Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 15.6, Problem 1PPA
Practice Problem
ATTEMPT
For the reaction:
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A chemical equilibrium A ⇄ 2B has a forward rate constant, kf = 12 M –1 s–1, and a reverse rate constant, kr = 18 s–1. If the system has a concentration of [A] = 0.15 M at equilibrium, what is the concentration of B at equilibrium? (no scientific notation)
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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 - These two diagrams represent systems at...Ch. 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 - The first diagram represents a system at...Ch. 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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- Please see attached image for Chemistry problem question Thank youarrow_forwardThe equilibrium for the formation of dinitrogen tetraoxide gas (N204) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: K. = 1.7 x 10-26 at 40.0°C 2 NO2 (g) <→ N2O4 (g) What is the value of Kp at this same temperature? -25 (A) 4.4 x 10 (B) 6.6 x 10-28 (C) 5.2 x 10-27 (D) 6.5 x 10-30 (E) 5.9 x 1025arrow_forwardpts eoch) The equilibrium for the formation of dinitrogen tetraoxide gas (N,0.) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: 2 NO, (g) + N2O4 (g) What is the value of Kpat this same temperature? K = 1.7 x 1026 at 40.0°C (A) (B) (C) (D) (E) 4.4 x 10-25 6.6 x 10-28 5.2 x 1027 6.5 x 10-30 5.9 x 1025arrow_forward
- At a certain temperature, the value of the equilibrium constant, K, for the reaction represented below is 2.0 x 105. What is the value of K for the reverse reaction at the same temperature? H2(g) + Br2(g) = 2HBr(g) (A) -2.0 x 10-5 (B) 5.0 x 10-6 (C) 2.0 x 10-5 (D) 5.0 x 10-5arrow_forwardPlease help with thisarrow_forwardQuestion attachedarrow_forward
- Change the values of Kc to values of KP or the values of KP to values of Kc. (a)Cl2(g) + Br2(g) 2BrCl(g) Kc=4.7 x 10-2 at 25C (b)2SO2(g) + O2(g) 2 SO3(g) Kp=48.2 at 500C (c)CaCl2 x 6H2O(s) CaCl2(s) + 6H2O(g) Kp=5.09 x 10-44 at 25 C (d) H2O(l) H2O (g) Kp= .196 at 60Carrow_forward5. Dinitrogen pentoxide is added to an evacuated rigid container at 25°C. Given that the initial pressure is 1.00 atm and at equi- librium the pressure is 0.500 atm, determine the final pressure in the reaction vessel at equilibrium. 2N2O5(g) = 4NO2(g) + O2(8) (A) 0.750 atm (B) 1.00 atm (C) 1.25 atm (D) 1.75 atmarrow_forwardA flask is charged with 1.600 atm of N2O4(g) and 1.06 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.N2O4(g) 2NO2(g)After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4? atm(b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? Yes, because the partial pressures of all the reactants and products are specified. No, because the value of Kc can be determined experimentally only. Yes, because the temperature is specified. If Kc can be calculated, find the value of Kc. Otherwise, enter 0.arrow_forward
- A flask is charged with 1.540 atm of N2O4(g) and 0.97 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.N2O4(g) 2NO2(g)After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4? atm(b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? No, because the value of Kc can be determined experimentally only.Yes, because the partial pressures of all the reactants and products are specified. Yes, because the temperature is specified. If Kc can be calculated, find the value of Kc. Otherwise, enter 0.arrow_forward9. The equilibrium constant for the reaction 2 BrCl (g) → Br2 (g) + Cl2 (g) at 25°C is Keq = 0.0172. What is the equilibrium constant for the reaction Br2 (g) + Cl2 (g) →2 BrCl (g)? (а) -0.0172 (b) 0.131 (c) 7.62 (d) 58.1 (e) none of thesearrow_forwardA flask is charged with 1.720 atm of N₂O4(g) and 0.88 atm NO₂(g) at 25°C. The equilibrium reaction is given in the equation below. N₂04(9) 2NO₂(g) After equilibrium is reached, the partial pressure of NO₂ is 0.512 atm. (a) What is the equilibrium partial pressure of N₂O4? 1.904 atm (b) Calculate the value of K, for the reaction. 0.137 (c) Is there sufficient information to calculate K for the reaction? O Yes, because the partial pressures of all the reactants and products are specified. Ⓒ Yes, because the temperature is specified. O No, because the value of K. can be determined experimentally only. If K can be calculated, find the value of K. Otherwise, enter 0. 2.30e-4 Xarrow_forward
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