A student mixes \(1.0\text{ mol}\) of \(\text{H}_2(g)\) and \(0.50\text{ mol}\) of \(\text{O}_2(g)\) in a rigid, sealed \(2.0\text{ L}\) container at \(298\text{ K}\). The balanced chemical equation and standard Gibbs free energy change for the reaction are shown below. \[ 2\,\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\,\text{H}_2\text{O}(g) \quad \Delta G^\circ_{298} = -457\text{ kJ/mol}_{rxn} \] After several days at \(298\text{ K}\), the student observes that no measurable amount of \(\text{H}_2\text{O}(g)\) has formed and the total pressure in the container remains unchanged. Which of the following best explains why no reaction is observed at this temperature?