(a)
Interpretation:
The equilibrium expression for the given reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,
The equilibrium constant for the above
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.43E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
The equilibrium constant for the given reaction is expressed as,
(b)
Interpretation:
The equilibrium expression for the given gaseous reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,
The equilibrium constant for the above chemical reaction is expressed as,
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.43E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
The equilibrium constant for the given reaction is expressed as,
(c)
Interpretation:
The equilibrium expression for the given gaseous reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,
The equilibrium constant for the above chemical reaction is expressed as,
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.43E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
The equilibrium constant for the given reaction is expressed as,
Want to see more full solutions like this?
Chapter 8 Solutions
Chemistry for Today: General, Organic, and Biochemistry
- Solid silver iodide, AgI, can be dissolved by adding aqueous sodium cyanide. Calculate Knet the following reaction. AgI(s)+2CN[Ag(CN)2](aq)+I(aq)arrow_forwardCalculate the Fe3+ equilibrium concentration when 0.0888 mole of K3[Fe(CN)6] is added to a solution with 0.0.00010 M CN-.arrow_forward. Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate Kspfor Cr(OH)3at this temperature.arrow_forward
- The Ksp for silver sulfate (Ag2SO4) is 1.2 105. Calculate the solubility of silver sulfate in each of the following. a. water b. 0.10 M AgNO3 c. 0.20 M K2SO4.arrow_forwardIn the presence of CN, Fe3+ forms the complex ion Fe(CN)63. The equilibrium concentrations of Fe3+ and Fe(CN)63 are 8.5 1040 M and 1.5 103 M, respectively, in a 0.11-M KCN solution. Calculate the value for the overall formation constant of Fe(CN)63. Fe3+(aq)+6CN(aq)Fe(CN)63(aq)Koverall=?arrow_forwardA solution is prepared by mixing 100.0 mL of 1.0 104 M Be(NO3)2 and 100.0 mL of 8.0 M NaF. Be2+(aq)+F(aq)BeF+(aq)K1=7.9104BeF+(aq)+F(aq)BeF2(aq)K2=5.8103BeF2(aq)+F(aq)BeF3(aq)K3=6.1102BeF3(aq)+F(aq)BeF42(aq)K4=2.7101 Calculate the equilibrium concentrations of F, Be2+, BeF+, BeF2, BeF3, and BeF42 in this solution.arrow_forward
- What is the solubility of silver oxide, Ag2O, in a solution buffered at pH 10.78? The equilibrium is Ag2O(s) + H2O(l) 2Ag+(aq) + 2OH (aq); Kc = 2.0 108.arrow_forwardPredict whether nickel(II) hydroxide, Ni(OH)2, will precipitate from a solution that is 0.0020 M NiSO4, 0.010 M NaOH, and 0.10 M NH3. Note that nickel(II) ion forms the Ni(NH3)62+ complex ion.arrow_forwardCrystals of AgBr can be removed from black-and-white photographic film by reacting the AgBr with sodium thiosulfate. AgBr(s)+2S2O32(aq)[Ag(S2O3)2]3(aq)+Br(aq) a What is the equilibrium constant for this dissolving process? b In order to dissolve 2.5 g of AgBr in 1.0 L of solution, how many moles of Na2S2O3 must be added?arrow_forward
- Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products). (a) TlCl. (b) BaF2. (c) Ag2CrO4. (d) CaC2O4H2O (e) the mineral anglesite, PbSO4arrow_forwardThe solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.arrow_forwardAssuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) Agl. (b) Ag2SO4. (c) Mn(OH)2. (d) Sr(OH)28H2O (e) the mineral brucite, Mg(OH)2arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning