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Suppose a 250. mL flask is filled with 1.5 mol of Cl₂, 0.20 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) → HCl(g) +CCl₂(g) The equilibrium constant K for this reaction is 0.973 at the temperature of the flask. Calculate the equilibrium molarity of CHCl3. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 1.5 mol of Cl₂, 0.20 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) → HCl(g) +CCl₂(g) The equilibrium constant K for this reaction is 0.973 at the temperature of the flask. Calculate the equilibrium molarity of CHCl3. Round your answer to two decimal places.

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
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Suppose a 250. mL flask is filled with 1.5 mol of Cl₂, 0.20 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) → HCl(g) +CCl4 (g) The equilibrium constant K for this reaction is 0.973 at the temperature of the flask. Calculate the equilibrium molarity of CHC13. Round your answer to two decimal places. M X
Transcribed Image Text:Suppose a 250. mL flask is filled with 1.5 mol of Cl₂, 0.20 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) → HCl(g) +CCl4 (g) The equilibrium constant K for this reaction is 0.973 at the temperature of the flask. Calculate the equilibrium molarity of CHC13. Round your answer to two decimal places. M X
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