The equilibrium constant, K., for the following reaction is 9.52×10-² at 350 K. CH4 (g) + CC14 (g) =2 CH2C12 (g) Calculate the equilibrium concentrations of reactants and product when 0.277 moles of CH4 and 0.277 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CC4] [ CH,Cl, ] = M %3D M %3D M
The equilibrium constant, K., for the following reaction is 9.52×10-² at 350 K. CH4 (g) + CC14 (g) =2 CH2C12 (g) Calculate the equilibrium concentrations of reactants and product when 0.277 moles of CH4 and 0.277 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CC4] [ CH,Cl, ] = M %3D M %3D M
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 9.52×10-2 at 350 K.
CH4 (g) + CC14 (g) =2 CH2Cl2 (g)
Calculate the equilibrium concentrations of reactants and product when 0.277 moles of CH, and 0.277 moles of CCl, are introduced into a 1.00 L vessel at 350 K.
[ CH4]
M
[CC4]
M
[ CH2C1, ] =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fee20ab8b-1fae-485e-ac9c-9e887dc6dd7a%2Fa7b94a9c-381d-4a22-bcb0-3f142339615f%2Fwuwdcje_processed.png&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, K., for the following reaction is 9.52×10-2 at 350 K.
CH4 (g) + CC14 (g) =2 CH2Cl2 (g)
Calculate the equilibrium concentrations of reactants and product when 0.277 moles of CH, and 0.277 moles of CCl, are introduced into a 1.00 L vessel at 350 K.
[ CH4]
M
[CC4]
M
[ CH2C1, ] =
M
Expert Solution
Step 1
The given reaction is
Equilibrium constant for the reaction is 9.52 at 350K
moles of CH4= 0.277
moles of CCl4=0.277
We're asked to calculate the equilibrium concentrations of reactants and products.
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