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

Hugo Gutierrez

Biology

26 February, 22:14

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

+4

Answers (1)

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Madelyn Harvey · Answer 1

If ΔG = ΔH - TΔS in a reaction most likely to be negative, this means when products have higher potential energy and higher entropy than reactants. This means the entropy is positive making the whole term negative. This is also considered a spontaneous type of reaction.