In an exergonic reaction, what is the ##DeltaG##?

##DeltaG## is negative, which means that the reaction is spontaneous in the forward direction.

As the chemical reaction proceeds, the reactants are being converted into products. The reactants are higher in energy than the products because energy must be released as the products are being formed. Since the reactants are losing energy, the free energy change must be negative (##Delta G<0##)

I hope this makes sense!