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Consider ammonia synthesis: N₂ + H₂NH₂. At temperature (T) and pressure (P), the extent of 2 reaction at equilibrium (z) can be found, given the Equilibrium Constant K. Express the necessary objective function, in terms of the mole fractions y. (Ideal gases. Feed is stoichiometric in reactants, has no product.) Now suppose that the reaction is instead N₂ + 3H₂2NH₂. How will the objective function change (but

Consider ammonia synthesis: N₂ + H₂NH₂. At temperature (T) and pressure (P), the extent of 2 reaction at equilibrium (z) can be found, given the Equilibrium Constant K. Express the necessary objective function, in terms of the mole fractions y. (Ideal gases. Feed is stoichiometric in reactants, has no product.) Now suppose that the reaction is instead N₂ + 3H₂2NH₂. How will the objective function change (but

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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Consider ammonia synthesis: N₂ + H₂NH₂. At temperature (T) and pressure (P), the extent of reaction at equilibrium (z) can be found, given the Equilibrium Constant K. Express the necessary objective function, in terms of the mole fractions y. (Ideal gases. Feed is stoichiometric in reactants, has no product.) Now suppose that the reaction is instead N₂ + 3H₂2NH₂. How will the objective function change (but yield the same answer for z)? That is, what is the relation between the new Equilibrium Constant Knew and the current K? Hint: Compare the Free Energy of Formation AG, of the two reactions, and recall how K is related to AG,. What else is different in the new objective function?
Transcribed Image Text:Consider ammonia synthesis: N₂ + H₂NH₂. At temperature (T) and pressure (P), the extent of reaction at equilibrium (z) can be found, given the Equilibrium Constant K. Express the necessary objective function, in terms of the mole fractions y. (Ideal gases. Feed is stoichiometric in reactants, has no product.) Now suppose that the reaction is instead N₂ + 3H₂2NH₂. How will the objective function change (but yield the same answer for z)? That is, what is the relation between the new Equilibrium Constant Knew and the current K? Hint: Compare the Free Energy of Formation AG, of the two reactions, and recall how K is related to AG,. What else is different in the new objective function?
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