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The equilibrium constant, Ka, for the following reaction is 1.29x10-2 at 600 K. coCI2(g) co(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ

The equilibrium constant, Ka, for the following reaction is 1.29x10-2 at 600 K. coCI2(g) co(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
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The equilibrium constant, Kc, for the following reaction is 1.29x10-2 at 600 K. coCI,(g) ? CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI2(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ
Transcribed Image Text:The equilibrium constant, Kc, for the following reaction is 1.29x10-2 at 600 K. coCI,(g) ? CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI2(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ
Expert Solution
Step 1

The balanced equilibrium reaction given is 

COCl2 (g) ⇌ CO (g) + Cl2 (g) 

The equilibrium constant Kc for the reaction = 1.29×10–2 at 600 K

Volume of the vessel, V= 1.00 L

Number of moles of COCl2, n = 0.373 moles

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