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1. H₂ is fed at a rate of 8.2 kg/min and N₂ is fed at a rate of 13.9 kg/min to a Haber-Bosch reactor to synthesize ammonia, a very important fertilizer. a. For this Haber-Bosch reactor, which reactant is limiting? b. How many moles of NH3 can be produced? C. For the reactant that is non-limiting, calculate the fractional excess.

1. H₂ is fed at a rate of 8.2 kg/min and N₂ is fed at a rate of 13.9 kg/min to a Haber-Bosch reactor to synthesize ammonia, a very important fertilizer. a. For this Haber-Bosch reactor, which reactant is limiting? b. How many moles of NH3 can be produced? C. For the reactant that is non-limiting, calculate the fractional excess.

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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Please make sure that you show all of your work. Please use line calculations and show all units throughout intermediate steps and in your final answer. Please combine all of your solutions into one file and upload by the deadline. Solutions must be uploaded in pdf form. 1. H₂ is fed at a rate of 8.2 kg/min and N₂ is fed at a rate of 13.9 kg/min to a Haber-Bosch reactor to synthesize ammonia, a very important fertilizer. a. For this Haber-Bosch reactor, which reactant is limiting? b. How many moles of NH3 can be produced? c. For the reactant that is non-limiting, calculate the fractional excess. d. If only 1.9 kg/min of ammonia is produced, what is the fractional conversion of the excess reactant? e. If only 1.9 kg/min of ammonia is produced, what is the extent of reaction? T 2. 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? CH3OH + CH3COOH → CH3COOCH3 + H₂O
Transcribed Image Text:Please make sure that you show all of your work. Please use line calculations and show all units throughout intermediate steps and in your final answer. Please combine all of your solutions into one file and upload by the deadline. Solutions must be uploaded in pdf form. 1. H₂ is fed at a rate of 8.2 kg/min and N₂ is fed at a rate of 13.9 kg/min to a Haber-Bosch reactor to synthesize ammonia, a very important fertilizer. a. For this Haber-Bosch reactor, which reactant is limiting? b. How many moles of NH3 can be produced? c. For the reactant that is non-limiting, calculate the fractional excess. d. If only 1.9 kg/min of ammonia is produced, what is the fractional conversion of the excess reactant? e. If only 1.9 kg/min of ammonia is produced, what is the extent of reaction? T 2. 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? CH3OH + CH3COOH → CH3COOCH3 + H₂O
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