Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 12, Problem 12.99PAE
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Chapter 12 Solutions
Chemistry for Engineering Students
Ch. 12 - list chemical reactions important in the...Ch. 12 - Explain that equilibrium is dynamic, and that at...Ch. 12 - Prob. 3COCh. 12 - calculate equilibrium constants from experimental...Ch. 12 - Prob. 5COCh. 12 - calculate molar solubility from Kspor vice versa.Ch. 12 - Prob. 7COCh. 12 - Prob. 8COCh. 12 - calculate the new equilibrium composition of a...Ch. 12 - Explain the importance of both kinetic and...
Ch. 12 - Identify the first chemical step in the production...Ch. 12 - Explain why the hydration process for concrete is...Ch. 12 - Prob. 12.3PAECh. 12 - 12.4 In what geographical region of the country...Ch. 12 - Prob. 12.5PAECh. 12 - Prob. 12.6PAECh. 12 - Prob. 12.7PAECh. 12 - On your desk is a glass half-filled with water and...Ch. 12 - An equilibrium involving the carbonate and...Ch. 12 - A small quantity of a soluble salt is placed in...Ch. 12 - Prob. 12.11PAECh. 12 - Prob. 12.12PAECh. 12 - Write equilibrium (mass action) expressions for...Ch. 12 - What is the difference between homogeneous...Ch. 12 - Write equilibrium expressions for each of the...Ch. 12 - Write equilibrium expressions for each of the...Ch. 12 - 12.17 Which of the following is more likely to...Ch. 12 - The reaction, 3 H2(g) + N2(g) (g), has the fol...Ch. 12 - 12.19 For each of the following equations, write...Ch. 12 - Consider the following equilibria involving SO2(g)...Ch. 12 - Prob. 12.21PAECh. 12 - Prob. 12.22PAECh. 12 - Prob. 12.23PAECh. 12 - Prob. 12.24PAECh. 12 - Prob. 12.25PAECh. 12 - The following data were collected for the...Ch. 12 - The following data were collected for a system at...Ch. 12 - Prob. 12.28PAECh. 12 - Nitrosyl chloride, NOCI, decomposes to NO and Cl,...Ch. 12 - Hydrogen gas and iodine gas react via the...Ch. 12 - 12.31 A system consisting of 0.100 mole of oxygen...Ch. 12 - Prob. 12.32PAECh. 12 - Prob. 12.33PAECh. 12 - 1’he reaction in Exercise 12.33 was repeated. This...Ch. 12 - In the reaction in Exercise 12.33, another trial...Ch. 12 - The experiment in Exercise 12.33 was redesigned so...Ch. 12 - Again the experiment in Exercise 12.33 was...Ch. 12 - At a particular temperature, the equilibrium...Ch. 12 - A student is simulating the carbonic acid—hydrogen...Ch. 12 - Because carbonic acid undergoes a second...Ch. 12 - Because calcium carbonate is a sink for CO32- in a...Ch. 12 - 12.42 The following reaction is in equilibrium in...Ch. 12 - Prob. 12.43PAECh. 12 - Prob. 12.44PAECh. 12 - The following equilibrium is established in a...Ch. 12 - Write the K_, expression for each of the following...Ch. 12 - Prob. 12.47PAECh. 12 - calculate the molar solubility of the following...Ch. 12 - 12.49 The Safe Drinking Water Act of 1974...Ch. 12 - In Exercise 12.49, what is the allowed...Ch. 12 - Prob. 12.51PAECh. 12 - Because barium sulfate is opaque to X-rays, it is...Ch. 12 - The ore cinnabar (HgS) is an important source of...Ch. 12 - Prob. 12.54PAECh. 12 - From the solubility data given for the following...Ch. 12 - The solubility of magnesium fluoride, MgF2, in...Ch. 12 - Solid Na2SO4 is added slowly to a solution that is...Ch. 12 - Will a precipitate of Mg(OH)2 form when 25.0 mL of...Ch. 12 - Use the web to look up boiler scale and explain...Ch. 12 - Prob. 12.60PAECh. 12 - Prob. 12.61PAECh. 12 - 12.62 Write the formula of the conjugate acid of...Ch. 12 - 12.63 For each of the following reactions,...Ch. 12 - What are the products of each of the following...Ch. 12 - Prob. 12.65PAECh. 12 - Prob. 12.66PAECh. 