For the reaction at equibrium. 3Feis) + 4H2Oul - Fez04ls) + 4H2(a), removing some of the product. FezOgls). would Multple Choice Couse no change Decreese the velue of the equibrium constent, K Increase the value of the equilbnum constant, K Shit the equibrum to the let Shih the equibrium to the right

For the reaction at equibrium. 3Feis) + 4H2Oul - Fez04ls) + 4H2(a), removing some of the product. FezOgls). would Multple Choice Couse no change Decreese the velue of the equibrium constent, K Increase the value of the equilbnum constant, K Shit the equibrum to the let Shih the equibrium to the right

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.5: Using Equilibrium Constants

Problem 12.6PSP

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A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
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)
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
. At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g)+O2(g)2NO(g)Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [N2]=0.041M. [O2]=0.0078M, and [NO]=4.710M. Calculate the value of K for the reaction.
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?
Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s)NH3(g)+H2S(g) In a sealed flask at 25C are 10.0 g of NH4HS, ammonia with a partial pressure of 0.692 atm, and H2S with a partial pressure of 0.0532 atm. When equilibrium is established, it is found that the partial pressure of ammonia has increased by 12.4%. Calculate K for the decomposition of NH4HS at 25C.
. For the reaction 2H2O(g)2H2(g)+O2(g)K=2.4103at a given temperature. At equilibrium ills found that [H2O(g)]=1.1101Mand [H2(g)]=1.9102M. What is the concentration of O2(g) under these conditions?
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In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q were expressed in units of pressure. We also can use units of mol/L for the quantities in Q, specifical.ly for aqueous reactions. With this in mind, consider the reaction HF(aq)H+(aq)+F-(aq) for which Ka = 7.2 104 at 25C. Calculate G for the reaction under the following conditions at 25C. a. [HF] = [H+] = [F] = 1.0 M b. [HF] = 0.98 M, [H+] = [F] = 2.7 102M c. [HF] = [H+] = [F] = 1.0 105 M d. [HF] = [F] = 0.27 M, [H+] = 7.2 104M e. [HF] = 0.52 M, [F] = 0.67 M, [H+] = 1.0 103M Based on the calculated G values, in what direction will the reaction shift to reach equilibrium for each of the five sets of conditions?