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Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 1164 K: 2SO2(g) + O2(g) = 2SO3 (9) When she introduced 0.0862 moles of SO2 (g) and 0.0786 moles of O2 (g) into a 1.00 liter container, she found the equilibrium concentration of O2 (g) to be 0.0549 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 1164 K: 2SO2(g) + O2(g) = 2SO3 (9) When she introduced 0.0862 moles of SO2 (g) and 0.0786 moles of O2 (g) into a 1.00 liter container, she found the equilibrium concentration of O2 (g) to be 0.0549 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 1164 K: 2SO2(g) + O2(g) = 2SO3 (9) When she introduced 0.0862 moles of SO2 (g) and 0.0786 moles of O2 (g) into a 1.00 liter container, she found the equilibrium concentration of O2 (g) to be 0.0549 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Transcribed Image Text:Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 1164 K: 2SO2(g) + O2(g) = 2SO3 (9) When she introduced 0.0862 moles of SO2 (g) and 0.0786 moles of O2 (g) into a 1.00 liter container, she found the equilibrium concentration of O2 (g) to be 0.0549 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
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