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Introduction to Chemical Engineering Thermodynamics | 8th Edition | ISBN: 9781259696527 | Authors: J.M. Smith, Hendrick Van Ness, Michael Abbott, Mark Swihart ISBN: 9781259696527 2049

Solution for problem 14.20 Chapter 14

Introduction to Chemical Engineering Thermodynamics | 8th Edition

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Introduction to Chemical Engineering Thermodynamics | 8th Edition | ISBN: 9781259696527 | Authors: J.M. Smith, Hendrick Van Ness, Michael Abbott, Mark Swihart

Introduction to Chemical Engineering Thermodynamics | 8th Edition

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Problem 14.20

For the ammonia synthesis reaction,

\(\frac{1}{2} \mathrm{N}_{2}(g)+\frac{3}{2} \mathrm{H}_{2} \rightarrow \mathrm{NH}_{3}(g)\)

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?

Text Transcription:

1/2 N_2(g)+3/2 H_2 rightarrow NH_3(g)

Step-by-Step Solution:
Step 1 of 3

Table of Contents Kevin M. Hoover ................................................................................................................ 1 Blank Workspace ................................................................................................................ 1 Lab ................................................................................................................................... 1 Output Table ...................................................................................................................... 2 Functions ........................................................................................................................... 4 Kevin M. Hoover %Lab 10, Week 10 %12/03/2014 Blank Workspace clear all; close all; clc; Lab load('pts_setC.mat'); x = ptsMixC(1,:); y = ptsMixC(2,:); [b0 b1,LF]=linearfitf(x,y); [B0 B1 B2,QF] = quadfitf(x,y); STDLF = std(LF-y); STDQF = std(QF-y); out1 = ['Linear fit error:(std Dev.): ',num2str(STDLF)]; out2 = ['Quadratic fit error:(std Dev.): ',num2str(STDQF)]; legend('Observations', out1,out2,'Location','southeast') %Beta Values: %%Linear Fit: %%%-10.4510 %%%7.3884 %%Quadratic Fit: %%%-0.4149 %%%4.3498 %%%0.1521 1 Output Table out3 = [' | X | Y |';' -------------']; out4 = [ptsMixC']; disp(ou

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Chapter 14, Problem 14.20 is Solved
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Textbook: Introduction to Chemical Engineering Thermodynamics
Edition: 8
Author: J.M. Smith, Hendrick Van Ness, Michael Abbott, Mark Swihart
ISBN: 9781259696527

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