Chemistry by OpenStax (2015-05-04) 1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
1 Essential Ideas 2 Atoms, Molecules, And Ions 3 Composition Of Substances And Solutions 4 Stoichiometry Of Chemical Reactions 5 Thermochemistry 6 Electronic Structure And Periodic Properties Of Elements 7 Chemical Bonding And Molecular Geometry 8 Advanced Theories Of Covalent Bonding 9 Gases 10 Liquids And Solids 11 Solutions And Colloids 12 Kinetics 13 Fundamental Equilibrium Concepts 14 Acid-base Equilibria 15 Equilibria Of Other Reaction Classes 16 Thermodynamics 17 Electrochemistry 18 Representative Metals, Metalloids, And Nonmetals 19 Transition Metals And Coordination Chemistry 20 Organic Chemistry 21 Nuclear Chemistry Chapter13: Fundamental Equilibrium Concepts
Chapter Questions Section: Chapter Questions
Problem 1E: What does it mean to describe a reaction as reversible? Problem 2E: When writing an equation, how is a reversible reaction distinguished from a nonreversible reaction? Problem 3E: If a reaction is reversible, when can it be said to have reached equilibrium? Problem 4E: Is a system at equilibrium if the rate constants of the forward and reverse reactions are equal? Problem 5E: If the concentrations of products and reactants are equal, is the system at equilibrium? Problem 6E: Explain why there may be an infinite number of values for the reaction quotient of a reaction at a... Problem 7E: Explain why an equilibrium between Br2(l) and Br2(g) would not be established if the container were... Problem 8E: If you observe the following reaction at equilibrium, is it possible to tell whether the reaction... Problem 9E: Among the solubility rules previously discussed is the statement: All chlorides are soluble except... Problem 10E: Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates,... Problem 11E: Benzene is one of the compounds used as octane enhancers in unleaded gasoline. It is manufactured by... Problem 12E: Show that the complete chemical equation, the total ionic equation, and the net ionic equation for... Problem 13E: For a titration to be effective, the reaction must be rapid and the yield of the reaction must... Problem 14E: For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction... Problem 15E: Write the mathematical expression for the reaction quotient, QC, for each of the following... Problem 16E: Write the mathematical expression for the reaction quotient, QC, for each of the following reactions... Problem 17E: The initial concentrations or pressures of reactants and products are given for each of the... Problem 18E: The initial concentrations or pressures of reactants and products are given for each of the... Problem 19E: The following reaction has KP=4.50105 at 720 K. N2(g)+3H2(g)2NH3 If a reaction vessel is filled with... Problem 20E: Determine if the following system is at equilibrium. If not, in which direction will the system need... Problem 21E: Which of the systems described in Exercise 13.15 give homogeneous equilibria? Which give... Problem 22E: Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give... Problem 23E: For which of the reactions in Exercise 13.15 does Kc (calculated using concentrations) equal KP... Problem 24E: For which of the reactions in Exercise 13.16 does Kc (calculated using concentrations) equal Kp... Problem 25E: Convert the values of KC to values of KP to the values of KP to values of Kc. (a)... Problem 26E: Covert the values of Kc to the values of KP or the values of Kp to values of Kc. (a)... Problem 27E: What is the value of the equilibrium constant expression for the change H2O(l)H2O(g) at 30 C? Problem 28E: Write the expression of the reaction quotient for the ionization of HOCN in water. Problem 29E: Write the reaction quotient expression for the ionization of NH3 in water. Problem 30E: What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5(l)C2H5OC2H5(g)... Problem 31E: The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what... Problem 32E: Explain how to recognize the conditions under which changes in pressure would affect systems at... Problem 33E: What property of a reaction can we use to predict the effect of a change in temperature on the value... Problem 34E: What would happen to the color of the solution in part (b) of Figure 13.8 if a small amount of NaOH... Problem 35E: The following reaction occurs when a burner on a gas stove is lit: CH4+2O2(g)CO2(g)+2H2O(g) Is an... Problem 36E: A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from... Problem 37E: Suggest four ways in which the concentration of hydrazine, N2H4, could be increased in an... Problem 38E: Suggest four ways in which the concentration of PH3could be increased in an equilibrium described by... Problem 39E: How will an increase in temperature affect each of the following equilibria? How will a decrease in... Problem 40E: How will an increase in temperature affect each of the following equilibria? How will a decrease in... Problem 41E: Water gas is a 1:1 mixture of carbon monoxide and hydrogen gas and is called water gas because it is... Problem 42E: Nitrogen and oxygen react at high temperatures. (a) Write the expression for the equilibrium... Problem 43E: Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam... Problem 44E: Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas. (a) Write the... Problem 45E: Ammonia is a weak base that reacts with water according to this equation:... Problem 46E: Acetic acid is a weak acid that reacts with water according to this equation:... Problem 47E: Suggest two ways in which the equilibrium concentration of Ag+ can be reduced in a solution of Na+,... Problem 48E: How can the pressure of water vapor be increased in the following equilibrium? H2O(l)H2O(g)H=41kJ Problem 49E: Additional solid silver sulfate, a slightly soluble solid, is added to a solution of silver ion and... Problem 50E: The