Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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- Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?arrow_forwardHydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]arrow_forwardThe equilibrium constant (Kc) for this reaction is 5.0 at a given temperature. CO(g)+H2O(g)CO2(g)+H2(g) (a) On analysis, an equilibrium mixture of the substances present at the given temperature was found to contain 0.20 mol of CO, 0.30 mol of water vapor, and 0.90 mol of H2 in a liter. How many moles of CO2 were there in the equilibrium mixture? (b) Maintaining the same temperature, additional H2 was added to the system, and some water vapor was removed by drying. A new equilibrium mixture was thereby established containing 0.40 mol of CO, 0.30 mol of water vapor, and 1.2 mol of H2 in a liter. How many moles of CO2 were in the new equilibrium mixture? Compare this with the quantity in part (a), and discuss whether the second value is reasonable. Explain how it is possible for the water vapor concentration to be the same in the two equilibrium solutions even though some vapor was removed before the second equilibrium was established.arrow_forward
- Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.arrow_forwardConsider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C, only A, B, and C are present. The partial pressures of A, B, and D are given as PA, PB, and PD. Equilibrium is established 18 minutes after the reaction starts. Use terms is less than (LT), is greater than (GT), is equal to (EQ), or insufficient information (X) to answer the following questions. (a) PD at 5 min PA. (b) PA at 21 min PA at 27 min. (c) PB at 7 min PB at 13 min.(d) After 20 min, more B is added. When equilibrium is reestablished, K before the addition K after the addition. (e) After 20 min, the temperature is increased to 35C. PA before the temperature increase PA after the temperature increase after equilibrium is reestablished.arrow_forwardConsider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.arrow_forward
- 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?arrow_forwardA 0.72-m01 sample of PCl5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3(g ) and 0.40 mol of Cl2(g). Calculate the value of the equilibrium constant for the decomposition of PCl5 to PCl3 and Cl2 at this temperature.arrow_forwardConsider the same reaction as in Question 11. In one experiment 1.0 mole of H2O(g) and 1.0 mole of CO(g) are put into a flask and heated to 350C. In a second experiment 1.0 mole of H2(g) and 1.0 mole of CO2(g) are put into another flask with the same volume as the first. This mixture is also heated to 350C. After equilibrium is reached, will there be any difference in the composition of the mixtures in the two flasks?arrow_forward
- Chemical Equilibrium I Part 1: You run the chemical reaction C(aq)+D(aq)2E(aq) at 25C. The equilibrium constant Kc for the reaction at this temperature is 2.0. a Write the equilibrium-constant expression for the reaction. b Can you come up with some possible concentrations of C, D, and E that you might observe when the reaction has reached equilibrium at 25C? What are these values? c A student says that only a very limited number of concentrations for C, D, and E are possible at equilibrium. Is this true? State why you think this is true or is not true. d If you start with 1.0 M concentrations of both C and D and allow the reaction to come to equilibrium, would you expect the concentration of C to have decreased to zero? If not, what would you expect for the concentration of C? (An approximate value is fine.) Part 2: Consider the reaction A(aq)F(aq)+G(aq), whose equilibrium constant is 1.0 105 at 20C. For each of the situations described below, indicate whether any reaction occurs. If reaction does occur, then indicate the direction of that reaction and describe how the concentrations of A, B, F, and G change during this reaction. a A(aq) and B(aq) are mixed together in a container. b F(aq) and G(aq) are mixed together in a container. c A(aq) and F(aq) are mixed together in a container. d B(aq) and G(aq) are mixed together in a container. e Just B(aq) is placed into a container. f Just G(aq) is placed into a container. Consider any one of these situations in which a reaction does occur. At equilibrium, does the reaction mixture have appreciably more products than reactants? If not, how would you describe the equilibrium composition of the reaction mixture? How did you arrive at this answer?arrow_forwardFor a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?arrow_forwardAt 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?arrow_forward
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