Calculate the equilibrium conversion and concentration for each of the following reactions: (A) The reversible reaction 2 A B is carried out in a flow reactor where pure A is fed at a concentration of 4.0 mol/dm³. If the equilibrium conversion is found to be 60%, then: (1) What is the equilibrium constant, Kc, if the reaction is a pure gas phase reaction? (2) What is the Kc if the reaction is a liquid phase reaction?
Calculate the equilibrium conversion and concentration for each of the following reactions: (A) The reversible reaction 2 A B is carried out in a flow reactor where pure A is fed at a concentration of 4.0 mol/dm³. If the equilibrium conversion is found to be 60%, then: (1) What is the equilibrium constant, Kc, if the reaction is a pure gas phase reaction? (2) What is the Kc if the reaction is a liquid phase reaction?
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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![**Chemical Equilibrium: Conversion and Concentration Analysis**
In this lesson, we will explore how to calculate the equilibrium conversion and concentration for a chemical reaction. The focus will be on the following reversible reaction:
\[ 2A \rightleftharpoons B \]
This reaction is performed in a flow reactor, where pure substance A is introduced at a concentration of 4.0 mol/dm³. The equilibrium conversion of substance A is observed to be 60%. Based on this information, we will address the following questions:
1. **Equilibrium Constant for Gas Phase Reaction:**
- Determine the equilibrium constant, \( K_c \), assuming the reaction occurs entirely in the gas phase.
2. **Equilibrium Constant for Liquid Phase Reaction:**
- Calculate \( K_c \) for the scenario where the reaction takes place in a liquid phase.
By understanding and solving these questions, you'll gain insights into how equilibrium concepts adapt based on the physical state of the reactants and products.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd47fc2c3-8f4b-4085-b234-bc909be774e3%2F0c2b49d6-0145-41e5-8624-401ca3a4b1df%2Fjmlevcj_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium: Conversion and Concentration Analysis**
In this lesson, we will explore how to calculate the equilibrium conversion and concentration for a chemical reaction. The focus will be on the following reversible reaction:
\[ 2A \rightleftharpoons B \]
This reaction is performed in a flow reactor, where pure substance A is introduced at a concentration of 4.0 mol/dm³. The equilibrium conversion of substance A is observed to be 60%. Based on this information, we will address the following questions:
1. **Equilibrium Constant for Gas Phase Reaction:**
- Determine the equilibrium constant, \( K_c \), assuming the reaction occurs entirely in the gas phase.
2. **Equilibrium Constant for Liquid Phase Reaction:**
- Calculate \( K_c \) for the scenario where the reaction takes place in a liquid phase.
By understanding and solving these questions, you'll gain insights into how equilibrium concepts adapt based on the physical state of the reactants and products.
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