Areaction is designated as exergonic rather than endergonic when

Reaction is called exergonic when ΔG is negative i.e. ΔG < 0  

Explanation:

The Gibbs free energy represents the spontaneity or feasibility of a given chemical reaction at constant pressure and temperature and is given by the equation:

ΔG = ΔH - TΔS

Here, ΔG - change in the Gibbs free energy

ΔS -  change in the entropy

ΔH - change in the enthalpy

T - temperature

If the value of ΔG for a chemical reaction is positive i.e. ΔG > 0, then the given chemical reaction is said to be nonspontaneous. Such a reaction is called endergonic.

Whereas, if the ΔG value for a chemical reaction is negative i.e. ΔG < 0, then the given chemical reaction is said to be spontaneous. Such a reaction is called exergonic.

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