At equilibrium, a 1.00 L flask contains: 0.750 mol of PCl5, 0.500 mol of H2O, 7.50 mol of HCl, and 5.00 mol of POCl3. Calculate the equilibrium constant for this reaction: PCl5 (s) + H2O (g) ⇄ 2HCl (g) + POCl3 (g)
At equilibrium, a 1.00 L flask contains: 0.750 mol of PCl5, 0.500 mol of H2O, 7.50 mol of HCl, and 5.00 mol of POCl3. Calculate the equilibrium constant for this reaction: PCl5 (s) + H2O (g) ⇄ 2HCl (g) + POCl3 (g)
Chemistry
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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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At equilibrium, a 1.00 L flask contains: 0.750 mol of PCl5, 0.500 mol of H2O, 7.50 mol of HCl, and 5.00 mol of POCl3. Calculate the equilibrium constant for this reaction: PCl5 (s) + H2O (g) ⇄ 2HCl (g) + POCl3 (g)
Expert Solution
Step 1
The equilibrium constant expression for the above reaction will be given by
Kc = [HCl]2 X [POCl3] / [H2O]
where [H2O] = concentration of H2O
[POCl3] = concentration of POCl3
And [HCl] = concentration of HCl
Since the PCl5 is solid. And the concentration of solid (s) and liquid (l) components dont appear in the equilibrium constant
Hence PCl5 is not present in the equilibrium constant expression
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