A student ran the following reaction in the laboratory at 375 K: CH4(g) + CCI4(g) = 2CH2CI2(g) When she introduced 4.58x10-2 moles of CH4(g) and 6.00x102 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 1.68x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

A student ran the following reaction in the laboratory at 375 K: CH4(g) + CCI4(g) = 2CH2CI2(g) When she introduced 4.58x10-2 moles of CH4(g) and 6.00x102 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 1.68x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

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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