A system is in dynamical equilibrium at equilibrium. At the same time, both the forward and backward responses exist. If the difference in Gibbs energy for the forward reaction is G, so the change in Gibbs energy is -G for the backward reaction. This is why energy from Gibbs is zero at equilibrium.
Unfavorable reactions to positive Delta G values (also called endergonic reactions). A reaction is considered to be at equilibrium when the Delta G for a reaction is zero. Equilibrium does NOT imply equivalent degrees. There is no net difference in A and B if Delta G is zero, since the system is at equilibrium.
Over the course of every natural process, the Gibbs energy G is a number that becomes more harmful. Thus, G just sinks and can never get more favourable when a chemical reaction takes place. G is at a minimum at this stage (see below), and there can be no more net change; the reaction is then at equilibrium.