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: McGraw-Hill Education
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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.](https://content.bartleby.com/qna-images/question/9b020904-503e-46f0-a83a-8c74ba785f01/5023cfa4-d1b8-4402-87db-72ca5c8c6e12/m55x11a_processed.png)
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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