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For the ammonia synthesis reaction, N:(8) + H2 → NH3(g) the equilibrium conversion to ammonia is large at 300 K, but it decreases rapidly with increasing T. However, reaction rates become appreciable only at higher temperatures. For a feed mixture of hydrogen and nitrogen in the stoichiometric proportions, (a) What is the equilibrium mole fraction of ammonia at 1 bar and 300 K? (b) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 1 bar? (c) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal gas? (d) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal solution of gases?

For the ammonia synthesis reaction, N:(8) + H2 → NH3(g) the equilibrium conversion to ammonia is large at 300 K, but it decreases rapidly with increasing T. However, reaction rates become appreciable only at higher temperatures. For a feed mixture of hydrogen and nitrogen in the stoichiometric proportions, (a) What is the equilibrium mole fraction of ammonia at 1 bar and 300 K? (b) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 1 bar? (c) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal gas? (d) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal solution of gases?

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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For the ammonia synthesis reaction, N2(8) +H2 → NH3(g) the equilibrium conversion to ammonia is large at 300 K, but it decreases rapidly with increasing T. However, reaction rates become appreciable only at higher temperatures. For a feed mixture of hydrogen and nitrogen in the stoichiometric proportions, (a) What is the equilibrium mole fraction of ammonia at 1 bar and 300 K? (b) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 1 bar? (c) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal gas? (d) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal solution of gases?
Transcribed Image Text:For the ammonia synthesis reaction, N2(8) +H2 → NH3(g) the equilibrium conversion to ammonia is large at 300 K, but it decreases rapidly with increasing T. However, reaction rates become appreciable only at higher temperatures. For a feed mixture of hydrogen and nitrogen in the stoichiometric proportions, (a) What is the equilibrium mole fraction of ammonia at 1 bar and 300 K? (b) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 1 bar? (c) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal gas? (d) At what temperature does the equilibrium mole fraction of ammonia equal 0.50 for a pressure of 100 bar, assuming the equilibrium mixture is an ideal solution of gases?
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