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The equilibrium constant at 25oC for the reaction H2+ S-→→→→→H2S is 6.0×105 calculate the a.standard enthalpy change b.standard free energy change c.standard entropy change Given that AG°E = 2.303RTlog k also given that the enthalpy values for H2S and S are 0.0001 and -21Kj/mol respectively (R=8.314J/kmol)

The equilibrium constant at 25oC for the reaction H2+ S-→→→→→H2S is 6.0×105 calculate the a.standard enthalpy change b.standard free energy change c.standard entropy change Given that AG°E = 2.303RTlog k also given that the enthalpy values for H2S and S are 0.0001 and -21Kj/mol respectively (R=8.314J/kmol)

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 equilibrium constant at 25oC for the reaction H2+ S-→→→→→H2S is 6.0×105 calculate the a.standard enthalpy change b.standard free energy change c.standard entropy change Given that AG°E = 2.303RTlog k also given that the enthalpy values for H2S and S are 0.0001 and -21Kj/mol respectively (R=8.314J/kmol)
Transcribed Image Text:The equilibrium constant at 25oC for the reaction H2+ S-→→→→→H2S is 6.0×105 calculate the a.standard enthalpy change b.standard free energy change c.standard entropy change Given that AG°E = 2.303RTlog k also given that the enthalpy values for H2S and S are 0.0001 and -21Kj/mol respectively (R=8.314J/kmol)
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