A student ran the following reaction in the laboratory at 543 K: CoCl₂(g) CO(g) + Cl₂(g) When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M. Calculate the equilibrium constant, K., she obtained for this reaction.
A student ran the following reaction in the laboratory at 543 K: CoCl₂(g) CO(g) + Cl₂(g) When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M. Calculate the equilibrium constant, K., she obtained for this reaction.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 41QRT: Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures.
2 NOCl(g) ⇌ 2 NO(g) +...
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![A student ran the following reaction in the laboratory at 543 K:
CoCl₂(g) CO(g) + Cl₂(g)
When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M.
Calculate the equilibrium constant, K, she obtained for this reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8e9aefa1-52f9-4bee-894a-5bceef7f78e2%2Ff48565b3-4611-4a14-bb17-b15a519b2ac5%2Fg6dn9pj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A student ran the following reaction in the laboratory at 543 K:
CoCl₂(g) CO(g) + Cl₂(g)
When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M.
Calculate the equilibrium constant, K, she obtained for this reaction.
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