General, Organic and Biochemistry - Laboratory Manualb. When SCN-ion is removed from the reaction mixture (by adding Ag ions, which form aninsoluble AgSCN(s) precipitate and thus reduce the amount of SCN-)? Explain why.c. When the temperature of the mixture is increased? Explain whyd. Would adding more Fe3 result in the color change to yellow or red? Explain why

(b)Le Châtelier’s principle states that when a system at equilibrium undergoes change in…

Answered: General, Organic and Biochemistry -…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 15CR

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The amino acid alanine has two isomers, -alanine and -alanine. When equal masses of these two compounds are dissolved in equal amounts of a solvent, the solution of -alanine freezes at the lowest temperature. Which form, -alanine or -alanine, has the larger equilibrium constant for ionization (HXH++X)?
. Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the inter-conversion reaction?
For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)
Which of the systems described in Exercise 13.15 give homogeneous equilibria? Which give heterogeneous equilibria?
5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of sulfur that comes from combustion of S-containing materials, to , which can combine with to make sulfuric acid (and thus contribute to acid rain): (a) Write the expression for K for this equilibrium. (b) Calculate the value of for this equilibrium using the values in Appendix 2. (c) Calculate the value of K for this equilibrium. (d) If of and of are enclosed in a system in the presence of some liquid, in which direction would the reaction move?
5.8. The hemoglobin in blood establishes an equilibrium with oxygen gas very quickly. The equilibrium can be represented as where “heme” stands for hemoglobin and “” stands for the hemoglobin-oxygen complex. The value for the equilibrium constant for this reaction is about . Carbon monoxide also binds with hemoglobin by the following reaction: This reaction has an equilibrium constant of . Which reaction’s equilibrium lies farther toward products? Does your answer justify the toxicity of ?
Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, and arsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equation CaCO3(s)Ca2+(aq)+CO32(aq). Is Kc1,1, or 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation 3Ba2+(aq)+2PO43(aq)Ba3( PO4)2(s). Is Kc1,1, or 1? Explain your answer.
12.85 In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. Describe what happens in the first few minutes after the partition is opened. WTiat would you expect to see several hours later? How is this system analogous to dynamic chemical equilibrium?
Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?
. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?
Why are there no changes specified for NH4HS in Exercise 13.62, part (e)? What property of NH4HS does change?
5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the reactants and products are all . If the volume of the system were doubled, all of the partial pressures would be . Would the system still be at equilibrium? Why or Why not?

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