Initially, 1.50 M of ammonia (NH3) were placed in an empty container without any other gases at789K. It started to decompose according to the chemical equation below:2 NH3(g) = N₂(g) + 3 H₂(g)After equilibrium was established, it was found that there are 0.055 M of ammonia left in thesame vessel. What is the equilibrium constant, Kc, for this reaction at 789 K?3.5289.8 x 1032.4 x 10³O4.8 x 104

Initially, 1.50 M of ammonia (NH3) were placed in an empty container without any other gases at 789K. It started to decompose according to the chemical equation below: 2 NH3(g) N2(g) + 3 H₂(g) After equilibrium was established, it was found that there are 0.055 M of ammonia left in the same vessel. What is the equilibrium constant, Kc, for this reaction at 789 K? 3.5 28 9.8 x 103 2.4 × 10³ 4.8 x 104

Initially, 1.50 M of ammonia (NH3) were placed in an empty container without any other gases at 789K. It started to decompose according to the chemical equation below: 2 NH3(g) N2(g) + 3 H₂(g) After equilibrium was established, it was found that there are 0.055 M of ammonia left in the same vessel. What is the equilibrium constant, Kc, for this reaction at 789 K? 3.5 28 9.8 x 103 2.4 × 10³ 4.8 x 104

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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