O Kinetics and EquilibriumCalculating an equilibrium constant from a heterogeneous equilibrium...Iron(III) oxide and hydrogen react to form iron and water, like this:Fe2O3(s)+3 H2(g) 2 Fe(s)+3 H₂O(g)3/5BiAt a certain temperature, a chemist finds that a 3.3 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has thefollowing composition:compound amountFe2O34.10 gH₂2.97 gFe1.46 gH₂O2.53 gCalculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.K₁ = 0XG

Answered: O Kinetics and Equilibrium Calculating…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.60QE

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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 interconversion reaction?
Solid ammonium iodide decomposes to ammonia and hydrogen gases at sufficiently high temperatures. NH4I(s)NH3(g)+HI(g)The equilibrium constant for the decomposition at 400C is 0.215. Twenty grams of ammonium iodide are sealed in a 7.50-L flask and heated to 400C. (a) What is the total pressure in the flask at equilibrium? (b) How much solid NH4I is left after the decomposition?
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Antimony pentachloride decomposes according to this equation: SbCl5(g)SbCl3+Cl2(g) An equilibrium mixture in a 5.00-L flask at 443 C contains 3.85 g of SbCl5, 9.14 g of SbCl3, and 2.84 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?
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Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.

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