2. One of the most widely produced chemicals in the world is ammonium to be used as fertilizer. It is synthesized by the Haber process (∆G° = –32.9 kJ/mol):N2(g) + 3H2(g) → 2NH3(g)How much does this reaction proceeded if you start with n moles of nitrogen and 3n moles of hydrogen? Also, let’s assume that the reactor maintains a pressure of 1 bar like the reaction is in a balloon, and that the temperature is maintained at 25 °C.Question to answer:In question 2, why was the extent of the reaction: N2(g) + 3H2(g) → 2NH3(g) equal to α=0.968 if the pressure is maintained at 1 bar but drops slightly to =0.956 if the pressure drops to 0.5 bar? Hint: We use the table below to calculate mole fractions and partial pressures:N₂n(1 - α)n(1-α)4n - 2naAmount at equilibriumMole fractionsPartial pressures(1-α)4- 2a-PK =H₂3n(1 - α)3n(1 - α)4n - 2na3(1 - α)4 – 2αPInNH32na2na4n - 2nawhere a represents the extent of the reaction. K = Пi where P₁ is the partial pressure of speciespipou¡,i. As usual, Pº is just 1 bar. Now we can show:2α4-2α2α(42P)²4- 2a Po(4-20). P) (³(1-a). P)²4Simplification gives:22α P34-2α.( ²2 )² (1-² F) (¹-² F) ³ = 16a²(2-a)²_p-²4-2α(1-α)-4-2α3(1-α)27(1-x)4=PP2.Since the pressure is maintained at 1 bar and the standard pressure is 1 bar, we can eliminate thepressure component on the right side and are thus left with: K=When you plug this16a²(2-a)²27(1-α)4into the expression for the Gibbs energy at equilibrium 4µGº = −RT · ln(K):(16a² (2 - α)²)27(1-x)4you can solve for a given that AG° = -32.9 kJ/mol.-4,GoRT

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Answered: One of the most widely produced…

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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Question

2. One of the most widely produced chemicals in the world is ammonium to be used as fertilizer. It is synthesized by the Haber process (∆G° = –32.9 kJ/mol):
N2(g) + 3H2(g) → 2NH3(g)
How much does this reaction proceeded if you start with n moles of nitrogen and 3n moles of hydrogen? Also, let’s assume that the reactor maintains a pressure of 1 bar like the reaction is in a balloon, and that the temperature is maintained at 25 °C.

Question to answer:

In question 2, why was the extent of the reaction: N2(g) + 3H2(g) → 2NH3(g) equal to α=0.968 if the pressure is maintained at 1 bar but drops slightly to =0.956 if the pressure drops to 0.5 bar?