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The equilibrium constant, Ke, for the following reaction is 0.0952 at 350. K. CH4 (9) + CCl4 (9) = 2CH₂Cl₂ (9) Calculate the equilibrium concentrations of reactants and product when 0.220 moles of CH4 and 0.220 moles of CCl4 are introduced into a 1.00 L vessel at 350. K. [CH₂] = [CCL]=[ [CH₂ C1₂] = M M M

The equilibrium constant, Ke, for the following reaction is 0.0952 at 350. K. CH4 (9) + CCl4 (9) = 2CH₂Cl₂ (9) Calculate the equilibrium concentrations of reactants and product when 0.220 moles of CH4 and 0.220 moles of CCl4 are introduced into a 1.00 L vessel at 350. K. [CH₂] = [CCL]=[ [CH₂ C1₂] = M M M

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 127QRT: The standard equilibrium constant is 2.1109for this reaction at 25 C Zn2+(aq)+4NH3(aq)Zn(NH3)42+(aq)...
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Equilibrium Concentrations part 1 and 2

The equilibrium constant, Kc, for the following reaction is 0.0952 at 350. K. CH4 (9) + CCl4 (9) 2CH₂ Cl2 (9) Calculate the equilibrium concentrations of reactants and product when 0.220 moles of CH4 and 0.220 moles of CCl4 are introduced into a 1.00 L vessel at 350. K. [CH4] = [CCL] [CH₂Cl₂] = 2 = M M M
Transcribed Image Text:The equilibrium constant, Kc, for the following reaction is 0.0952 at 350. K. CH4 (9) + CCl4 (9) 2CH₂ Cl2 (9) Calculate the equilibrium concentrations of reactants and product when 0.220 moles of CH4 and 0.220 moles of CCl4 are introduced into a 1.00 L vessel at 350. K. [CH4] = [CCL] [CH₂Cl₂] = 2 = M M M
The equilibrium constant, K, for the following reaction is 77.5 at 600 K. CO(g) + Cl₂(g) —cocl₂(g) Calculate the equilibrium concentrations of reactant and products when 0.562 moles of CO and 0.562 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K. [Co] [Cl₂] [CoCl₂] = ΣΣΣ
Transcribed Image Text:The equilibrium constant, K, for the following reaction is 77.5 at 600 K. CO(g) + Cl₂(g) —cocl₂(g) Calculate the equilibrium concentrations of reactant and products when 0.562 moles of CO and 0.562 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K. [Co] [Cl₂] [CoCl₂] = ΣΣΣ
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