Suppose a 500. mL flask is filled with 0.10 mol of Cl₂, 0.90 mol of CHC13 and 0.30 mol of HC1. The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HC1(g) +CC1₂(g) The equilibrium constant K for this reaction is 9.98 at the temperature of the flask. Calculate the equilibrium molarity of C1₂. Round your answer to two decimal places. ☐M X
Suppose a 500. mL flask is filled with 0.10 mol of Cl₂, 0.90 mol of CHC13 and 0.30 mol of HC1. The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HC1(g) +CC1₂(g) The equilibrium constant K for this reaction is 9.98 at the temperature of the flask. Calculate the equilibrium molarity of C1₂. Round your answer to two decimal places. ☐M X
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 500. mL flask is filled with 0.10 mol of Cl₂, 0.90 mol of CHC13 and 0.30 mol of HC1. The following reaction becomes possible:
Cl₂(g) + CHC1₂(g) → HC1(g) +CC1₂(g)
The equilibrium constant K for this reaction is 9.98 at the temperature of the flask.
Calculate the equilibrium molarity of C1₂. Round your answer to two decimal places.
☐M
X](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F24823098-9e78-4458-9f4a-747264229ccb%2F6ccc8677-992c-4322-ab87-4a3f4b2cfff7%2F4u1bzrh_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 0.10 mol of Cl₂, 0.90 mol of CHC13 and 0.30 mol of HC1. The following reaction becomes possible:
Cl₂(g) + CHC1₂(g) → HC1(g) +CC1₂(g)
The equilibrium constant K for this reaction is 9.98 at the temperature of the flask.
Calculate the equilibrium molarity of C1₂. Round your answer to two decimal places.
☐M
X
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