If ΔG = ΔH - TΔS, when is the overall free energy change (ΔG) in a reaction most likely to be negative (meaning that the reaction is exergonic)?

A. when products have lower potential energy and higher entropy than reactants
B. when products have higher potential energy and lower entropy than reactants
C. when products have lower potential energy and lower entropy than reactants
D. when products have higher potential energy and higher entropy than reactants

Question

If ΔG = ΔH - TΔS, when is the overall free energy change (ΔG) in a reaction most likely to be negative (meaning that the reaction is exergonic)?

A. when products have lower potential energy and higher entropy than reactants
B. when products have higher potential energy and lower entropy than reactants
C. when products have lower potential energy and lower entropy than reactants
D. when products have higher potential energy and higher entropy than reactants

anonymous · Answer

Hello dmarcynyszyn. Welcome to OpenStudy, I see you are new. However this is not History related. You have posted this in the History section. Please move it to a different section. You can select different subjects and topics at the top where it says "Find More Subjects" from there you can find a whole bunch of categories that I'm sure will fit your needs! This is considered as spam, please read the code of conduct at http://openstudy.com/code-of-conduct Thanks and have a wonderful day!