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For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H6(g)+H2(g)↽−−⇀2CH4(g)   the standard change in Gibbs free energy is  Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are  ?C2H6=0.250 atm ,  ?H2=0.200 atm , and  ?CH4=0.850 atm

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H6(g)+H2(g)↽−−⇀2CH4(g)   the standard change in Gibbs free energy is  Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are  ?C2H6=0.250 atm ,  ?H2=0.200 atm , and  ?CH4=0.850 atm

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 105QRT
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For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species.

For the reaction

C2H6(g)+H2(g)↽−−⇀2CH4(g)
 
the standard change in Gibbs free energy is  Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are  ?C2H6=0.250 atm ,  ?H2=0.200 atm , and  ?CH4=0.850 atm ? 

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