こ P = Ac for the following reaction if the equilibrium concentrations are as follows: (HCI)eq = 0.13 M, [HI]eq = 5.6 x 10-16 M, [Cl2leq = 0.0019 M. 2 HCl(g) +12(s) 2 HI(g) + Cl2(g) 6. Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(CO)eq = 6.8 x 10-11 atm, P(O2)eq = 1.3 x 10-3 atm, P(CO2)eq = 0.041 atm. 2 CO(g)+ O2(g) = 2 CO2(g) [PCO [PO₂] [PCD]² (0.0412 (1.3x103) (6.8x1071)2 7. Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = SO3(g) + NO(g) Kc = 0.33 Is the reaction at equilibrium if it contains: 0.39 M SO2, 0.14 M NO2, 0.11 M SO3 and 0.14 M NO. = 2.8x10 [50₂] [NO] If it is not at equilibrium, in which direction will the equilibrium shift? 2] [NO₂] (0.39) (0.14) (0.11) (0.14) = 0.28 which is less than K√o.z , the reaction will Since @skel Proceed to the more produce 8. Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H₂O(g). Product. Tum the page Please C2H4(g) + H2O(g) = C2H5OH(g) [C2H4]eq = 0.015 M volume of [C₂H5OHJeq = 1.69 M Kc = 9.0 x 103

こ P = Ac for the following reaction if the equilibrium concentrations are as follows: (HCI)eq = 0.13 M, [HI]eq = 5.6 x 10-16 M, [Cl2leq = 0.0019 M. 2 HCl(g) +12(s) 2 HI(g) + Cl2(g) 6. Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(CO)eq = 6.8 x 10-11 atm, P(O2)eq = 1.3 x 10-3 atm, P(CO2)eq = 0.041 atm. 2 CO(g)+ O2(g) = 2 CO2(g) [PCO [PO₂] [PCD]² (0.0412 (1.3x103) (6.8x1071)2 7. Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = SO3(g) + NO(g) Kc = 0.33 Is the reaction at equilibrium if it contains: 0.39 M SO2, 0.14 M NO2, 0.11 M SO3 and 0.14 M NO. = 2.8x10 [50₂] [NO] If it is not at equilibrium, in which direction will the equilibrium shift? 2] [NO₂] (0.39) (0.14) (0.11) (0.14) = 0.28 which is less than K√o.z , the reaction will Since @skel Proceed to the more produce 8. Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H₂O(g). Product. Tum the page Please C2H4(g) + H2O(g) = C2H5OH(g) [C2H4]eq = 0.015 M volume of [C₂H5OHJeq = 1.69 M Kc = 9.0 x 103

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 9RQ: What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at...

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Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) 2 H2O(g) + O2(g) (b) CO(g) + O2g CO2(g) (c) C(s) + CO2(g) 2 CO(g) (d) NiO(s) + CO(g) Ni(s) + CO2(g)
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?