At which temperature would a reaction with h = -92 kj/mol, s = -0.199 kj/(molk) be spontaneous?

The relationship between change in Gibb's free energy, change in enthalpy and change in entropy is:

Δ = ΔΔ

For a reaction at equilibrium, Δ = 0

So ΔΔ = 0

ΔΔ

-92 kJ/mol = T(-0.199kJ/(mol.K))

T = 462 K

At temperatures greater than 462 K, the value T [/tex]Δ would become more than Δ, giving a negative value for Δ . Therefore, the reaction would become spontaneous at temperatures > 462 K