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Problem 2. In the 1980's the U.S. government put forth the following plan for automobile manufacturers to reduce emission from automobiles over two decades: Hydrocarbons CO NO 1981 0.41 3.4 1.0 -TN = Year 1993 0.25 3.4 0.4 All values are in grams per mile. An automobile emitting 3.74 lb of CO and 0.37 lb of NO on a journey of 1000 miles would meet the current government requirements. To remove oxides of nitrogen (assumed to be NO) from automobile exhaust, a scheme has been proposed that uses unburned carbon monoxide (CO) in the exhaust to reduce the NO over a solid catalyst, according to the reaction CO + NO → Products (N₂, CO₂) Experimental data for a particular solid catalyst indicate the reaction rate can be well represented over a large range of temperature using the following rate law: 2004 0.125 1.7 0.2 kPNPC (1 + K₁PN + K₂Pc)² where PN = gas-phase partial pressure of NO and Pc = gas-phase partial pressure of CO. For this system, answer the following questions: (a) You are asked to propose an adsorption-surface reaction-desorption mechanism that will explain the experimentally observed kinetics. (b) An engineer in the company suggests it would be desirable to operate with a very large stoichiometric excess of CO to minimize catalytic reactor volume. Do you agree or disagree? Explain your answer.

Problem 2. In the 1980's the U.S. government put forth the following plan for automobile manufacturers to reduce emission from automobiles over two decades: Hydrocarbons CO NO 1981 0.41 3.4 1.0 -TN = Year 1993 0.25 3.4 0.4 All values are in grams per mile. An automobile emitting 3.74 lb of CO and 0.37 lb of NO on a journey of 1000 miles would meet the current government requirements. To remove oxides of nitrogen (assumed to be NO) from automobile exhaust, a scheme has been proposed that uses unburned carbon monoxide (CO) in the exhaust to reduce the NO over a solid catalyst, according to the reaction CO + NO → Products (N₂, CO₂) Experimental data for a particular solid catalyst indicate the reaction rate can be well represented over a large range of temperature using the following rate law: 2004 0.125 1.7 0.2 kPNPC (1 + K₁PN + K₂Pc)² where PN = gas-phase partial pressure of NO and Pc = gas-phase partial pressure of CO. For this system, answer the following questions: (a) You are asked to propose an adsorption-surface reaction-desorption mechanism that will explain the experimentally observed kinetics. (b) An engineer in the company suggests it would be desirable to operate with a very large stoichiometric excess of CO to minimize catalytic reactor volume. Do you agree or disagree? Explain your answer.

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
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Problem 2. In the 1980's the U.S. government put forth the following plan for automobile manufacturers to reduce emission from automobiles over two decades: Hydrocarbons CO NO 1981 0.41 3.4 1.0 Year 1993 2004 0.25 0.125 1.7 0.2 -TN = 3.4 0.4 All values are in grams per mile. An automobile emitting 3.74 lb of CO and 0.37 lb of NO on a journey of 1000 miles would meet the current government requirements. To remove oxides of nitrogen (assumed to be NO) from automobile exhaust, a scheme has been proposed that uses unburned carbon monoxide (CO) in the exhaust to reduce the NO over a solid catalyst, according to the reaction CO + NO → Products (N₂, CO₂) Experimental data for a particular solid catalyst indicate the reaction rate can be well represented over a large range of temperature using the following rate law: KPNPC (1 + K₁PN + K₂Pc)² where PN = gas-phase partial pressure of NO and Pc = gas-phase partial pressure of CO. For this system, answer the following questions: (a) You are asked to propose an adsorption-surface reaction-desorption mechanism that will explain the experimentally observed kinetics. (b) An engineer in the company suggests it would be desirable to operate with a very large stoichiometric excess of CO to minimize catalytic reactor volume. Do you agree or disagree? Explain your answer.
Transcribed Image Text:Problem 2. In the 1980's the U.S. government put forth the following plan for automobile manufacturers to reduce emission from automobiles over two decades: Hydrocarbons CO NO 1981 0.41 3.4 1.0 Year 1993 2004 0.25 0.125 1.7 0.2 -TN = 3.4 0.4 All values are in grams per mile. An automobile emitting 3.74 lb of CO and 0.37 lb of NO on a journey of 1000 miles would meet the current government requirements. To remove oxides of nitrogen (assumed to be NO) from automobile exhaust, a scheme has been proposed that uses unburned carbon monoxide (CO) in the exhaust to reduce the NO over a solid catalyst, according to the reaction CO + NO → Products (N₂, CO₂) Experimental data for a particular solid catalyst indicate the reaction rate can be well represented over a large range of temperature using the following rate law: KPNPC (1 + K₁PN + K₂Pc)² where PN = gas-phase partial pressure of NO and Pc = gas-phase partial pressure of CO. For this system, answer the following questions: (a) You are asked to propose an adsorption-surface reaction-desorption mechanism that will explain the experimentally observed kinetics. (b) An engineer in the company suggests it would be desirable to operate with a very large stoichiometric excess of CO to minimize catalytic reactor volume. Do you agree or disagree? Explain your answer.
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