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A reversible reaction is done in an isothermal constant-volume batch reactor as shown: A(1) B(l) The reaction is found to be first-order in both A and B. Using CAO = 0.75" L mol mol and CRO = 0.25 m², it took 1.25 hours to achieve 60% conversion of A. If the equilibrium conversion is 90%, what conversion will we expect after 1.50 hours under the same conditions?

A reversible reaction is done in an isothermal constant-volume batch reactor as shown: A(1) B(l) The reaction is found to be first-order in both A and B. Using CAO = 0.75" L mol mol and CRO = 0.25 m², it took 1.25 hours to achieve 60% conversion of A. If the equilibrium conversion is 90%, what conversion will we expect after 1.50 hours under the same conditions?

Introduction to Chemical Engineering Thermodynamics
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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A reversible reaction is done in an isothermal constant-volume batch reactor as shown: A(1) B(l) mol The reaction is found to be first-order in both A and B. Using CAO = 0.75- L mol and CRO = 0.25 m², it took 1.25 hours to achieve 60% conversion of A. If the equilibrium conversion is 90%, what conversion will we expect after 1.50 hours under the same conditions?
Transcribed Image Text:A reversible reaction is done in an isothermal constant-volume batch reactor as shown: A(1) B(l) mol The reaction is found to be first-order in both A and B. Using CAO = 0.75- L mol and CRO = 0.25 m², it took 1.25 hours to achieve 60% conversion of A. If the equilibrium conversion is 90%, what conversion will we expect after 1.50 hours under the same conditions?
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