The relationship between change in Gibb's free energy, change in enthalpy and change in entropy is:
Δ [tex] G^{0} [/tex] = Δ[tex] H^{0} - T [/tex]Δ[tex] S^{0} [/tex]
For a reaction at equilibrium, Δ [tex] G^{0} [/tex] = 0
So Δ[tex] H^{0} - T [/tex]Δ[tex] S^{0} [/tex] = 0
Δ[tex] H^{0} = T [/tex]Δ[tex] S^{0} [/tex]
-92 kJ/mol = T(-0.199kJ/(mol.K))
T = 462 K
At temperatures greater than 462 K, the value T [/tex]Δ[tex] S^{0} [/tex] would become more than Δ[tex] H^{0} [/tex], giving a negative value for Δ [tex] G^{0} [/tex] . Therefore, the reaction would become spontaneous at temperatures > 462 K
