A student ran the following reaction in the laboratory at 540 K:COC1₂ (g) CO(g) + Cl₂(g)When she introduced 1.28 moles of COC1₂ (g) into a 1.00 liter container, she found the equilibrium concentration ofCOCl₂ (g) to be 1.24 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.Ke=

Reaction COCl2(g) -------->CO(g) + Cl2(g)

A student ran the following reaction in the laboratory at 540 K: COC12 (g) CO(g) + Cl₂ (g) When she introduced 1.28 moles of COC12 (g) into a 1.00 liter container, she found the equilibrium concentration of COC1₂ (g) to be 1.24 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Ke =

A student ran the following reaction in the laboratory at 540 K: COC12 (g) CO(g) + Cl₂ (g) When she introduced 1.28 moles of COC12 (g) into a 1.00 liter container, she found the equilibrium concentration of COC1₂ (g) to be 1.24 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Ke =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 60QRT

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Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
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