A chemical reaction has a standard Gibbs free-energy change of ΔG∘=+12.5kJmol−1. Which of the following statements is correct about the reaction under standard conditions?
a) Because ΔG∘ is positive, the equilibrium constant K is greater than 1, so the reaction proceeds spontaneously toward products.
b) The reaction is non-spontaneous under standard conditions because a positive ΔG∘ indicates that reactants are thermodynamically favored.
c) The reaction is spontaneous since a positive ΔG∘ means the products have lower free energy than the reactants.
d) The reaction rate will be high because a positive ΔG∘ reduces the activation energy barrier.