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(11a) A student ran the following reaction in the laboratory at 641 K: CO(g) + Cl2(g)     COCl2(g) When she introduced 8.17×10-2 moles of CO(g) and 0.110 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 4.63×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = (b) The equilibrium constant, Kc, for the following reaction is 7.95×10-4 at 529 K. COCl2(g) CO(g) + Cl2(g) When a sufficiently large sample of COCl2(g) is introduced into an evacuated vessel at 529 K, the equilibrium concentration of Cl2(g) is found to be 0.238 M. Calculate the concentration of COCl2 in the equilibrium mixture.

(11a) A student ran the following reaction in the laboratory at 641 K: CO(g) + Cl2(g)     COCl2(g) When she introduced 8.17×10-2 moles of CO(g) and 0.110 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 4.63×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = (b) The equilibrium constant, Kc, for the following reaction is 7.95×10-4 at 529 K. COCl2(g) CO(g) + Cl2(g) When a sufficiently large sample of COCl2(g) is introduced into an evacuated vessel at 529 K, the equilibrium concentration of Cl2(g) is found to be 0.238 M. Calculate the concentration of COCl2 in the equilibrium mixture.

Chemistry
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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(11a) A student ran the following reaction in the laboratory at 641 K:

CO(g) + Cl2(g)     COCl2(g)

When she introduced 8.17×10-2 moles of CO(g) and 0.110 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 4.63×10-2 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Kc =

(b) The equilibrium constant, Kc, for the following reaction is 7.95×10-4 at 529 K.

COCl2(g) CO(g) + Cl2(g)

When a sufficiently large sample of COCl2(g) is introduced into an evacuated vessel at 529 K, the equilibrium concentration of Cl2(g) is found to be 0.238 M.

Calculate the concentration of COCl2 in the equilibrium mixture.

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