A student ran the following reaction in the laboratory at 579 K: CO(g) + Cl2(g)=COCl,(g) When she introduced 0.465 moles of CO(g) and 0.494 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 6.76×10² M. Calculate the equilibrium constant, K, she obtained for this reaction. K.
A student ran the following reaction in the laboratory at 579 K: CO(g) + Cl2(g)=COCl,(g) When she introduced 0.465 moles of CO(g) and 0.494 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 6.76×10² M. Calculate the equilibrium constant, K, she obtained for this reaction. K.
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 579 K:
CO(g) + Cl2(g) cOC»(g)
When she introduced 0.465 moles of CO(g) and 0.494 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of
Cl,(g) to be 6.76×102 M.
Calculate the equilibrium constant, K, she obtained for this reaction.
K.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3d2b0534-65d7-4c4f-8595-adc051f2d27b%2F55bba04a-7426-487d-85dc-5a37e30c2e28%2Fg7ar3i4_processed.png&w=3840&q=75)
Transcribed Image Text:A student ran the following reaction in the laboratory at 579 K:
CO(g) + Cl2(g) cOC»(g)
When she introduced 0.465 moles of CO(g) and 0.494 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of
Cl,(g) to be 6.76×102 M.
Calculate the equilibrium constant, K, she obtained for this reaction.
K.
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