4. Ethanol can be produced industrially using ethene gas and steam. The equation for the reaction is: C2H4(g) + H2O(g) = C2H50H(g) AH= -49kJmol-1 Although a high pressure and low temperature should produce the highest yield, this reaction is usually carried out under the compromise conditions of: pressure of 7Mpa temperature 3000C phosphoric acid (H3PO4) catalyst a. Use Le Chatelier's principle to explain why a high pressure is used to achieve a high yield in this process. b. Use Le Chatelier's principle to justify the use of the compromise temperature and catalyst in this process.

4. Ethanol can be produced industrially using ethene gas and steam. The equation for the reaction is: C2H4(g) + H2O(g) = C2H50H(g) AH= -49kJmol-1 Although a high pressure and low temperature should produce the highest yield, this reaction is usually carried out under the compromise conditions of: pressure of 7Mpa temperature 3000C phosphoric acid (H3PO4) catalyst a. Use Le Chatelier's principle to explain why a high pressure is used to achieve a high yield in this process. b. Use Le Chatelier's principle to justify the use of the compromise temperature and catalyst in this process.

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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