amino acid alanine has two isomers, -alanine and -alanine. When equal masses of these two... Problem 51E: A reaction is represented by this equation: A(aq)+2B2C(aq) Kc=1103 (a) Write the mathematical... Problem 52E: A reaction is represented by this equation: 2W(aq)X(aq)+2Y(aq)Kc=5104 (a) Write the mathematical... Problem 53E: What is the value of the equilibrium constant at 500 C for the formation of NH3 according to the... Problem 54E: Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated... Problem 55E: A 0.72-m01 sample of PCl5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel... Problem 56E: At 1 atm and 25 C, NO2 with an initial concentration of 1.00 M is 3.3103 decomposed into NO and O2.... Problem 57E: Calculate the value of the equilibrium constant Kp for the reaction 2NO2(g)+Cl2(g)2NOCl(g) from... Problem 58E: When heated, iodine vapor dissociates according to this equation: I2(g)2I(g) At 1274 K, a sample... Problem 59E: A sample of ammonium chloride was heated in a closed container. NH4CI(s)NH3(g)+HCI(g) At... Problem 60E: At a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the... Problem 61E: Complete the changes in concentrations (or pressure, if requested) for each of the following... Problem 62E: Complete the changes in concentrations (or pressure, if requested) for each of the following... Problem 63E: Why are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does... Problem 64E: Why are there no changes specified for NH4HS in Exercise 13.62, part (e)? What property of NH4HS... Problem 65E: Analysis of the gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400 C... Problem 66E: Calculate the number of moles of HI that are at equilibrium with 1.25 mol of H2 and 1.25 mol of I2... Problem 67E: What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2... Problem 68E: What is the pressure of CO2 in a mixture at equilibrium that contains 0.50 mm H2, 2.0 atm of H2O,... Problem 69E: Cobalt metal can be prepared by reducing cobalt (II) oxide with carbon monoxide.... Problem 70E: Carbon reacts with water vapor at elevated temperatures. C(s)+H2O(g)Co(g)+H2(g)Kc=0.2 at 1000 C What... Problem 71E: Sodium sulfate 10-hydrate, Na2SO410H2O, dehydrates according to the equation... Problem 72E: Calcium Chloride 6-hydrate, CaCl26H2O, dehydrates according to the equation... Problem 73E: A student solved the following problem and found the equilibrium concentrations to be... Problem 74E: A student solved the following problem and found [N2O4]=0.16M at equilibrium. How could this student... Problem 75E: Assume that the change in concentration of N2O4 is small enough to be neglected in the following... Problem 76E: Assume that the change in concentration of COCI2 is small enough to be neglected in the following... Problem 77E: Assume that the change in pressure of H2S is small enough to be neglected in the following problem,... Problem 78E: What are all concentrations after a mixture that contains [H2O]=1.00M and [Cl2O]=1.00M comes to... Problem 79E: What are the concentrations of PCl5, PCl3, and Cl2 in an equilibrium mixture produced by the... Problem 80E: Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced... Problem 81E: Calculate the equilibrium concentrations of NO, O2, and NO2 in a mixture at 250 C that results from... Problem 82E: Calculate the equilibrium concentrations that result when 0.25 M O2 and 1.0 M HCl react and come to... Problem 83E: One of the important reactions in the formation of smog is represented by the equation... Problem 84E: Calculate the pressures of NO, Cl2, and NOCI in an equilibrium mixture produced by the reaction of a... Problem 85E: Calculate the number of grams of HI that are at equilibrium with 1.25 mol of H2 and 63.5 g of iodine... Problem 86E: Butane exists as two isomers, n -butane and isobutane. Kp=2.5 at 25 C What is the pressure of... Problem 87E: What is the minimum mass of CaCO3 required to establish equilibrium at a certain temperature in a... Problem 88E: The equilibrium constant (Kc) for this reaction is 1.60 at 990 c: H2(g)+CO2(g)H2O(g)+CO(g) Calculate... Problem 89E: At 25 C and at 1 atm, the partial pressures in an equilibrium mixture of N2O4 and NO2 are PN2O4=0.70... Problem 90E: In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317... Problem 91E: The equilibrium constant (Kc) for this reaction is 5.0 at a given temperature.... Problem 92E: Antimony pentachloride decomposes according to this equation: SbCl5(g)SbCl3+Cl2(g) An equilibrium... Problem 93E: Consider the reaction between H2 and O2 at 1000 2H2(g)+O22H2O(g)Kp=( P H 2 O )2(P o2 )( P H 2... Problem 94E: An equilibrium is established according to the following equation... Problem 95E: Consider the equilibrium 4NO2(g)+6H2O(g)4NH3(g)+7O2(g) (a) What is the expression for the... Problem 96E: The binding of oxygen by hemoglobin (Hb), giving oxy-hemoglobin (HbO2), is partially regulated by... Problem 97E: The hydrolysis of the sugar sucrose to the sugars glucose and fructose follows a first-order rate... Problem 98E: The density of trifluoroacetic acid vapor was determined at 118.1 C and 468.5 torr, and found to be... Problem 99E: Liquid N2o3 is dark blue at low temperatures, but the color fades and becomes greenish at higher... Problem 100E: A 1.00-L vessel at 400 C contains the following equilibrium concentrations: N2, 1.00 M; H2, 0.50 M;... Problem 101E: A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and... Problem 12E: Show that the complete chemical equation, the total ionic equation, and the net ionic equation for...
Related questions
The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K.
A sample of gas in which [H2 S] = 3.45 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2 S]? Assume no H2 or S2 was present in the original sample.
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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