Acetaldehyde (CH3CHO) is produced by dehydrogenation of ethanol (C2HSOH). C2HSOH S CH3CHO + H2 (R1) An undesired side reaction produces ethyl acetate (CH3COOC2H5) 2C2HSOH S CH3COOC2HS + 2H2 (R2) 120 gmol ethanol/ h is fed continuously to a pilot-plant scale reactor. The exit gas flow rate is 166 gmol/h. The exit gases are analyzed and found to contain 41.7 mol% ethanol, 30.65 mol% Hz, 24.6 mol% acetaldehyde and 3.0 mol% ethyl acetate. Calculate 31, 32, fractional conversion of ethanol, and fractional selectivity for producing acetaldehyde from ethanol.
Acetaldehyde (CH3CHO) is produced by dehydrogenation of ethanol (C2HSOH). C2HSOH S CH3CHO + H2 (R1) An undesired side reaction produces ethyl acetate (CH3COOC2H5) 2C2HSOH S CH3COOC2HS + 2H2 (R2) 120 gmol ethanol/ h is fed continuously to a pilot-plant scale reactor. The exit gas flow rate is 166 gmol/h. The exit gases are analyzed and found to contain 41.7 mol% ethanol, 30.65 mol% Hz, 24.6 mol% acetaldehyde and 3.0 mol% ethyl acetate. Calculate 31, 32, fractional conversion of ethanol, and fractional selectivity for producing acetaldehyde from ethanol.
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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![**Title: Chemical Reaction Analysis and Calculation**
**Introduction:**
This section provides a detailed analysis of the chemical reaction involving ethanol, acetaldehyde, and ethyl acetate. The calculations include flow rates, compositions, and selectivity for the given reaction process.
**Details:**
1. **Ethanol Feed and Exit Gas Flow Rate:**
- Ethanol fed = 120 gmol/h
- Exit gas flow rate = 166 gmol/h
2. **Composition of Exit Gas:**
- Ethanol (C₂H₅OH): 41.7 mol%
- Hydrogen (H₂): 30.65 mol%
- Acetaldehyde: 24.6 mol%
- Ethyl acetate: 3 mol%
3. **Calculations:**
- **Moles of C₂H₅OH in the product:**
\[
166 \times 0.417 = 69.22 \, \text{gmol/h}
\]
- **Moles of Acetaldehyde:**
\[
166 \times 0.246 = 40.84 \, \text{gmol/h}
\]
- **Moles of Ethyl Acetate:**
\[
166 \times 0.03 = 4.98 \, \text{gmol/h}
\]
4. **Fractional Conversion:**
\[
F_{C_2E} = \frac{120 - 69.22}{120} = 0.423
\]
5. **Selectivity:**
- Defined as the ratio of moles of acetaldehyde to moles of ethyl acetate.
\[
S = \frac{40.84}{4.98} = 8.2
\]
**Conclusion:**
The selectivity for acetaldehyde over ethyl acetate in the reaction is 8.2, indicating a higher conversion preference towards acetaldehyde. The fractional conversion of ethanol is 0.423, demonstrating the extent of ethanol consumption in the process.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff4dfc165-1571-419f-99fc-a4587d76c340%2Fd91d0557-c234-4625-a850-4a50b9bd27a4%2Ftmcyndg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Chemical Reaction Analysis and Calculation**
**Introduction:**
This section provides a detailed analysis of the chemical reaction involving ethanol, acetaldehyde, and ethyl acetate. The calculations include flow rates, compositions, and selectivity for the given reaction process.
**Details:**
1. **Ethanol Feed and Exit Gas Flow Rate:**
- Ethanol fed = 120 gmol/h
- Exit gas flow rate = 166 gmol/h
2. **Composition of Exit Gas:**
- Ethanol (C₂H₅OH): 41.7 mol%
- Hydrogen (H₂): 30.65 mol%
- Acetaldehyde: 24.6 mol%
- Ethyl acetate: 3 mol%
3. **Calculations:**
- **Moles of C₂H₅OH in the product:**
\[
166 \times 0.417 = 69.22 \, \text{gmol/h}
\]
- **Moles of Acetaldehyde:**
\[
166 \times 0.246 = 40.84 \, \text{gmol/h}
\]
- **Moles of Ethyl Acetate:**
\[
166 \times 0.03 = 4.98 \, \text{gmol/h}
\]
4. **Fractional Conversion:**
\[
F_{C_2E} = \frac{120 - 69.22}{120} = 0.423
\]
5. **Selectivity:**
- Defined as the ratio of moles of acetaldehyde to moles of ethyl acetate.
