Final answer:
The closer the value of ΔG is to zero, the closer the reaction is to equilibrium.
Step-by-step explanation:
The closer the value of ΔG (Gibbs free energy) is to zero, the closer the reaction is to equilibrium.
When ΔG is less than zero, the reaction is spontaneous in the forward direction and is far from equilibrium. As ΔG approaches zero, the reaction becomes closer to equilibrium.
For example, if the reaction has a ΔG of -10 kJ/mol, it is more spontaneous and further from equilibrium compared to a reaction with a ΔG of -2 kJ/mol, which is less spontaneous and closer to equilibrium.