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The equilibrium constant, K. for the following reaction is 9.52x102 at 350 K. CH4 (g) - CC14 (g) =2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.299 moles of CH, and 0.299 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [ CH4 ] [CC4 ] [ CH,Cl, ] = [ M %3D %3D M M

The equilibrium constant, K. for the following reaction is 9.52x102 at 350 K. CH4 (g) - CC14 (g) =2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.299 moles of CH, and 0.299 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [ CH4 ] [CC4 ] [ CH,Cl, ] = [ M %3D %3D M M

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 9.52×102 at 350 K. CH4 (g) + CCl, (g) =2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.299 moles of CH4 and 0.299 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CC4 ] [ CH,Cl, ] = | M M M
Transcribed Image Text:The equilibrium constant, K. for the following reaction is 9.52×102 at 350 K. CH4 (g) + CCl, (g) =2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.299 moles of CH4 and 0.299 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CC4 ] [ CH,Cl, ] = | M M M
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