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
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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![**Problem 2**: In the 1980s, the U.S. government put forth a plan for automobile manufacturers to reduce emissions over two decades:
| Year | Hydrocarbons | CO | NO |
|------|--------------|-----|-----|
| 1981 | 0.41 | 3.4 | 1.0 |
| 1993 | 0.25 | 3.4 | 0.4 |
| 2004 | 0.125 | 1.7 | 0.2 |
- All values are in grams per mile. An automobile emitting 3.74 lb of CO and 0.37 lb of NO over 1000 miles would meet current requirements.
- To remove nitrogen oxides (assumed to be NO) from exhaust, a scheme has been proposed using unburned carbon monoxide (CO) in the exhaust to reduce NO over a solid catalyst. The reaction is:
\[ \text{CO + NO} \rightarrow \text{Products } (N_2, CO_2) \]
- Experimental data for a specific solid catalyst indicate that the reaction rate is well represented over a wide temperature range by the rate law:
\[ -r'_{N} = \frac{k P_N P_C}{(1 + K_1 P_N + K_2 P_C)^2} \]
Where:
- \( P_N \) = gas-phase partial pressure of NO
- \( P_C \) = gas-phase partial pressure of CO
**Questions:**
(a) Propose an adsorption-surface reaction-desorption mechanism that explains the observed kinetics.
(b) An engineer proposes operating with an excess of CO to minimize catalytic reactor volume. Agree or disagree and explain.
This educational content covers historical emission reduction regulations, fundamental chemical reaction mechanisms, and catalyst kinetics.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b020904-503e-46f0-a83a-8c74ba785f01%2F5023cfa4-d1b8-4402-87db-72ca5c8c6e12%2Fm55x11a_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem 2**: In the 1980s, the U.S. government put forth a plan for automobile manufacturers to reduce emissions over two decades:
| Year | Hydrocarbons | CO | NO |
|------|--------------|-----|-----|
| 1981 | 0.41 | 3.4 | 1.0 |
| 1993 | 0.25 | 3.4 | 0.4 |
| 2004 | 0.125 | 1.7 | 0.2 |
- All values are in grams per mile. An automobile emitting 3.74 lb of CO and 0.37 lb of NO over 1000 miles would meet current requirements.
- To remove nitrogen oxides (assumed to be NO) from exhaust, a scheme has been proposed using unburned carbon monoxide (CO) in the exhaust to reduce NO over a solid catalyst. The reaction is:
\[ \text{CO + NO} \rightarrow \text{Products } (N_2, CO_2) \]
- Experimental data for a specific solid catalyst indicate that the reaction rate is well represented over a wide temperature range by the rate law:
\[ -r'_{N} = \frac{k P_N P_C}{(1 + K_1 P_N + K_2 P_C)^2} \]
Where:
- \( P_N \) = gas-phase partial pressure of NO
- \( P_C \) = gas-phase partial pressure of CO
**Questions:**
(a) Propose an adsorption-surface reaction-desorption mechanism that explains the observed kinetics.
(b) An engineer proposes operating with an excess of CO to minimize catalytic reactor volume. Agree or disagree and explain.
This educational content covers historical emission reduction regulations, fundamental chemical reaction mechanisms, and catalyst kinetics.
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