Question

gibbs free energy of the reaction (kj/mol)
reaction progress
reaction is exergonic and it favors the product formation
reaction is endergonic and it favors the reactant formation
reaction is exergonic and it favors the reactant formation
reaction is endergonic and it favors the product formation

Explanation:

Exergonic reactions have a negative change in Gibbs - free energy ($\Delta G<0$), meaning the products have lower free energy than the reactants. In the graph, the free energy of products (P) is lower than that of reactants (R), so it is an exergonic reaction. Exergonic reactions are spontaneous and favor product formation.

Answer:

Reaction is Exergonic and it favors the product formation