Final answer:
Option c is the answer. The incorrect thermodynamic reason for a process being endergonic is that it 'liberates free energy.' Endergonic reactions require an input of energy and the products have higher free energy than the reactants, making them non-spontaneous and energy-consuming.
Step-by-step explanation:
The thermodynamic reason that is NOT why a process or reaction could be endergonic is: The process or reaction liberates free energy. Because an endergonic reaction requires an input of energy and is characterized by the products having higher free energy than the reactants, it does not liberate free energy; it is energy consuming. If a process releases free energy, it is typically exothermic and the reactions are spontaneous, contradicting the definition of an endergonic reaction.
Conversely, endergonic reactions, which are non-spontaneous, often have a positive ∆G value, indicating that free energy is absorbed to convert reactants to products. The case where the concentration of reactants and products favors too much product can also lead to a non-spontaneous (endergonic) reaction, as it shifts away from equilibrium towards the reactants. Lastly, a significant loss of entropy (decrease in disorder) in the system can contribute to the non-spontaneous nature of endergonic reactions, as this also requires input of energy to maintain the orderliness of the system.