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 a1.00 L vessel at 350. K.[CH4] =[CCL][CH₂Cl₂] =2=MMM 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 Lvessel at 600 K.[Co][Cl₂][CoCl₂] =ΣΣΣ

Answered: Image /qna-images/answer/5570bb13-039e-4411-bc90-9e487a143d62.jpg

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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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