The equilibrium constant, Ke, for the following reaction is 1.29x102 at 600 K. COCI2(g) CO(g) + C2(g) Calculate the equilibrium concentrations of reactant and products when 0.313 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COCH) - M [CO) %3D [Cl2] M

The equilibrium constant, Ke, for the following reaction is 1.29x102 at 600 K. COCI2(g) CO(g) + C2(g) Calculate the equilibrium concentrations of reactant and products when 0.313 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COCH) - M [CO) %3D [Cl2] M

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...

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Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
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