In industry, ethanol is produced from the hydration of ethylene. Calculate the value of the equilibrium 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 between the 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)

In industry, ethanol is produced from the hydration of ethylene. Calculate the value of the equilibrium 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 between the 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)

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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Consider the following reaction: shown in photo 1.1 Determine the estimated value of the equilibrium constant for this reaction at 200 degrees celcius by making use of the following data: Shown in photo 1.2 Based on your final answer in question 1.1, is the reaction reactant- or product favoured at this temperature? Use a short sentence to explain your answer. 1.3 Calculate the value of ΔrG for this reaction at this temperature, if O2 and SO2 are present at 0.900 atm and 0.800 atm, respectively.
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Calculate AHxn for the reaction 2Ni(s) + 25(s) + 30,(g) – → 2NISO, (s) from the following information: 1. Niso,(s) - Nio(s) + So,(g) = 156 kJ rxn 2. s(s) + 0,(3) so, (g) AH° =-297 kJ fxn 3. Ni(s) + 0,(g) → Nio(s) AH° =-241 kJ rxn AH pn= kJ
The equilibrium constant of the reaction COCl2(g) CO(g) + Cl2(g) was found to fit the expression ln K = + 1.75 ln T(K) – 2.667 Find the degree of dissociation of COCl2(g) at 227°C when the total pressure is 2 bar. Calculate the standard reaction enthaply and standard reaction entropy at 227°C.
Consider the following reaction: A (g) + B(g) ↔ 2C(g) Kp = 0.0825 at 298 K Calculate ΔG (J/mol) at 25°C when P(A) = 1.50 atm, P(B) = 3.20 atm and P(C) = 4.00 atm Enter your answer with the correct number of sig figs, without any units. If you want to use scientific notation, use the #e# format.
99+ [References] Use the References to access important values if needed for this question. Consider the reaction H₂(g) + Cl₂(g) →→→→2HCI(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of HCI(g) is reduced to 13.25 mm Hg, while the pressures of H₂(g) and Cl₂(g) remain at 1 atm. ANSWER: Submit Answer B kJ/mol Try Another Version 1 item attempt remaining Previous Next 3:18 AM 11/22/2022
For which reactions or processes is AS > 0? Select all that apply 2 C,H6(1) + 15 O2(g) →12 CO2(g) + 6 H2O(1) O PH3BCI3(s) → PH3(g) + BCI3(g) Fe3+(aq)+ 3CI(aq) →FECI3(s) Na(s) → Na(g) 6CO2(g) + 6H2O(g) → C6H1206(s) + 602(g O 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(1)
Using Appendix II from your textbook and DG°rxn for the reaction below, determine the standard Gibbs Free energy of formation, DG°F, for urea (CO(NH2)2) (aq). CO(NH2)2 (aq) + H20 (1) --> CO2 (g) + 2 NH3 (g) DG° = 13 kJ Edit View Insert Format Tools Table 12pt v Paragraph v BIUA 2v Tン: PrtScn
At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4 B(g) 2C(g) + 2D(g) were found to be PA = 4.67 atm, På = 5.73 atm, Pc = 5.60 atm, and Pp = 5.84 atm. What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ mol privacy policy contact us help terms of use 6:11 PM about us careers 3/25/202
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 87.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. Al₂O3(s) + 2Fe(s) → 2Al(s) + Fe₂O₂ (s) AH = 852. kJ AS = 2272. AG = | KJ J K Which is spontaneous? this reaction the reverse reaction neither 3
Species AG° Fe(OH)3 -696.5 Fe+ -4.6 OH -157.3 Calculate the AG° of the reaction: Fe(OH)3(s) = Fe*(aq) + 3 OH (aq) T= 25° C Express the answer to 1 decimal place. kJ
s) The equilibrium constant of a reaction is found to fit the expression In K = A + B/T + C/T3 between 400 K and 500 K with A = -2.04, B = -1176 K, and C = 2.1 x 107 K3. Calculate the standard reaction enthalpy and standard reaction entropy at 450 K.