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Suppose a 500. ml. flask is filled with 1.9 mol of H₂ and 0.80 mol of HCI. The following reaction becomes possible: H₂(g) +Cl₂(g) 2HCl(g) The equilibrium constant K for this reaction is 1.33 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. M

Suppose a 500. ml. flask is filled with 1.9 mol of H₂ and 0.80 mol of HCI. The following reaction becomes possible: H₂(g) +Cl₂(g) 2HCl(g) The equilibrium constant K for this reaction is 1.33 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. M

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Suppose a 500. mL flask is filled with 1.9 mol of H₂ and 0.80 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 1.33 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. 0 M
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.9 mol of H₂ and 0.80 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 1.33 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. 0 M
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