Suppose a 500. mL flask is filled with 1.8 mol of Cl,, 1.6 mol of CHCI, and 1.7 mol of HCl. The following reaction becomes possible:Cl,(g) +CHCI, (g) HCl(g)+CCl,(g)The equilibrium constant K for this reaction is 0.642 at the temperature of the flask.Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places.

The given reaction is as follows. Cl2g+CHCl3g⇔HClg+CCl4g Equilibrium constant will remain constant…

Suppose a 500. mL flask is filled with 1.8 mol of Cl,, 1.6 mol of CHCI, and 1.7 mol of HCI. The following reaction becomes possible: Cl,(2) +CHCI; (g) – HC1(g) + CCI, (g) The equilibrium constant K for this reaction is 0.642 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places.

Suppose a 500. mL flask is filled with 1.8 mol of Cl,, 1.6 mol of CHCI, and 1.7 mol of HCI. The following reaction becomes possible: Cl,(2) +CHCI; (g) – HC1(g) + CCI, (g) The equilibrium constant K for this reaction is 0.642 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. 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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