Calculate the standard free energy change and equilibrium constant for the vapor-phase hydration of ethylene at 145°C. Hydration of ethylene means reaction of ethylene with water vapor to produce ethanol vapor as per reaction below: C2H4(g) + H2O(g) → C₂H5OH(g) From the heat-capacity data: (Table C.1) Constants in equation C½³/R = A + BT + CT² + DT−² for T (K) from 298 K A Ethylene (C2H4) 1.424 103 B 14.394 Water vapor (H₂O) 3.470 1.450 Ethanol (C₂HO) 3.518 20.001 106 C -4.392 -6.002 Values of AH298° and AG298° at 298.15 K for the hydration reaction are found from the heat-of-formation and Gibbs-energy-of-formation data. (Table C.4) Ethylene (C2H4) Water vapor (H₂O) Ethanol (C₂HO) 68,460 A Hf 298 52,510 A Gf 298 -241,818 -228,572 -235,100 -168,490
Calculate the standard free energy change and equilibrium constant for the vapor-phase hydration of ethylene at 145°C. Hydration of ethylene means reaction of ethylene with water vapor to produce ethanol vapor as per reaction below: C2H4(g) + H2O(g) → C₂H5OH(g) From the heat-capacity data: (Table C.1) Constants in equation C½³/R = A + BT + CT² + DT−² for T (K) from 298 K A Ethylene (C2H4) 1.424 103 B 14.394 Water vapor (H₂O) 3.470 1.450 Ethanol (C₂HO) 3.518 20.001 106 C -4.392 -6.002 Values of AH298° and AG298° at 298.15 K for the hydration reaction are found from the heat-of-formation and Gibbs-energy-of-formation data. (Table C.4) Ethylene (C2H4) Water vapor (H₂O) Ethanol (C₂HO) 68,460 A Hf 298 52,510 A Gf 298 -241,818 -228,572 -235,100 -168,490
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Need Correct answer, How to use Cpig/R values Datas in your calculations. Please I'm confused in it mostly.
Transcribed Image Text:Calculate the standard free energy change and equilibrium constant for the vapor-phase hydration of
ethylene at 145°C. Hydration of ethylene means reaction of ethylene with water vapor to produce ethanol
vapor as per reaction below:
C₂H4(g) + H₂O(g) → C₂H5OH(g)
From the heat-capacity data: (Table C.1)
Constants in equation C/R = A + BT + CT² + DT−² for T (K) from 298 K
Ethylene (C₂H4)
Water vapor (H₂O)
Ethanol (C₂H5O)
A
1.424
Ethylene (C₂H4)
Water vapor (H₂O)
Ethanol (C₂HO)
3.470
3.518
10³ B
14.394
1.450
20.001
106 C
-4.392
Values of AH298° and AG298 at 298.15 K for the hydration reaction are found from the heat-of-formation and
Gibbs-energy-of-formation data. (Table C.4)
A Hf 298
52,510
-241,818
-235,100
-6.002
A Gf 298
68,460
-228,572
-168,490
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