Suppose a 500. mL flask is filled with 0.90 mol of Cl,, 1.1 mol of HCl and 0.20 mol of CCl. The following reaction becomes possible:4'Cl,(g) + CHCI, (g) –HCl (g)+CCI,(g)The equilibrium constant K for this reaction is 0.723 at the temperature of the flask.Calculate the equilibrium molarity of CHCI3. Round your answer to two decimal places.M

Given, Volume = 500 mL = 0.500 L Moles of Cl2 = 0.90 mol Moles of HCl = 1.1 mol Moles of CCl4 =…

Suppose a 500. mL flask is filled with 0.90 mol of Cl,, 1.1 mol of HCl and 0.20 mol of CCl.. The following reaction becomes possible: Cl,(g) + CHCI, (g) -HCI (g)+ CC14(g) The equilibrium constant K for this reaction is 0.723 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 0.90 mol of Cl,, 1.1 mol of HCl and 0.20 mol of CCl.. The following reaction becomes possible: Cl,(g) + CHCI, (g) -HCI (g)+ CC14(g) The equilibrium constant K for this reaction is 0.723 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places. ?

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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