Methanol (CH3OH) and acetic acid (CH3COOH) react in the gas phase at a temperature of 170°C toform methyl acetate (CH3COOCH3) and water. At 170°C, this reaction has an equilibrium constant of3.87. A chemical engineer wants to use 92 mol of methanol to produce 68 mol of CH3COOCH3 oncethe reaction has reached equilibrium. How much CH3COOH must be fed? What is the finalcomposition of the equilibrium mixture? 2. Methanol (CH3OH) and acetic acid (CH3COOH) react in the gas phase at a temperature of 170°C toform methyl acetate (CH3COOCH3) and water. At 170°C, this reaction has an equilibrium constant of3.87. A chemical engineer wants to use 92 mol of methanol to produce 68 mol of CH3COOCH3 oncethe reaction has reached equilibrium. How much CH3COOH must be fed? What is the finalcomposition of the equilibrium mixture?CH3OH + CH3COOH → CH3COOCH3 + H₂O

Given data: Equilibrium constant = 3.87 Initial number of moles of methanol = 92 mol Moles of…

Answered: Methanol (CH3OH) and acetic acid…

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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Methanol (CH3OH) and acetic acid (CH3COOH) react in the gas phase at a temperature of 170°C to
form methyl acetate (CH3COOCH3) and water. At 170°C, this reaction has an equilibrium constant of
3.87. A chemical engineer wants to use 92 mol of methanol to produce 68 mol of CH3COOCH3 once
the reaction has reached equilibrium. How much CH3COOH must be fed? What is the final
composition of the equilibrium mixture?