91Ó°ÊÓ

${\mathrm{Δ³Ò}}^{°}$corresponds to the change in free energy, ${\mathrm{Δ\pm á}}^{°}$corresponds to the enthalpy change, and ${\mathrm{Δ³\S }}^{°}$ represents the change in entropy.

width="134" height="22" role="math">Δ³Ò°=Δ±á°+TΔ³§

The free energy change of a reaction can be estimated/approximated using the change in the bonding energy i.e., the change in enthalpy.

${\mathrm{Δ³Ò}}^{°}≈{\mathrm{Δ\pm á}}^{°}$

The free energy change for favorable reactions (the reactions that favors product formation) is always negative.

Since ${\mathrm{Δ\pm á}}^{°}$is directly related to ${\mathrm{Δ³Ò}}^{°}$, a negative value of ${\mathrm{Δ\pm á}}^{°}$indicates that the reaction favors products, and a positive value of ${\mathrm{Δ\pm á}}^{°}$indicates that the reaction favors the reactants (starting material).

The negative value of indicates that the reaction favors products at equilibrium.