When is the overall free energy change ΔG in a reaction most likely to be negative (meaning that the reaction is exergonic)? When is the overall free energy change ΔG in a reaction most likely to be negative (meaning that the reaction is exergonic)? When products have higher potential energy and lower entropy than reactants 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

Question

When is the overall free energy change ΔG in a reaction most likely to be negative (meaning that the reaction is exergonic)? When is the overall free energy change ΔG in a reaction most likely to be negative (meaning that the reaction is exergonic)? 	 When products have higher potential energy and lower entropy than reactants 	 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

anonymous · Answer

I would recommend reading this article, it helps. http://en.wikipedia.org/wiki/Exergonic_reaction