Answer :
Answer: The standard Gibbs free energy of the reaction is -15.8 kJ/mol
Explanation:
Relation between standard Gibbs free energy and equilibrium constant follows:
[tex]\Delta G^o=-RT\ln K_{eq}[/tex]
where,
[tex]\Delta G^o[/tex] = Standard Gibbs free energy = ?
R = Gas constant = [tex]8.314J/K mol[/tex]
T = temperature = 298 K
[tex]K_{eq}[/tex] = equilibrium constant = 581
Putting values in above equation, we get:
[tex]\Delta G^o=-(8.314J/Kmol)\times 298K\times \ln (581)\\\\\Delta G^o=-15769.13J/mol=-15.8kJ/mol[/tex]
Conversion factor used: 1 kJ = 1000 J
Hence, the standard Gibbs free energy of the reaction is -15.8 kJ/mol