1 Introduction To Chemistry 2 Atoms And Molecules 3 Molecules, Moles, And Chemical Equations 4 Stoichiometry 5 Gases 6 The Periodic Table And Atomic Structure 7 Chemical Bonding And Molecular Structure 8 Molecules And Materials 9 Energy And Chemistry 10 Entropy And The Second Law Of Thermodynamics 11 Chemical Kinetics 12 Chemical Equilibrium 13 Electrochemistry 14 Nuclear Chemistry Chapter12: Chemical Equilibrium
Chapter Questions Section: Chapter Questions
Problem 1CO: list chemical reactions important in the production and weathering of concrete. Problem 2CO: Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates... Problem 3CO Problem 4CO: calculate equilibrium constants from experimental data. Problem 5CO Problem 6CO: calculate molar solubility from Kspor vice versa. Problem 7CO Problem 8CO Problem 9CO: calculate the new equilibrium composition of a system after an applied stress. Problem 10CO: Explain the importance of both kinetic and equilibrium considerations in the design of industrial... Problem 12.1PAE: Identify the first chemical step in the production of Portland cement. How is this reaction related... Problem 12.2PAE: Explain why the hydration process for concrete is exothermic by considering the chemical bonds in... Problem 12.3PAE Problem 12.4PAE: 12.4 In what geographical region of the country would a civil engineer be most likely to use... Problem 12.5PAE Problem 12.6PAE Problem 12.7PAE Problem 12.8PAE: On your desk is a glass half-filled with water and a square glass plate to use as a cover for the... Problem 12.9PAE: An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=*... Problem 12.10PAE: A small quantity of a soluble salt is placed in water. Equilibrium between dissolved and undissolved... Problem 12.11PAE Problem 12.12PAE Problem 12.13PAE: Write equilibrium (mass action) expressions for each of the following reactions. 2 NOBr(g) 2 NO(g) +... Problem 12.14PAE: What is the difference between homogeneous equilibrium and heterogeneous equilibrium? Problem 12.15PAE: Write equilibrium expressions for each of the following heterogeneous equilibria. CaCO,(s) **... Problem 12.16PAE: Write equilibrium expressions for each of the following equilibria. 2 C(s) + O2(g) «=* 2 CO(g) Zn... Problem 12.17PAE: 12.17 Which of the following is more likely to precipitate sulfate ions? PbSO4(s) Pb*+(aq) +... Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures... Problem 12.19PAE: 12.19 For each of the following equations, write the equilibrium expression for the reverse... Problem 12.20PAE: Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants.... Problem 12.21PAE Problem 12.22PAE Problem 12.23PAE Problem 12.24PAE Problem 12.25PAE Problem 12.26PAE: The following data were collected for the reaction, H2(g) + L(g) ** - HI(g), at equilibrium at 25°C:... Problem 12.27PAE: The following data were collected for a system at equilibrium at 140°C. Calculate the equilibrium... Problem 12.28PAE Problem 12.29PAE: Nitrosyl chloride, NOCI, decomposes to NO and Cl, at high temperatures: 2NOCl(g)^2NO(g) + Cl,(g)... Problem 12.30PAE: Hydrogen gas and iodine gas react via the following equation: H2(g) + I2(g)2 HI(g) \ = 76 (at 600 K)... Problem 12.31PAE: 12.31 A system consisting of 0.100 mole of oxygen gas, O2, is placed in a closed 1.00-L container... Problem 12.32PAE Problem 12.33PAE Problem 12.34PAE: 1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was... Problem 12.35PAE: In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial... Problem 12.36PAE: The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of... Problem 12.37PAE: Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was... Problem 12.38PAE: At a particular temperature, the equilibrium constant, A, for the dissociation of N,O4 into NO, is... Problem 12.39PAE: A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2CO5(aq)«=*... Problem 12.40PAE: Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that... Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go... Problem 12.42PAE: 12.42 The following reaction is in equilibrium in lake water: HCO,_(aq) + H+(aq)«=*H,CO,(aq) Predict... Problem 12.43PAE Problem 12.44PAE Problem 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does... Problem 12.46PAE: Write the K_, expression for each of the following equilih ria for dissolution of the salt in water.... Problem 12.47PAE Problem 12.48PAE: calculate the molar solubility of the following compounds. (a) MgF2, (b) Fe(OH)3, (c) Mg3(PO4)2 Problem 12.49PAE: 12.49 The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver... Problem 12.50PAE: In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe... Problem 12.51PAE Problem 12.52PAE: Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make... Problem 12.53PAE: The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility... Problem 12.54PAE Problem 12.55PAE: From the solubility data