a) Consider the reaction network of the gaseous isomerisation, decomposition and dimerisation reactions of the same reactant A: Isomerisation: Decomposition: A B+C Dimerisation: 2A D At the reaction temperature, the equilibrium constants, expressed in terms of partial pressures, are: Isomerisation: KI = 5 Decomposition: KDe = 0.5 bar Dimerisation: KDi = 5 bar -1 At 1 bar, there is only 1 mol of A initially. Express the mole-fraction of each reaction component at equilibrium as function of the extents of the three reactions at equilibrium, či, čde, čDi. Calculations resulted in the following values of the extents of the three reactions, isomerisation, decomposition and dimerization at equilibrium: Š= 0.5400 mol, ŠDe = 0.2553 mol, EDI= 0.0483 mol. Calculate the equilibrium mole-fractions of reaction components A, I, B, C and D and show that the equilibrium extent values are correct. b) If the pressure increases, how would each one of the above quantities - equilibrium extents of each reaction and mole-fractions of each component- change and why? c) If the temperature increases, how would each one of the above quantities change and why? For your answer, consider the nature of the above reactions.
a) Consider the reaction network of the gaseous isomerisation, decomposition and dimerisation reactions of the same reactant A: Isomerisation: Decomposition: A B+C Dimerisation: 2A D At the reaction temperature, the equilibrium constants, expressed in terms of partial pressures, are: Isomerisation: KI = 5 Decomposition: KDe = 0.5 bar Dimerisation: KDi = 5 bar -1 At 1 bar, there is only 1 mol of A initially. Express the mole-fraction of each reaction component at equilibrium as function of the extents of the three reactions at equilibrium, či, čde, čDi. Calculations resulted in the following values of the extents of the three reactions, isomerisation, decomposition and dimerization at equilibrium: Š= 0.5400 mol, ŠDe = 0.2553 mol, EDI= 0.0483 mol. Calculate the equilibrium mole-fractions of reaction components A, I, B, C and D and show that the equilibrium extent values are correct. b) If the pressure increases, how would each one of the above quantities - equilibrium extents of each reaction and mole-fractions of each component- change and why? c) If the temperature increases, how would each one of the above quantities change and why? For your answer, consider the nature of the above reactions.
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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Transcribed Image Text:a) Consider the reaction network of the gaseous isomerisation, decomposition and
dimerisation reactions of the same reactant A:
Isomerisation:
Decomposition:
Aस्B
B+C
Dimerisation:
2A D
At the reaction temperature, the equilibrium constants, expressed in terms of partial
pressures, are:
Isomerisation:
KI = 5
Decomposition:
KDe = 0.5 bar
Dimerisation:
KDi = 5 bar -1
At 1 bar, there is only 1 mol of A initially. Express the mole-fraction of each reaction
component at equilibrium as function of the extents of the three reactions at
equilibrium, či, čDe, ŠDi.
Calculations resulted in the following values of the extents of the three reactions,
isomerisation, decomposition and dimerization at equilibrium: Š= 0.5400 mol, EDe =
0.2553 mol, čDi= 0.0483 mol.
Calculate the equilibrium mole-fractions of reaction components A, I, B, C and D and
show that the equilibrium extent values are correct.
b) If the pressure increases, how would each one of the above quantities - equilibrium
extents of each reaction and mole-fractions of each component- change and why?
c) If the temperature increases, how would each one of the above quantities change
and why? For your answer, consider the nature of the above reactions.
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