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The equilibrium constant, K., for the following reaction is 9.52x102 at 350 K. CH4 (g) + CCl, (g) 2 CH,Cl,2 (g) Calculate the equilibrium concentrations of reactants and product when 0.339 moles of CH, and 0.339 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] M [CC4] M [ CH,Cl, ] =|

The equilibrium constant, K., for the following reaction is 9.52x102 at 350 K. CH4 (g) + CCl, (g) 2 CH,Cl,2 (g) Calculate the equilibrium concentrations of reactants and product when 0.339 moles of CH, and 0.339 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] M [CC4] M [ CH,Cl, ] =|

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, K., for the following reaction is 9.52x102 at 350 K. CH4 (g) + CC1, (g) 2 CH,Cl,2 (g) Calculate the equilibrium concentrations of reactants and product when 0.339 moles of CH, and 0.339 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CCI4 ] [ CH,Cl, ] = | M M
Transcribed Image Text:The equilibrium constant, K., for the following reaction is 9.52x102 at 350 K. CH4 (g) + CC1, (g) 2 CH,Cl,2 (g) Calculate the equilibrium concentrations of reactants and product when 0.339 moles of CH, and 0.339 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CCI4 ] [ CH,Cl, ] = | M M
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