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(4) At a reaction temperature of 1000 K, when Cg = 1 mol/L, which one of the two products (i.e., D vs. U) has a higher formation rate? Explain your answer. (5) To promote the formation of D, should we use CSTR or PFR? Why? Assume that mass transfer is not limiting. (6) To promote the formation of D, should we operate the reaction at a higher or lower temperature? Why?

(4) At a reaction temperature of 1000 K, when Cg = 1 mol/L, which one of the two products (i.e., D vs. U) has a higher formation rate? Explain your answer. (5) To promote the formation of D, should we use CSTR or PFR? Why? Assume that mass transfer is not limiting. (6) To promote the formation of D, should we operate the reaction at a higher or lower temperature? Why?

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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i need help with last 3 parts of this question (4),(5) and (6) asap

Consider a complex reaction system: In k A -B rA¬B = k,C^ kp D A *1•B ky * U ľB¬D = kpCg B•D B-U • 1/T 0.002 0.001 where A is the reactant, B is a reaction intermediate, D is the desired product, and U is the undesired product. The rate constants of the three reactions are kı, kD, and ku, respectively. The rate law for each reaction is provided above. The Arrhenius relationships for the three reactions are plotted in the above figure. (1) If the rates of the reactions (i.e., ra¬B, rB–D, and r3-u) have the units of mol/(L-s), write down the units for kı, kp, and ku, respectively. (2) At a reaction temperature of 500 K, which one of the three reactions is the rate-limiting (rate- determining) reaction in terms of producing D? Explain your answer. (3) At a reaction temperature of 500 K, when Cg = 1 mol/L, which one of the two products (i.e., D vs. U) has a higher formation rate? Explain your answer. (4) At a reaction temperature of 1000 K, when Cg = 1 mol/L, which one of the two products (i.e., D vs. U) has a higher formation rate? Explain your answer. (5) To promote the formation of D, should we use CSTR or PFR? Why? Assume that mass transfer is not limiting. (6) To promote the formation of D, should we operate the reaction at a higher or lower temperature? Why?
Transcribed Image Text:Consider a complex reaction system: In k A -B rA¬B = k,C^ kp D A *1•B ky * U ľB¬D = kpCg B•D B-U • 1/T 0.002 0.001 where A is the reactant, B is a reaction intermediate, D is the desired product, and U is the undesired product. The rate constants of the three reactions are kı, kD, and ku, respectively. The rate law for each reaction is provided above. The Arrhenius relationships for the three reactions are plotted in the above figure. (1) If the rates of the reactions (i.e., ra¬B, rB–D, and r3-u) have the units of mol/(L-s), write down the units for kı, kp, and ku, respectively. (2) At a reaction temperature of 500 K, which one of the three reactions is the rate-limiting (rate- determining) reaction in terms of producing D? Explain your answer. (3) At a reaction temperature of 500 K, when Cg = 1 mol/L, which one of the two products (i.e., D vs. U) has a higher formation rate? Explain your answer. (4) At a reaction temperature of 1000 K, when Cg = 1 mol/L, which one of the two products (i.e., D vs. U) has a higher formation rate? Explain your answer. (5) To promote the formation of D, should we use CSTR or PFR? Why? Assume that mass transfer is not limiting. (6) To promote the formation of D, should we operate the reaction at a higher or lower temperature? Why?
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