Final answer:
The suitable reactions involve analyzing ΔG; a negative value indicates an exothermic reaction, while a positive value denotes an endothermic reaction.
Step-by-step explanation:
The subject of the question relates to determining whether a chemical reaction is exothermic or endothermic based on the change in Gibbs free energy (ΔG) for each reaction given. An exothermic reaction is one that releases energy to the surroundings, usually indicated by a negative ΔG, indicating that the reaction can occur spontaneously under standard conditions. On the other hand, an endothermic reaction absorbs energy from the surroundings and is indicated by a positive ΔG, suggesting that the reaction is not spontaneous under standard conditions.
In the proposed reactions, the first reaction (B + F <--> G + H) with ΔG = -5.4 kcal/mole is exothermic, as the negative ΔG indicates energy is released. The other reactions (C + F <--> G + H with ΔG = +9.7 kcal/mole and A + F <--> G + H with ΔG = +10.2 kcal/mole) are both endothermic as their positive ΔG values suggest that they absorb energy.