Suppose a 500 ml. flask is filled with 1.3 mol of Cl₂, 0.70 mol of CHCI, and 0.80 mol of HCI. The following reaction becomes possible: CL₂(g) +CHCI, (e)-HC1 (g) +CCI, (g) The equilibrium constant K for this reaction is 1.55 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places. OM X Ś

Suppose a 500 ml. flask is filled with 1.3 mol of Cl₂, 0.70 mol of CHCI, and 0.80 mol of HCI. The following reaction becomes possible: CL₂(g) +CHCI, (e)-HC1 (g) +CCI, (g) The equilibrium constant K for this reaction is 1.55 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places. OM X Ś

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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Answer with two decimal places, please!
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