An elementary irreversible gas-phase reaction, A → B + C, is carried out at fixed temperature and pressure in two separate ideal reactors: (i) a 10 m plug flow reactor (PFR), (ii) a 10 m3 continuous-stirred tank reactor (CSTR). If pure A is fed at 5 m3 h-1 to the PFR operating at 400 K, the conversion is 80%. If a mixture of 50 mol% of A and 50 mol% of an inert is fed at 5 m³ h-1 to the CSTR operating at 425 K, the conversion is 80%. The universal gas constant R = 8.314 J mol-1 K-1. Assuming the Arrhenius rate law, the estimated activation energy is kJ mol-1 (rounded off to one decimal place).
An elementary irreversible gas-phase reaction, A → B + C, is carried out at fixed temperature and pressure in two separate ideal reactors: (i) a 10 m plug flow reactor (PFR), (ii) a 10 m3 continuous-stirred tank reactor (CSTR). If pure A is fed at 5 m3 h-1 to the PFR operating at 400 K, the conversion is 80%. If a mixture of 50 mol% of A and 50 mol% of an inert is fed at 5 m³ h-1 to the CSTR operating at 425 K, the conversion is 80%. The universal gas constant R = 8.314 J mol-1 K-1. Assuming the Arrhenius rate law, the estimated activation energy is kJ mol-1 (rounded off to one decimal place).
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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Transcribed Image Text:An elementary irreversible gas-phase reaction, A → B + C, is carried out at fixed
temperature and pressure in two separate ideal reactors: (i) a 10 m plug flow reactor
(PFR), (ii) a 10 m3 continuous-stirred tank reactor (CSTR). If pure A is fed at 5 m3 h-1
to the PFR operating at 400 K, the conversion is 80%. If a mixture of 50 mol% of A
and 50 mol% of an inert is fed at 5 m³ h-1 to the CSTR operating at 425 K, the conversion
is 80%. The universal gas constant R = 8.314 J mol-1 K-1. Assuming the Arrhenius rate
law, the estimated activation energy is
kJ mol-1 (rounded off to one decimal
place).
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