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Determine the equilibrium concentrations of the conversion of the hydrobutyric acid in dilute solution, i.e.: CH₂ CH3-CH₂-CH₂-COOH ⇒CH₂ - CH₂-C=O+H₂ o The initial concentration of the acid at 25°C is 0.182 mol/L and the equilibrium constant is 2.68.

Determine the equilibrium concentrations of the conversion of the hydrobutyric acid in dilute solution, i.e.: CH₂ CH3-CH₂-CH₂-COOH ⇒CH₂ - CH₂-C=O+H₂ o The initial concentration of the acid at 25°C is 0.182 mol/L and the equilibrium constant is 2.68.

Introduction to Chemical Engineering Thermodynamics
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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Determine the equilibrium concentrations of the conversion of the hydrobutyric acid in dilute solution, i.e.: CH ₂ CH3-CH₂-CH₂-COOH CH₂ - CH₂ - C = O + H₂ 0 The initial concentration of the acid at 25°C is 0.182 mol/L and the equilibrium constant is 2.68.
Transcribed Image Text:Determine the equilibrium concentrations of the conversion of the hydrobutyric acid in dilute solution, i.e.: CH ₂ CH3-CH₂-CH₂-COOH CH₂ - CH₂ - C = O + H₂ 0 The initial concentration of the acid at 25°C is 0.182 mol/L and the equilibrium constant is 2.68.
Expert Solution
Step 1

Given reaction for conversion of hydrobutyric acid is-

Chemical Engineering homework question answer, step 1, image 1

Representing the equation in form of-

A⇔R

Initial concentration of acid, CAi= 0.182 mol/L

Temperature, T=250C

Equilibrium constant, Keq=2.68

If equilibrium fraction for A= XA

Equilibrium fraction of R= (1-XA)

Representing the equilibrium constant as function of concentration-

K=CReCAe=XA(1-XA)

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