If delta G (not delta G naught) is positive, it means that the reaction is not spontaneous and requires energy input to occur. In this case, there are more substrates than products at equilibrium.
The positive value of delta G tells us that the reaction is not favorable under current conditions. It suggests that the reactants have more free energy than the products, and the reaction would naturally go in the reverse direction.
To reach equilibrium, the reaction needs to proceed in the direction that reduces the free energy. Therefore, the reaction would need to go from products to substrates in order to reach equilibrium.
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