When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303K, 56% of the SO2Cl2 decomposes to SO2 and Cl2 :SO2Cl2(g) ⇌ SO2(g) + Cl2(g)(a) Calculate Kc for this reaction at this temperature.(b) Calculate Kp for this reaction at 303 K. (c) Accordingto Le Châtelier’s principle, would the percent of SO2Cl2that decomposes increase, decrease or stay the same if themixture were transferred to a 15.00-L vessel? (d) Use theequilibrium constant you calculated above to determinethe percentage of SO2Cl2 that decomposes when 2.00mol of SO2Cl2 is placed in a 15.00-L vessel at 303 K.
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303K, 56% of the SO2Cl2 decomposes to SO2 and Cl2 :SO2Cl2(g) ⇌ SO2(g) + Cl2(g)(a) Calculate Kc for this reaction at this temperature.(b) Calculate Kp for this reaction at 303 K. (c) Accordingto Le Châtelier’s principle, would the percent of SO2Cl2that decomposes increase, decrease or stay the same if themixture were transferred to a 15.00-L vessel? (d) Use theequilibrium constant you calculated above to determinethe percentage of SO2Cl2 that decomposes when 2.00mol of SO2Cl2 is placed in a 15.00-L vessel at 303 K.
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 89AP
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Question
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303
K, 56% of the SO2Cl2 decomposes to SO2 and Cl2 :
SO2Cl2(g) ⇌ SO2(g) + Cl2(g)
(a) Calculate Kc for this reaction at this temperature.
(b) Calculate Kp for this reaction at 303 K. (c) According
to Le Châtelier’s principle, would the percent of SO2Cl2
that decomposes increase, decrease or stay the same if the
mixture were transferred to a 15.00-L vessel? (d) Use the
equilibrium constant you calculated above to determine
the percentage of SO2Cl2 that decomposes when 2.00
mol of SO2Cl2 is placed in a 15.00-L vessel at 303 K.
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