At a certain temperature \(T\), the standard Gibbs free energy change for the gas-phase reaction represented below is \(\Delta G^\circ = -5.7\text{ kJ/mol}_{\text{rxn}}\), and the equilibrium constant is \(K_p = 10.0\).

\[ \text{I}_2(g) + \text{Cl}_2(g) \rightleftharpoons 2\,\text{ICl}(g) \]

A rigid reaction vessel at temperature \(T\) is filled with the gases such that the initial partial pressures are \(P_{\text{I}_2} = 0.20\text{ atm}\), \(P_{\text{Cl}_2} = 0.20\text{ atm}\), and \(P_{\text{ICl}} = 2.0\text{ atm}\). Which of the following correctly predicts the sign of the instantaneous Gibbs free energy change, \(\Delta G\), for the forward reaction under these initial conditions and the direction the reaction will proceed to reach equilibrium?