Chemistry
3rd Edition
ISBN: 9780073402734
Author: Julia Burdge
Publisher: MCGRAW-HILL HIGHER EDUCATION
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Chapter 15, Problem 116AP
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Chapter 15 Solutions
Chemistry
Ch. 15.1 - Practice Problem ATTEMPT
In an analysis of the...Ch. 15.1 - Prob. 1PPBCh. 15.1 - Practice Problem CONCEPTUALIZE
Consider the...Ch. 15.2 - Practice ProblemATTEMPT Write the reaction...Ch. 15.2 - Practice Problem BUILD
Write the equation for the...Ch. 15.2 - Practice ProblemCONCEPTUALIZE In principle, in the...Ch. 15.2 - Select the correct equilibrium expression for the...Ch. 15.2 - Prob. 2CPCh. 15.3 - Practice Problem ATTEMPT Write equilibrium...Ch. 15.3 - Practice Problem BUILD
Which of the following...
Ch. 15.3 - Prob. 1PPCCh. 15.3 - Prob. 1CPCh. 15.3 - Prob. 2CPCh. 15.3 - Given the following information: HF ( a q ) ⇄ H +...Ch. 15.3 - Prob. 4CPCh. 15.4 - Practice ProblemATTEMPT The following reactions...Ch. 15.4 - Practice Problem BUILD
The equation represents a...Ch. 15.4 - Practice ProblemCONCEPTUALIZE Consider a chemical...Ch. 15.4 - Use the following information to answer questions...Ch. 15.4 - Prob. 2CPCh. 15.4 - 15.4.3 If for the reaction at a certain...Ch. 15.4 - If K c = 3 for the reaction X + 2Y ⇄ Z at a...Ch. 15.5 - Practice ProblemATTEMPT Write K? expressions for (...Ch. 15.5 - Prob. 1PPBCh. 15.5 - Prob. 1PPCCh. 15.5 - Prob. 1CPCh. 15.5 - Prob. 2CPCh. 15.5 - Prob. 3CPCh. 15.5 - Prob. 4CPCh. 15.5 - Prob. 5CPCh. 15.5 - Prob. 6CPCh. 15.6 - Practice Problem ATTEMPT
For the reaction:
....Ch. 15.6 - Practice ProblemBUILD K p = 2.79 × 10 − 5 for the...Ch. 15.6 - Practice Problem CONCEPTUALIZE
Consider the...Ch. 15.7 - Prob. 1PPACh. 15.7 - Prob. 1PPBCh. 15.7 - Prob. 1PPCCh. 15.8 - Practice ProblemATTEMPT Calculate the equilibrium...Ch. 15.8 - Practice ProblemBUILD Determine the initial...Ch. 15.8 - Practice Problem CONCEPTUALIZE
Consider the...Ch. 15.9 - Prob. 1PPACh. 15.9 - Prob. 1PPBCh. 15.9 - Prob. 1PPCCh. 15.10 - Practice ProblemATTEMPT Aqueous hydrocyanic acid...Ch. 15.10 - Practice Problem BUILD Consider a weak acid, HA,...Ch. 15.10 - Practice ProblemCONCEPTUALIZE Each of the...Ch. 15.11 - Practice Problem ATTEMPT Determine the equilibrium...Ch. 15.11 - Prob. 1PPBCh. 15.11 - Prob. 1PPCCh. 15.12 - Practice ProblemATTEMPT For each change indicated,...Ch. 15.12 - Prob. 1PPBCh. 15.12 - Practice ProblemCONCEPTUALIZE Consider the...Ch. 15.13 - Practice Problem ATTEMPT
For each reaction,...Ch. 15.13 - Practice Problem BUILD
For the following...Ch. 15.13 - Practice Problem CONCEPTUALIZE
Consider the...Ch. 15.14 - Practice Problem ATTEMPT
The reaction of carbon...Ch. 15.14 - Practice Problem BUILD
Consider the hypothetical...Ch. 15.14 - Practice Problem CONCEPTUALIZE
The decomposition...Ch. 15 - The K a for hydrocyanic acid ( HCN ) is 4 .9 × 10...Ch. 15 - 15.2
Determine the concentrations of in a...Ch. 15 - 15.3
Determine the for a weak acid if a 0.10-M...Ch. 15 - Prob. 4KSPCh. 15 - Define equilibrium. Give two examples of a dynamic...Ch. 15 - 15.2 Which of the following statements is correct...Ch. 15 - 15.3 Consider the reversible reaction Explain how...Ch. 15 - What is the law of mass action?Ch. 15 - Briefly describe the importance of equilibrium in...Ch. 15 - Define reaction quotient. How does it differ from...Ch. 15 - Write reaction quotients for the following...Ch. 15 - Write the equation for the reaction that...Ch. 15 - Consider the reaction: 2NO ( g ) + 2H 2 ( g ) ⇄ N...Ch. 15 - The equilibrium constant for the reaction: 2SO 2 (...Ch. 15 - Consider the following equilibrium process