A 1.00-L flask is filled with 1.00 moles of H2 and 2.00 moles of 2. The value of the equilibrium constant for the reaction of hydrogen and iodine reacting to form hydrogen iodide is 16.0 under the given conditions. What are the equilibrium concentrations of H2, 2, and HI? H2(g)+l2(g) =2HI(g) O IH2] = 0.155 M [12] = 1.155 M [H]] = 1.690 M O IH2] = 0.155 M [12] = 0.255 M [Hi] = 0.690 M O (H2) = 0.055 M [12] = 1.155 M [Hi] = 2.690 M O (H2] = 0.655 M [12] = 0.155 M [H]] = 1.690 M

A 1.00-L flask is filled with 1.00 moles of H2 and 2.00 moles of 2. The value of the equilibrium constant for the reaction of hydrogen and iodine reacting to form hydrogen iodide is 16.0 under the given conditions. What are the equilibrium concentrations of H2, 2, and HI? H2(g)+l2(g) =2HI(g) O IH2] = 0.155 M [12] = 1.155 M [H]] = 1.690 M O IH2] = 0.155 M [12] = 0.255 M [Hi] = 0.690 M O (H2) = 0.055 M [12] = 1.155 M [Hi] = 2.690 M O (H2] = 0.655 M [12] = 0.155 M [H]] = 1.690 M

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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