When the reaction below is at equilibrium there are 0.250 mol of Br2, 1.25 mol of Cl2, and 1.5 mol of BrCl in a closed flask of 1.00 L at 100 degrees C. A Chem 109 student upsets the equilibrium by adding 0.0500 mol of Br2 into the 1L sealed flask. The equilibrium constant for the reaction is Kc = 7.20 at 100 degrees C. Calculate the concentration of Br2, Cl2 and BrCl when the new equilibrium is established. Br2 (g) + Cl2 (g) <---> 2 BrCl (g) Kc = 7.20 at 100 degrees C
When the reaction below is at equilibrium there are 0.250 mol of Br2, 1.25 mol of Cl2, and 1.5 mol of BrCl in a closed flask of 1.00 L at 100 degrees C. A Chem 109 student upsets the equilibrium by adding 0.0500 mol of Br2 into the 1L sealed flask. The equilibrium constant for the reaction is Kc = 7.20 at 100 degrees C. Calculate the concentration of Br2, Cl2 and BrCl when the new equilibrium is established. Br2 (g) + Cl2 (g) <---> 2 BrCl (g) Kc = 7.20 at 100 degrees C
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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When the reaction below is at equilibrium there are 0.250 mol of Br2, 1.25 mol of Cl2, and 1.5 mol of BrCl in a closed flask of 1.00 L at 100 degrees C. A Chem 109 student upsets the equilibrium by adding 0.0500 mol of Br2 into the 1L sealed flask. The equilibrium constant for the reaction is Kc = 7.20 at 100 degrees C. Calculate the concentration of Br2, Cl2 and BrCl when the new equilibrium is established.
Br2 (g) + Cl2 (g) <---> 2 BrCl (g) Kc = 7.20 at 100 degrees C
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