Consider the elementary gas-phase reversible reaction A← ⎯⎯⎯⎯→ 3CPure 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 conversion?
Consider the elementary gas-phase reversible reaction A← ⎯⎯⎯⎯→ 3CPure 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 conversion?
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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Consider the elementary gas-phase reversible reaction
A← ⎯⎯⎯⎯→ 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 conversion?
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