal to (Kp)3.

  15. Kp does not change since all coefficients were multiplied by the same number. • the magnitude of the new Kp is 3 times the original Kp. • the magnitude of the new Kp cannot be determined without knowing the energy of reaction. • the new equilibrium constant is equal to (Kp)3.

  16. Kp = 1/[H2Og] • Kp = PH2O • Kp = [H2Og] • Kp = 1/PH2O

  17. Kp = 1/[H2Og] • Kp = PH2O • Kp = [H2Og] • Kp = 1/PH2O

  18. a. • the equilibrium shifts to the right, using up some of the added O2. • cannot determine what happens without knowing the size of the reaction container. • the equilibrium does not change unless more NO is also added. • the equilibrium shifts to the left, using up some of the NO2.

  19. a. • the equilibrium shifts to the right, using up some of the added O2. • cannot determine what happens without knowing the size of the reaction container. • the equilibrium does not change unless more NO is also added. • the equilibrium shifts to the left, using up some of the NO2.

  20. b. • the amount of O2 in the equilibrium mixture also decreases. • the equilibrium does not change unless more NO2 is added. • the equilibrium shifts to the left, forming more NO. • the equilibrium shifts to the right, forming more NO2.

  21. b. • the amount of O2 in the equilibrium mixture also decreases. • the equilibrium does not change unless more NO2 is added. • the equilibrium shifts to the left, forming more NO. • the equilibrium shifts to the right, forming more NO2.

  22. the equilibrium shifts to the left. • the equilibrium does not change. • the equilibrium shifts to the right. • cannot determine what happens without knowing the magnitude of increase.

  23. the equilibrium shifts to the left. • the equilibrium does not change. • the equilibrium shifts to the right. • cannot determine what happens without knowing the magnitude of increase.

  24. evaporation is an exothermic process and increasing temperature shifts equilibrium to the left. • evaporation is an endothermic process and increasing temperature shifts equilibrium to the right. • evaporation is an endothermic process and increasing temperature shifts equilibrium to the left. • evaporation is an exothermic process and increasing temperature shifts equilibrium to the right.

  25. evaporation is an exothermic process and increasing temperature shifts equilibrium to the left. • evaporation is an endothermic process and increasing temperature shifts equilibrium to the right. • evaporation is an endothermic process and increasing temperature shifts equilibrium to the left. • evaporation is an exothermic process and increasing temperature shifts equilibrium to the right.

  26. cannot determine without information about energy of reaction. • cannot determine without information about reaction rate constant. • no. • yes.

  27. cannot determine without information about energy of reaction. • cannot determine without information about reaction rate constant. • no. • yes.

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