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The following data are available for the two "traditional” solid forms of carbon at 300 K, Allotrope diamond graphite AH combustion (kJ/mol) 395.320 393.425 5° (J/mol-K) 2.397 5.740 Density (g/cm³) 3.513 2.260 (a) What is the Gibbs energy (in kJ/mol) of the transition from graphite to diamond at 1 bar and 300 K? In which direction is the process spontaneous? Using these same parameters, calculate the Gibbs energy at 1000 K. Does the system move closer to or further from phase equilibrium at this higher temperature? (b) Estimate the pressure (in bars) at which the two allotropes would be in equilibrium at 1000 K. To address this question, consider how the Gibbs energy changes with pressure at a given T using (36) = V. Assume that the densities of the two allotropes are T independent of pressure (this is actually incorrect in real life!).

The following data are available for the two "traditional” solid forms of carbon at 300 K, Allotrope diamond graphite AH combustion (kJ/mol) 395.320 393.425 5° (J/mol-K) 2.397 5.740 Density (g/cm³) 3.513 2.260 (a) What is the Gibbs energy (in kJ/mol) of the transition from graphite to diamond at 1 bar and 300 K? In which direction is the process spontaneous? Using these same parameters, calculate the Gibbs energy at 1000 K. Does the system move closer to or further from phase equilibrium at this higher temperature? (b) Estimate the pressure (in bars) at which the two allotropes would be in equilibrium at 1000 K. To address this question, consider how the Gibbs energy changes with pressure at a given T using (36) = V. Assume that the densities of the two allotropes are T independent of pressure (this is actually incorrect in real life!).

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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The following data are available for the two "traditional" solid forms of carbon at 300 K, Allotrope AH combustion (kJ/mol) 5° (J/mol-K) Density (g/cm³) diamond 2.397 graphite 5.740 (a) What is the Gibbs energy (in kJ/mol) of the transition from graphite to diamond at 1 bar and 300 K? In which direction is the process spontaneous? Using these same parameters, calculate the Gibbs energy at 1000 K. Does the system move closer to or further from phase equilibrium at this higher temperature? 395.320 393.425 3.513 2.260 (b) Estimate the pressure (in bars) at which the two allotropes would be in equilibrium at 1000 K. To address this question, consider how the Gibbs energy changes with pressure at a given T using (30) = V. Assume that the densities of the two allotropes are ӘР. independent of pressure (this is actually incorrect in real life!).
Transcribed Image Text:The following data are available for the two "traditional" solid forms of carbon at 300 K, Allotrope AH combustion (kJ/mol) 5° (J/mol-K) Density (g/cm³) diamond 2.397 graphite 5.740 (a) What is the Gibbs energy (in kJ/mol) of the transition from graphite to diamond at 1 bar and 300 K? In which direction is the process spontaneous? Using these same parameters, calculate the Gibbs energy at 1000 K. Does the system move closer to or further from phase equilibrium at this higher temperature? 395.320 393.425 3.513 2.260 (b) Estimate the pressure (in bars) at which the two allotropes would be in equilibrium at 1000 K. To address this question, consider how the Gibbs energy changes with pressure at a given T using (30) = V. Assume that the densities of the two allotropes are ӘР. independent of pressure (this is actually incorrect in real life!).
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