Final answer:
An exothermic reaction with a negative ΔG (option c) is likely to be product-favored because it indicates that the reaction is energetically favorable and spontaneous.
Step-by-step explanation:
It deals with predicting whether a chemical reaction is product-favored based on its thermodynamic properties, looking at both the enthalpy change (ΔH) and the Gibbs free energy change (ΔG) of the reaction.
Reaction (c) is described as being exothermic with a negative ΔG, which is the hallmark of a reaction that is energetically favorable and would be product-favored.
An exothermic reaction releases energy which contributes to a negative ΔG, and according to the Gibbs free energy equation, a negative ΔG implies that the reaction is spontaneous and will proceed without any additional energy input.