+O2 (8) 2 SO, (8) A,2.000 Lflask was initially filled with,0.0400 mol SO and 0.0200 mol O, and was allowed to reach equilibrium. If the flask contained, 0.0296 mol SO, at equilibrium: Consider the following: 2 SO, (e) 2 (g) 32 3. al Calculate the moles of each substance present at equilibrium. b| Calculate the equilibrium constant, K. + O2 (3) = 2SO, (8) 3 (g) c Calculate the equilibrium constant, K, for the following: 2 SO, +2O2(8) = 4 SO, (3) 2 (g) d| Calculate the equilibrium constant, K, for the following: 4 SO, (e) of HCN CHEMISTRY 1516L

+O2 (8) 2 SO, (8) A,2.000 Lflask was initially filled with,0.0400 mol SO and 0.0200 mol O, and was allowed to reach equilibrium. If the flask contained, 0.0296 mol SO, at equilibrium: Consider the following: 2 SO, (e) 2 (g) 32 3. al Calculate the moles of each substance present at equilibrium. b| Calculate the equilibrium constant, K. + O2 (3) = 2SO, (8) 3 (g) c Calculate the equilibrium constant, K, for the following: 2 SO, +2O2(8) = 4 SO, (3) 2 (g) d| Calculate the equilibrium constant, K, for the following: 4 SO, (e) of HCN CHEMISTRY 1516L

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 30P

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Similar questions

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Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced. Sb2S3(s)+3H2(g)2Sb(s)+3H2S(g) A vessel whose volume was 2.50 L was filled with 0.0100 mol of antimony(III) sulfide, Sb2S3, and 0.0100 mol H2. After the mixture came to equilibrium in the closed vessel at 440C, the gaseous mixture was removed, and the hydrogen sulfide was dissolved in water. Sufficient lead(II) ion was added to react completely with the H2S to precipitate lead(II) sulfide, PbS. If 1.029 g PbS was obtained, what is the value of Kc at 440C?
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