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The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH2Cl2 (g) CH4 (9) + CCl4 (9) Calculate the equilibrium concentrations of reactant and products when 0.232 moles of CH₂ Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂ Cl₂] M [CH4] = = [CCL4] = M M

The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH2Cl2 (g) CH4 (9) + CCl4 (9) Calculate the equilibrium concentrations of reactant and products when 0.232 moles of CH₂ Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂ Cl₂] M [CH4] = = [CCL4] = M M

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
Section: Chapter Questions
Problem 71GQ: The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at...
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The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH2 Cl2 (g) CH4 (9) + CCl4 (9) Calculate the equilibrium concentrations of reactant and products when 0.232 moles of CH₂ Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂ Cl₂] M [CH₁] = = [CCL4] = M M
Transcribed Image Text:The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH2 Cl2 (g) CH4 (9) + CCl4 (9) Calculate the equilibrium concentrations of reactant and products when 0.232 moles of CH₂ Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂ Cl₂] M [CH₁] = = [CCL4] = M M
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