12 - 12.67 Hydrofluoric acid is a weak acid used in the...Ch. 12 - The pH of a 0.129 M solution of a weak acid, HB,...Ch. 12 - Calculate the pH of a 0.10 M solution of propanoic...Ch. 12 - Find the pH of a 0.115 M solution of NH3(aq).Ch. 12 - Acrylic acid is used in the polymer industry in...Ch. 12 - Prob. 12.72PAECh. 12 - Prob. 12.73PAECh. 12 - Prob. 12.74PAECh. 12 - Cyanic acid (HOCN) is a weak acid with AL, = 3.5 X...Ch. 12 - In a particular experiment, the equilibrium...Ch. 12 - Prob. 12.77PAECh. 12 - Prob. 12.78PAECh. 12 - Prob. 12.79PAECh. 12 - Prob. 12.80PAECh. 12 - Prob. 12.81PAECh. 12 - Prob. 12.82PAECh. 12 - Prob. 12.83PAECh. 12 - Prob. 12.84PAECh. 12 - 12.85 In the figure, orange fish are placed in one...Ch. 12 - For the system in the preceding problem, show the...Ch. 12 - Prob. 12.87PAECh. 12 - Which of the following is more likely to...Ch. 12 - Prob. 12.89PAECh. 12 - Prob. 12.90PAECh. 12 - In the following equilibrium in a closed system,...Ch. 12 - Consider the following system:...Ch. 12 - The decomposition of NH4HS , NH4HS(s)NH3(g)+H2S(g)...Ch. 12 - You are designing a process to remove carbonate...Ch. 12 - Equal amounts of two gases, A and B3, are placed...Ch. 12 - Prob. 12.96PAECh. 12 - Prob. 12.97PAECh. 12 - Prob. 12.98PAECh. 12 - Solid CaCO3 ; is placed in a closed container and...Ch. 12 - 12.100 A reaction important in smog formation is...Ch. 12 - 12.101 An engineer working on a design to extract...Ch. 12 - 12.102 A chemical engineer is working to optimize...Ch. 12 - 12.103 Methanol, CH3OH, can be produced by the...Ch. 12 - Prob. 12.104PAECh. 12 - 12.105 Using the kinetic-molecular theory, explain...Ch. 12 - 12.106 The solubility of KCl is 34.7 g per 100 g...Ch. 12 - Prob. 12.107PAECh. 12 - 12.108 A nuclear engineer is considering the...Ch. 12 - 12.109 Copper(II) iodate has a solubility of 0.136...Ch. 12 - 12.110 In Exercise 12.109, what do you predict...Ch. 12 - 12.111 You have three white solids. What...Ch. 12 - Prob. 12.112PAECh. 12 - Prob. 12.113PAECh. 12 - Prob. 12.114PAECh. 12 - Prob. 12.115PAECh. 12 - Prob. 12.116PAECh. 12 - 12.117 The vapor pressure of water at 80.0 °C is...Ch. 12 - Prob. 12.118PAE
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- Write the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)arrow_forwardCalculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.arrow_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forward
- Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forwardThe equilibrium constant for the reaction N2(g) + O2(g) 2 NO(g) is 1.7 103 at 2300 K. (a) What is K for the reaction when written as follows? N2(g) + O2(g) NO(g) (b) What is K for the following reaction? 2 NO(g) N2(g) + O2(g)arrow_forwardBecause 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?arrow_forward
- . Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for K for each process. a. AgIO3(s) c. Zn3(PO4)2(s) b. Sn(OH)2(s) d. BaF2(s)arrow_forwardThe value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.arrow_forwardWrite 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)arrow_forward
- In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.arrow_forwardThe creation of shells by mollusk species is a fascinating process. By utilizing the Ca2+ in their food and aqueous environment, as well as some complex equilibrium processes, a hard calcium carbonate shell can be produced. One important equilibrium reaction in this complex process is HCO3(aq)H+(aq)+CO32(aq)K=5.61011 If 0.16 mole of HCO3 is placed into 1.00 L of solution, what will be the equilibrium concentration of CO32?arrow_forwardWhat is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.arrow_forward
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