Dissociation of products of combustion at high temperature can alter the expected composition. Determine if water is likely to form other products at 3000 K and 1 atm. Determine the equilibrium composition of O2, H₂ and H₂O at these conditions. Note: The reaction H₂O ⇒ H₂ + 1/2 O₂ is tabulated with log10Kp = -1.343 at 3000 K.
Dissociation of products of combustion at high temperature can alter the expected composition. Determine if water is likely to form other products at 3000 K and 1 atm. Determine the equilibrium composition of O2, H₂ and H₂O at these conditions. Note: The reaction H₂O ⇒ H₂ + 1/2 O₂ is tabulated with log10Kp = -1.343 at 3000 K.
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:Dissociation of products of combustion at high temperature can alter the expected composition.
Determine if water is likely to form other products at 3000 K and 1 atm. Determine the
equilibrium composition of O2, H₂ and H₂O at these conditions. Note: The reaction H₂O H₂ +
1/2 O₂ is tabulated with log₁0Kp = -1.343 at 3000 K.
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Step 1: Vant Hoff's isotherm
VIEWStep 2: Spontaneity and the change in the molar Gibbs free energy
VIEWStep 3: Spontaneity(feasibility) of decomposition of water at 3000 K and 1 atm
VIEWStep 4: The equilibrium constant Ky
VIEWStep 5: The Mole Balance Table
VIEWStep 6: Equilibrium composition of the vapour mixture
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