Do not answer in image format Suppose a 250. mL. flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible:Cl₂(g) + CHC1₂(g) → HCl(g) +CCl4 (g)The equilibrium constant K for this reaction is 3.83 at the temperature of the flask.Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places.MS

Equilibrium constant K for the reaction = 3.83Volume of the flask = 250mL = (250/1000)L = 0.25…

Suppose a 250. mL flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) HCI(g) +CC14(g) The equilibrium constant K for this reaction is 3.83 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M

Suppose a 250. mL flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) HCI(g) +CC14(g) The equilibrium constant K for this reaction is 3.83 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M

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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