An equilibrium mixture of PCI, (g), PCI, (g), and Cl,(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr,respectively. A quantity of Cl, (g) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment ofmixing. The system then re-equilibrates.The chemical equation for this reaction isPCI, (g) + Cl, (g) = PCI, (g)Calculate the new partial pressures, P, after equilibrium is reestablished.TorrPPCI,%3DTorrPch%3DTorrPoC%3DQuestion Source: MRG - General Chemistry Publisher: Universprivacy policyterms of, usecontact ushelpabout uscareers4/2

The given balanced chemical reaction at equilibrium is The Kp expression and Kp value for above…

Answered: An equilibrium mixture of PCI, (g),…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 33P

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. 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?
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 30 s? After 90 s?
. For a given reaction at a given temperature, the special ratio of products to reactants defined by the equilibrium constant is always equal to the same number. Explain why this is true, no matter what initial concentrations of reactants (or products) may have been taken in setting up an experiment.
Chemical Equilibrium II Magnesium hydroxide. Mg(OH)2, is a white, partially soluble solid that is used in many antacids. The chemical equation for the dissolving of Mg(OH)2(s) in water is Mg(OH)2(s)Mg2+(aq)+2OH(aq) a Describe a simple experimental procedure that you could use to study this solubility equilibrium. In your experiment, how would you determine when the solution process has attained equilibrium? b Write the equilibrium-constant expression for this dissolving of magnesium hydroxide. c Suppose equilibrium has been established in a container of magnesium hydroxide in water, and you decide to add more solid Mg(OH)2. What would you expect to observe? What effect will this addition of Mg(OH)2 have on the concentrations of Mg2+(aq) and OH(aq)? d Say you haw prepared an equilibrium solution of Mg(OH)2 by adding pure solid Mg(OH)2 to water. If you know the concentration of OH(aq), can you determine the concentration of Mg2+(aq)? If not, what information do you need that will allow you to determine the answer? e You slowly add OH from another source (say, NaOH) to an equilibrium mixture of Mg(OH)2 and water. How do you expect the concentration of the Mg2+(aq) to change? What might you be able to observe happening to the Mg(OH)2(s) as you add the OH? f Next you remove some, but not all, of the Mg(OH)2(s) from the mixture. How will this affect the concentrations of the Mg2+(aq) and OH(aq)? g If someone hands you a container of Mg(OH)2(aq) and there is no solid Mg(OH)2 present, is this solution at equilibrium? If it is not at equilibrium, what could you add to or remove from the container that would give an equilibrium system? h Consider an individual OH(aq) ion in an Mg(OH)2 solution at equilibrium. If you could follow this ion over a long period of time, would you expect it always to remain as an OH(aq) ion, or could it change in some way?
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?
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)

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