Suppose a 250. mL flask is filled with 1.2 mol of CHCI,, 0.10 mol of HCl and 1.7 mol of CCl. The following reaction becomes possible: Cl, (g) + CHCI, (g) - HCI(g) +CCl,(g) The equilibrium constant K for this reaction is 5.74 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 1.2 mol of CHCI,, 0.10 mol of HCl and 1.7 mol of CCl. The following reaction becomes possible: Cl, (g) + CHCI, (g) - HCI(g) +CCl,(g) The equilibrium constant K for this reaction is 5.74 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 17A

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