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
General Chemistry - Standalone book (MindTap Course List)
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Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.19QP: During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction...
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![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.
M
S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe572a379-918d-4607-9ea3-d5ea5ddef594%2F58862926-748f-49f8-bb8c-1fa670e1508b%2F9vyuguf_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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.
M
S
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