The equilibrium constant, Kc, for the following reaction is 9.52x10-2 at 350 K. CH4(g) + CCl4(g) 2CH₂Cl₂(g) Calculate the equilibrium concentrations of reactants and product when 0.245 moles of CH4 and 0.245 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [CH4] [CC14] [CH₂Cl₂] = M M M
The equilibrium constant, Kc, for the following reaction is 9.52x10-2 at 350 K. CH4(g) + CCl4(g) 2CH₂Cl₂(g) Calculate the equilibrium concentrations of reactants and product when 0.245 moles of CH4 and 0.245 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [CH4] [CC14] [CH₂Cl₂] = M M M
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
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 1PS: Write equilibrium constant expressions for the following reactions. For gases, use either pressures...
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![The equilibrium constant, Kc, for the following reaction is 9.52x10-2 at 350 K.
CH4(g) + CCl4(g)
2CH₂Cl₂(g)
Calculate the equilibrium concentrations of reactants and product when 0.245 moles of CH4 and 0.245 moles of CCl4 are introduced into a 1.00 L vessel at 350 K.
[CH4]
[CCI4]
[CH₂Cl₂] =
=
=
M
ΣΣ](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf9e6852-449d-43c7-86eb-bcce975e72f8%2F7a740ff0-4fed-424a-a44d-e26151c62199%2Fxbf3oiln_processed.png&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, Kc, for the following reaction is 9.52x10-2 at 350 K.
CH4(g) + CCl4(g)
2CH₂Cl₂(g)
Calculate the equilibrium concentrations of reactants and product when 0.245 moles of CH4 and 0.245 moles of CCl4 are introduced into a 1.00 L vessel at 350 K.
[CH4]
[CCI4]
[CH₂Cl₂] =
=
=
M
ΣΣ
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