A student investigates the biochemical synthesis of glucose-6-phosphate from glucose and inorganic phosphate (\(\text{P}_i\)). The individual chemical equations and their standard Gibbs free energy changes at \(298\text{ K}\) are shown below.

\[ \text{Glucose(aq)} + \text{P}_i\text{(aq)} \rightleftharpoons \text{Glucose-6-phosphate(aq)} + \text{H}_2\text{O(l)} \quad \Delta G^\circ_{298} = +14\text{ kJ/mol}_{\text{rxn}} \]
\[ \text{ATP(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{ADP(aq)} + \text{P}_i\text{(aq)} \quad \Delta G^\circ_{298} = -31\text{ kJ/mol}_{\text{rxn}} \]

Which of the following statements best explains whether the net reaction coupling the phosphorylation of glucose to the hydrolysis of \(\text{ATP}\) is thermodynamically favorable under standard conditions at \(298\text{ K}\)?