given for the following com pounds, calculate their solubility product... Problem 12.56PAE: The solubility of magnesium fluoride, MgF2, in water is 0.016 g/L. What is the solubility, in grams... Problem 12.57PAE: Solid Na2SO4 is added slowly to a solution that is 0.10 M in PbfNO,), and 0.10 M in Ba(NO})2. In... Problem 12.58PAE: Will a precipitate of Mg(OH)2 form when 25.0 mL of 0.010 M NaOH is combined with 75.0 mL of a 0.10 M... Problem 12.59PAE: Use the web to look up boiler scale and explain chemically why it is a problem in equipment where... Problem 12.60PAE Problem 12.61PAE Problem 12.62PAE: 12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c)... Problem 12.63PAE: 12.63 For each of the following reactions, indicate the Bronsted-Lowrv acids and bases. What are the... Problem 12.64PAE: What are the products of each of the following acid-base reactions? Indicate the acid and its... Problem 12.65PAE Problem 12.66PAE Problem 12.67PAE: 12.67 Hydrofluoric acid is a weak acid used in the building industry to etch patterns into glass for... Problem 12.68PAE: The pH of a 0.129 M solution of a weak acid, HB, is 2.34. What is Kafor the weak acid? Problem 12.69PAE: Calculate the pH of a 0.10 M solution of propanoic acid and determine its percent ionization. Problem 12.70PAE: Find the pH of a 0.115 M solution of NH3(aq). Problem 12.71PAE: Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’.... Problem 12.72PAE Problem 12.73PAE Problem 12.74PAE Problem 12.75PAE: Cyanic acid (HOCN) is a weak acid with AL, = 3.5 X IO-4. Consider the titration of 25.0 inL of 0.125... Problem 12.76PAE: In a particular experiment, the equilibrium constant measured for the reaction,... Problem 12.77PAE Problem 12.78PAE Problem 12.79PAE Problem 12.80PAE Problem 12.81PAE Problem 12.82PAE Problem 12.83PAE Problem 12.84PAE Problem 12.85PAE: 12.85 In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium.... Problem 12.86PAE: For the system in the preceding problem, show the equilibrium condition in terms of the rates of the... Problem 12.87PAE Problem 12.88PAE: Which of the following is more likely to precipitate the hydroxide ion? Cu(OH)2(s) *=» Ctr+(aq) + 2... Problem 12.89PAE Problem 12.90PAE Problem 12.91PAE: In the following equilibrium in a closed system, indicate how the equilibrium is shifted by the... Problem 12.92PAE: Consider the following system: 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=153.04kJ (a) How will the amount of... Problem 12.93PAE: The decomposition of NH4HS , NH4HS(s)NH3(g)+H2S(g) is an endothermic process. Using Le principle,... Problem 12.94PAE: You are designing a process to remove carbonate ions from an aqueous system by precipitation. If the... Problem 12.95PAE: Equal amounts of two gases, A and B3, are placed in an evacuated container and react to form AB and... Problem 12.96PAE Problem 12.97PAE Problem 12.98PAE Problem 12.99PAE: Solid CaCO3 ; is placed in a closed container and heated to 800 °C. What is the equilibrium... Problem 12.100PAE: 12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial... Problem 12.101PAE: 12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to... Problem 12.102PAE: 12.102 A chemical engineer is working to optimize the production of acrylonitrile to be used in the... Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat.... Problem 12.104PAE Problem 12.105PAE: 12.105 Using the kinetic-molecular theory, explain why an increase in pressure produces more N2O4 in... Problem 12.106PAE: 12.106 The solubility of KCl is 34.7 g per 100 g of water at 20 °C. Calculate its molar solubility... Problem 12.107PAE Problem 12.108PAE: 12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant... Problem 12.109PAE: 12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar... Problem 12.110PAE: 12.110 In Exercise 12.109, what do you predict would happen to an aqueous copper(ll) iodate... Problem 12.111PAE: 12.111 You have three white solids. What experiment could you carry out to rank them in order of... Problem 12.112PAE Problem 12.113PAE Problem 12.114PAE Problem 12.115PAE Problem 12.116PAE Problem 12.117PAE: 12.117 The vapor pressure of water at 80.0 °C is 0.467 atm. Find the value of Kcfor the process... Problem 12.118PAE Problem 2CO: Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates...
Related questions
The chemical equilibrium , 2A(g) = B(g) + C(g) has a Kc of 0.0460. Calculate the equilibrium concentrations of all three species if the starting concentrations are as follow:
[A] = 0.450 M, [B] = 0.330 M, and [C] = 0.330 M
Definition Definition State where the components involved in a reversible reaction, namely reactants and product, do not change concentration any further with time. Chemical equilibrium results when the rate of the forward reaction becomes equal to the rate of the reverse reaction.
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