A student ran the following reaction in the laboratory at 547 K: COCl2 = CO+ Cl2 When she introduced 0.878 moles of COCl2 into a 1.00 liter container, she found the equilibrium concentration of COCl2 to be 0.840 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 547 K: COCl2 = CO+ Cl2 When she introduced 0.878 moles of COCl2 into a 1.00 liter container, she found the equilibrium concentration of COCl2 to be 0.840 M. Calculate the equilibrium constant, Kc, 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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Question
A student ran the following reaction in the laboratory at 547 K:
COCl2 = CO+ Cl2
When she introduced 0.878 moles of COCl2 into a 1.00 liter container, she found the equilibrium concentration of COCl2 to be 0.840 M.
Calculate the equilibrium constant, Kc, she obtained for this reaction.
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