\[
S = \frac{40.84}{4.98} = 8.2
\]
**Conclusion:**
The selectivity for acetaldehyde over ethyl acetate in the reaction is 8.2, indicating a higher conversion preference towards acetaldehyde. The fractional conversion of ethanol is 0.423, demonstrating the extent of ethanol consumption in the process.
![**Title: Production of Acetaldehyde from Ethanol**
**Introduction:**
Acetaldehyde (\( \text{CH}_3\text{CHO} \)) is produced by the dehydrogenation of ethanol (\( \text{C}_2\text{H}_5\text{OH} \)).
**Reactions:**
1. **Main Reaction:**
\[
\text{C}_2\text{H}_5\text{OH} \rightleftharpoons \text{CH}_3\text{CHO} + \text{H}_2 \quad \text{(R1)}
\]
2. **Side Reaction:**
\[
2\text{C}_2\text{H}_5\text{OH} \rightleftharpoons \text{CH}_3\text{COOC}_2\text{H}_5 + 2\text{H}_2 \quad \text{(R2)}
\]
**Process Details:**
- 120 gmol of ethanol per hour is fed continuously to a pilot-plant scale reactor.
- Exit gas flow rate is 166 gmol/h.
- Exit gas composition:
- 41.7 mol% ethanol
- 30.65 mol% hydrogen (\( \text{H}_2 \))
- 24.6 mol% acetaldehyde
- 3.0 mol% ethyl acetate (\( \text{CH}_3\text{COOC}_2\text{H}_5 \))
**Calculations:**
- Moles of \( \text{C}_2\text{H}_5\text{OH} \) in products:
\[
166 \times 0.417 = 69.22 \, \text{gmol/h}
\]
- Moles of acetaldehyde:
\[
166 \times 0.246 = 40.84 \, \text{gmol/h}
\]
- Moles of ethyl acetate:
\[
166 \times 0.03 = 4.98 \, \text{gmol/h}
\]
**Variables:**
- \( \xi_1 \) for acetaldehyde:
\[
= 40.84 \, \text{gmol/h](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff4dfc165-1571-419f-99fc-a4587d76c340%2Fd91d0557-c234-4625-a850-4a50b9bd27a4%2Ftuncfe5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Production of Acetaldehyde from Ethanol**
**Introduction:**
Acetaldehyde (\( \text{CH}_3\text{CHO} \)) is produced by the dehydrogenation of ethanol (\( \text{C}_2\text{H}_5\text{OH} \)).
**Reactions:**
1. **Main Reaction:**
\[
\text{C}_2\text{H}_5\text{OH} \rightleftharpoons \text{CH}_3\text{CHO} + \text{H}_2 \quad \text{(R1)}
\]
2. **Side Reaction:**
\[
2\text{C}_2\text{H}_5\text{OH} \rightleftharpoons \text{CH}_3\text{COOC}_2\text{H}_5 + 2\text{H}_2 \quad \text{(R2)}
\]
**Process Details:**
- 120 gmol of ethanol per hour is fed continuously to a pilot-plant scale reactor.
- Exit gas flow rate is 166 gmol/h.
- Exit gas composition:
- 41.7 mol% ethanol
- 30.65 mol% hydrogen (\( \text{H}_2 \))
- 24.6 mol% acetaldehyde
- 3.0 mol% ethyl acetate (\( \text{CH}_3\text{COOC}_2\text{H}_5 \))
**Calculations:**
- Moles of \( \text{C}_2\text{H}_5\text{OH} \) in products:
\[
166 \times 0.417 = 69.22 \, \text{gmol/h}
\]
- Moles of acetaldehyde:
\[
166 \times 0.246 = 40.84 \, \text{gmol/h}
\]
- Moles of ethyl acetate:
\[
166 \times 0.03 = 4.98 \, \text{gmol/h}
\]
**Variables:**
- \( \xi_1 \) for acetaldehyde:
\[
= 40.84 \, \text{gmol/h
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