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
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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.
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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