The equilibrium constant for the dissociation of ethanol into ethylene and water C₂H5OH(g) — C₂H4 (g) + H₂O(g) is 0.6246 at 351 K (the normal boiling point of ethanol). Calculate the degree of dissociation a at this temperature. The reaction does not normally occur (in the absence of a catalyst) because it is too slow. If it did, it would be a major problem for the distillers of alcoholic beverages. ? a data: K, T, P | C E C₂H5OH (g) 1 1- x C₂H₂(g) + H₂O(g) 0 0 x K = 1-x (1) + x 1/23

The equilibrium constant for the dissociation of ethanol into ethylene and water C₂H5OH(g) — C₂H4 (g) + H₂O(g) is 0.6246 at 351 K (the normal boiling point of ethanol). Calculate the degree of dissociation a at this temperature. The reaction does not normally occur (in the absence of a catalyst) because it is too slow. If it did, it would be a major problem for the distillers of alcoholic beverages. ? a data: K, T, P | C E C₂H5OH (g) 1 1- x C₂H₂(g) + H₂O(g) 0 0 x K = 1-x (1) + x 1/23

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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