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 for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.34PAE: 1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was...
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