Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.257 moles of CH2Cl2(g), 0.350 moles of CH4, and 0.657 moles of CCl4 are at equilibrium in a 10.3 L container at 422 K, the value of the equilibrium constant, Kc, is .
Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.257 moles of CH2Cl2(g), 0.350 moles of CH4, and 0.657 moles of CCl4 are at equilibrium in a 10.3 L container at 422 K, the value of the equilibrium constant, Kc, is .
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.2QE: Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium...
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Consider the following reaction:
2CH2Cl2(g) CH4(g) + CCl4(g)
If 0.257 moles of CH2Cl2(g), 0.350 moles of CH4, and 0.657 moles of CCl4 are at equilibrium in a 10.3 L container at 422 K, the value of the equilibrium constant, Kc, is .
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