A plug flow reactor is used to carry out parallel reactions that convert reactants A and B to a desired product D and an undesired product C. The reactor operates under isothermal and isobaric conditions. If an equimola
A plug flow reactor is used to carry out parallel reactions that convert reactants A and B to a desired product D and an undesired product C. The reactor operates under isothermal and isobaric conditions. If an equimola
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
Related questions
Question
A plug flow reactor is used to carry out parallel reactions that convert reactants A and
B to a desired product D and an undesired product C. The reactor operates under isothermal and isobaric
conditions. If an equimolar feed (CA,o = CB,o = 2 mol cm-3) undergoes a 65% conversion in the PFR, calculate
the concentrations of desired product CD and undesired product CC exiting the reactor. [Hint: use the
Levenspiel yield approach]
![### Reaction Kinetics
In this section, we explore a set of chemical reaction kinetics involving two parallel reactions:
1. **Reaction Pathways:**
- **Reaction 1:**
\[
A + B \xrightarrow{k_1} 2D
\]
- **Reaction 2:**
\[
A + B \xrightarrow{k_2} 2C
\]
2. **Rate Expressions:**
- The rate of disappearance of reactant \( A \) in Reaction 1 is expressed as:
\[
-r_{A,1} = k_1 C_A
\]
- The rate of disappearance of reactant \( A \) in Reaction 2 is expressed as:
\[
-r_{A,2} = k_2 C_A C_B
\]
3. **Rate Constants:**
- The rate constant for Reaction 1 (\( k_1 \)) is \( 2.8 \, \text{min}^{-1} \).
- The rate constant for Reaction 2 (\( k_2 \)) is \( 1.4 \, \text{L mol}^{-1} \text{min}^{-1} \).
These equations help determine how the concentration of reactants \( A \) and \( B \) influences the rate at which products \( D \) and \( C \) are formed. Understanding these kinetics is critical for optimizing reaction conditions in industrial and laboratory settings.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b020904-503e-46f0-a83a-8c74ba785f01%2F97ac2962-3fb7-4222-8c9f-721d90db1ba7%2Fi8qfmk_processed.png&w=3840&q=75)
Transcribed Image Text:### Reaction Kinetics
In this section, we explore a set of chemical reaction kinetics involving two parallel reactions:
1. **Reaction Pathways:**
- **Reaction 1:**
\[
A + B \xrightarrow{k_1} 2D
\]
- **Reaction 2:**
\[
A + B \xrightarrow{k_2} 2C
\]
2. **Rate Expressions:**
- The rate of disappearance of reactant \( A \) in Reaction 1 is expressed as:
\[
-r_{A,1} = k_1 C_A
\]
- The rate of disappearance of reactant \( A \) in Reaction 2 is expressed as:
\[
-r_{A,2} = k_2 C_A C_B
\]
3. **Rate Constants:**
- The rate constant for Reaction 1 (\( k_1 \)) is \( 2.8 \, \text{min}^{-1} \).
- The rate constant for Reaction 2 (\( k_2 \)) is \( 1.4 \, \text{L mol}^{-1} \text{min}^{-1} \).
These equations help determine how the concentration of reactants \( A \) and \( B \) influences the rate at which products \( D \) and \( C \) are formed. Understanding these kinetics is critical for optimizing reaction conditions in industrial and laboratory settings.
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