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A sealed 1 L flask containing Ag₂S(s) and H₂(g) is heated to 90 °C, and they react according to the following equation: Ag2S(s) + H₂(g) 2 Ag(s) + H₂S(g) At equilibrium, the following amounts are present: 0.048 mol Ag2S, 0.017 mol H₂. 0.114 mol Ag, and 0.540 mol H₂S. What is the value of K for this reaction, expressed in terms of the concentrations of these materials? O 8.6 074 O 0.032 O 32

A sealed 1 L flask containing Ag₂S(s) and H₂(g) is heated to 90 °C, and they react according to the following equation: Ag2S(s) + H₂(g) 2 Ag(s) + H₂S(g) At equilibrium, the following amounts are present: 0.048 mol Ag2S, 0.017 mol H₂. 0.114 mol Ag, and 0.540 mol H₂S. What is the value of K for this reaction, expressed in terms of the concentrations of these materials? O 8.6 074 O 0.032 O 32

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A sealed 1 L flask containing Ag2S(s) and H₂(g) is heated to 90 °C, and they react according to the following equation: Ag2S(s) + H₂(g) 2 Ag(s) + H₂S(g) At equilibrium, the following amounts are present: 0.048 mol Ag2S, 0.017 mol H₂. 0.114 mol Ag, and 0.540 mol H₂S. What is the value of K for this reaction, expressed in terms of the concentrations of these materials? O 8.6 074 O 0.032 32
Transcribed Image Text:A sealed 1 L flask containing Ag2S(s) and H₂(g) is heated to 90 °C, and they react according to the following equation: Ag2S(s) + H₂(g) 2 Ag(s) + H₂S(g) At equilibrium, the following amounts are present: 0.048 mol Ag2S, 0.017 mol H₂. 0.114 mol Ag, and 0.540 mol H₂S. What is the value of K for this reaction, expressed in terms of the concentrations of these materials? O 8.6 074 O 0.032 32
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