107. A student ran the following reaction in the laboratory at 287 K:2CH₂Cl₂ (9) CH. (g) + CCl4 (9)When she introduced 0,0732 moles of CH₂Cl₂ (g) into a 1.00 liter container, she found the equilibrium concentration of CCL, (g)to be 0.0340 M.Calculate the equilibrium constant, Ke. she obtained for this reaction.Ke

Answered: Image /qna-images/answer/5ebe7c0c-73c7-4df6-91a8-2415187f2f16.jpg

A student ran the following reaction in the laboratory at 287 K: 2CH₂Cl₂ (9) CH. (g) + CCl4 (9) When she introduced 0.0732 moles of CH₂Cl₂ (9) into a 1.00 liter container, she found the equilibrium concentration of CCl4 (9) to be 0.0340 M. Calculate the equilibrium constant, Ke, she obtained for this reaction. Ke

A student ran the following reaction in the laboratory at 287 K: 2CH₂Cl₂ (9) CH. (g) + CCl4 (9) When she introduced 0.0732 moles of CH₂Cl₂ (9) into a 1.00 liter container, she found the equilibrium concentration of CCl4 (9) to be 0.0340 M. Calculate the equilibrium constant, Ke, she obtained for this reaction. Ke

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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