at...Ch. 15 - The equilibrium constant for the reaction: 2 H 2 (...Ch. 15 - The first diagram represents a system at...Ch. 15 - Prob. 14QPCh. 15 - Define homogeneous equilibrium and heterogeneous...Ch. 15 - What do the symbols K c and K p represent?Ch. 15 - Write the expressions for the equilibrium...Ch. 15 - Write equilibrium constant expressions for K c ,...Ch. 15 - Write the equilibrium constant expressions for K c...Ch. 15 - 15.20 Write the equation relating to , and define...Ch. 15 - 15.21 The equilibrium constant () for the...Ch. 15 - What is K p at 1273°C for the reaction 2CO ( g ) +...Ch. 15 - 15.23 The equilibrium constant for the...Ch. 15 - 15.24 Consider the reaction:
If the equilibrium...Ch. 15 - 15.25 A reaction vessel contains at equilibrium...Ch. 15 - 15.26 The equilibrium constant Kc for the...Ch. 15 - At equilibrium, the pressure of the reacting...Ch. 15 - The equilibrium constant K p for the reaction: PCl...Ch. 15 - Ammonium carbamate ( NH 4 CO 2 NH 2 ) decomposes...Ch. 15 - The following equilibrium constants were...Ch. 15 - 15.31 At a certain temperature, the following...Ch. 15 - 15.32 Pure phosgene gas , was placed in a 1.50-L...Ch. 15 - Consider the equilibrium: 2 NOBr( g ) ⇄ 2 NO( g...Ch. 15 - The following equilibrium constants have been...Ch. 15 - 15.35 The following equilibrium constants have...Ch. 15 - 15.36 The equilibrium constant for the reaction at...Ch. 15 - The following diagrams represent the equilibrium...Ch. 15 - 15.38 Outline the steps for calculating the...Ch. 15 - 15.39 The equilibrium constant K? for the...Ch. 15 - 15.40 For the synthesis of ammonia:
the...Ch. 15 - For the reaction: H 2 ( g ) + CO 2 ( g ) ⇄ H 2 O (...Ch. 15 - At 1000 K, a sample of pure NO, gas decomposes:...Ch. 15 - The equilibrium constant K c for the reaction H 2...Ch. 15 - The dissociation of molecular iodine into iodine...Ch. 15 - The equilibrium constant Kc for the decomposition...Ch. 15 - 15.46 Consider the following equilibrium process...Ch. 15 - 15.47 Consider the heterogeneous equilibrium...Ch. 15 - The equilibrium constant K c for the reaction: H 2...Ch. 15 - The aqueous reaction: L-glutamate + pyruvate ⇄...Ch. 15 - 15.50 Explain Le Châtelier’s principle. How does...Ch. 15 - Use Le Chatelier's principle to explain why the...Ch. 15 - 15.52 List four factors that can shift the...Ch. 15 - Does the addition of a catalyst have any effects...Ch. 15 - 15.54 Consider the following equilibrium system...Ch. 15 - 15.55 Heating solid sodium bicarbonate in a closed...Ch. 15 - 15.56 Consider the following equilibrium...Ch. 15 - 15.57 What effect does an increase in pressure...Ch. 15 - Prob. 58QPCh. 15 - Consider the following equilibrium process: PCl 5...Ch. 15 - Consider the reaction: 2SO 2 ( g ) ⇄ 2 SO 3 ( g )...Ch. 15 - In the uncatalyzed reaction: N 2 O 4 ( g ) ⇄ 2 NO...Ch. 15 - 15.62 Consider the gas-phase reaction:
Predict...Ch. 15 - Consider the following equilibrium reaction in a...Ch. 15 - 15.64 The following diagrams show the reaction at...Ch. 15 - 15.65 The following diagrams show an equilibrium...Ch. 15 - 15.66 Consider the reaction . The first diagram...Ch. 15 - Prob. 67APCh. 15 - Consider the equilibrium system 3A → B . Sketch...Ch. 15 - Baking soda (sodium bicarbonate) undergoes thermal...Ch. 15 - Consider the following reaction at equilibrium: A...Ch. 15 - Prob. 71APCh. 15 - 15.72 Consider the following reacting...Ch. 15 - 15.73 At a certain temperature and a total...Ch. 15 - The decomposition of ammonium hydrogen sulfide: N...Ch. 15 - 15.75 Consider the following reaction at a certain...Ch. 15 - When heated, ammonium carbamate decomposes as...Ch. 15 - A mixture of 0 .47 mole of H2 and 3 .59 moles of...Ch. 15 - When heated at high temperatures, iodine vapor...Ch. 15 - 15.79 One mole of and three moles of are placed...Ch. 15 - At 1130°C , the equilibrium constant ( K c ) for...Ch. 15 - For the purpose of determining K p using Equation...Ch. 15 - The following diagram represents a gas-phase...Ch. 15 - 15.83 Consider the following reaction at
