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The equilibrium constant, K., for the following reaction is 10.5 at 350 K. 2CH,Cl½(g)CH4(g) + CC14(g) Calculate the equilibrium concentrations of reactant and products when 0.283 moles of CH,Cl, are introduced into a 1.00 L vessel at 350 K. [CH,Cl2] = M [CH4] M %3D [CCL] M %3D

The equilibrium constant, K., for the following reaction is 10.5 at 350 K. 2CH,Cl½(g)CH4(g) + CC14(g) Calculate the equilibrium concentrations of reactant and products when 0.283 moles of CH,Cl, are introduced into a 1.00 L vessel at 350 K. [CH,Cl2] = M [CH4] M %3D [CCL] M %3D

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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The equilibrium constant, K., for the following reaction is 10.5 at 350 K. 2CH,Cl,(g)CHĄ(g) + CC14(g) Calculate the equilibrium concentrations of reactant and products when 0.283 moles of CH,Cl, are introduced into a 1.00 L vessel at 350 K. [CH,Cl,] = M [CH4] M [CC1] M
Transcribed Image Text:The equilibrium constant, K., for the following reaction is 10.5 at 350 K. 2CH,Cl,(g)CHĄ(g) + CC14(g) Calculate the equilibrium concentrations of reactant and products when 0.283 moles of CH,Cl, are introduced into a 1.00 L vessel at 350 K. [CH,Cl,] = M [CH4] M [CC1] M
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