Question

when is the overall free energy change δg in a reaction most likely to be negative (meaning that the reaction is exergonic)? see section 8.1.
when products have higher potential energy and higher entropy than reactants.
when products have lower potential energy and higher entropy than reactants.
when products have lower potential energy and lower entropy than reactants.
when products have higher potential energy and lower entropy than reactants.

Explanation:

The Gibbs free - energy change formula is \(\Delta G=\Delta H - T\Delta S\). For \(\Delta G\) to be negative (exergonic reaction), \(\Delta H\) (enthalpy change related to potential energy) should be negative (products have lower potential energy than reactants) and \(\Delta S\) (entropy change) should be positive (products have higher entropy than reactants).

Answer:

When products have lower potential energy and higher entropy than reactants.