When...Ch. 15 - 15.84 A quantity of 0.20 mole of carbon dioxide...Ch. 15 - 15.85 When dissolved in water, glucose (com sugar)...Ch. 15 - 15 86 At room temperature, solid iodine is in...Ch. 15 - 15.87 A student placed a few ice cubes in a...Ch. 15 - 15.88 A mixture containing 3.9 moles of and 0.88...Ch. 15 - 15.89 The equilibrium constant for the...Ch. 15 - When heated, a gaseous compound A dissociates as...Ch. 15 - 15.91 When a gas was heated under atmospheric...Ch. 15 - Prob. 92APCh. 15 - A sealed glass bulb contains a mixture of NO 2 and...Ch. 15 - At 20°C , the vapor pressure of water is 0.0231...Ch. 15 - A 2.50-mol sample of NOCl was initially in a...Ch. 15 - 15.96 About 75 percent of hydrogen for industrial...Ch. 15 - Water is a very weak electrolyte that undergoes...Ch. 15 - 15.98 Consider the following reaction, which takes...Ch. 15 - The equilibrium constant Kc for the reaction: 2NH...Ch. 15 - At 25°C, a mixture of NO 2 and N 2 O 4 gases are...Ch. 15 - 15.101 Consider the reaction between and in a...Ch. 15 - In 1899 the German chemist Ludwig Mond developed a...Ch. 15 - For which of the following reactions is K c equal...Ch. 15 - The equilibrium constant K p for the following...Ch. 15 - At 1024°C, , the pressure of oxygen gas from the...Ch. 15 - 15.06 The equilibrium constant for the following...Ch. 15 - 15.107 Industrially, sodium metal is obtained by...Ch. 15 - Consider the equilibrium reaction described in...Ch. 15 - The K p for the reaction: SO 2 Cl 2 ( g ) ⇄ SO 2 (...Ch. 15 - The "boat" form and the “chair" form of...Ch. 15 - A quantity of 6.75 g of SO 2 Cl 2 was placed in a...Ch. 15 - 15.112 Industrial production of ammonia from...Ch. 15 - 15.113 The equilibrium constant for the formation...Ch. 15 - Consider the reaction: 2NO( g )+ O 2 ( g ) ⇄ 2N O...Ch. 15 - The formation of SO 3 from SO 2 and O 2 is an...Ch. 15 - At 25°C , the equilibrium partial pressures of N O...Ch. 15 - 15.117 The vapor pressure of mercury is 0.0020...Ch. 15 - 15.118 Both ' and are important biological ions....Ch. 15 - Photosynthesis can be represented by: 6C O 2 ( g...Ch. 15 - Consider the decomposition of ammonium chloride at...Ch. 15 - 15.121 Eggshells are composed mostly of calcium...Ch. 15 - In the gas phase, nitrogen dioxide is actually a...Ch. 15 - Consider the potential-energy diagrams for two...Ch. 15 - Iodine is sparingly soluble in water but much more...Ch. 15 - The dependence of the equilibrium constant of a...Ch. 15 - Lime ( CaO ) is used to prevent SO 2 from escaping...Ch. 15 - Lime is used to prevent from escaping from the...Ch. 15 - Lime ( CaO ) is used to prevent SO 2 from escaping...Ch. 15 - Lime ( CaO ) is used to prevent SO 2 from escaping...
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- 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.arrow_forwardAt 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forwardDuring an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?arrow_forward
- 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?arrow_forwardExplain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?arrow_forward12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?arrow_forward
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