In industry, ethanol is produced from the hydration of ethylene. Calculate the value of theequilibrium constant for this reaction from 298 K to 800 K, and plot In(K) vs 1/T.Why does the reaction become non-spontaneous at higher temperatures?At what temperatures is this reaction typically run in industry? What else is different betweenthe reaction below and the industry standard? Provide at least two sources for your answer,using MLA citation format in your report.C2H4(g) + H2O(g)=C2H5OH (g)

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 16.DCP

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Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
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For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N,(g) + 3 H,(g) = 2 NH,(g) the standard change in Gibbs free energy is AG° = –72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, 0.200 atm, PH, = 0.350 atm, and PNH3 0.800 atm? AG = kJ/mol
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