P4-10B Consider the elementary gas-phase reversible reaction A 2 3C Pure A enters at a temperature of 400 K and a pressure of 10 atm. At this temperature, Kc 0.25(mol/dm³)². Calculate the equilibrium conversion for each of the following situations: (a) The gas-phase reaction is carried out in a constant-volume batch reactor. (b) The gas-phase reaction is carried out in a constant-pressure batch reactor. (c) Can you explain the reason why there would be a difference in the two values of the equilibrium %3D conversion?

Introduction to Chemical Engineering Thermodynamics
8th Edition
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Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
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P4-10B Consider the elementary gas-phase reversible reaction
A 2 3C
Pure A enters at a temperature of 400 K and a pressure of 10 atm. At this temperature, Kc
0.25(mol/dm³)². Calculate the equilibrium conversion for each of the following situations:
(a) The gas-phase reaction is carried out in a constant-volume batch reactor.
(b) The gas-phase reaction is carried out in a constant-pressure batch reactor.
(c) Can you explain the reason why there would be a difference in the two values of the equilibrium
%3D
conversion?
Transcribed Image Text:P4-10B Consider the elementary gas-phase reversible reaction A 2 3C Pure A enters at a temperature of 400 K and a pressure of 10 atm. At this temperature, Kc 0.25(mol/dm³)². Calculate the equilibrium conversion for each of the following situations: (a) The gas-phase reaction is carried out in a constant-volume batch reactor. (b) The gas-phase reaction is carried out in a constant-pressure batch reactor. (c) Can you explain the reason why there would be a difference in the two values of the equilibrium %3D conversion?
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