According to the Gibbs equation, the standard Gibbs free energy change ($\Delta G^\circ$) is given by: $\Delta G^\circ = \Delta H^\circ - T\Delta S^\circ$ Given: Standard enthalpy change, $\Delta H^\circ = -382.64\text{ kJ mol}^{-1}$ Standard entropy change, $\Delta S^\circ = -145.6\text{ J K}^{-1}\text{ mol}^{-1} = -0.1456\text{ kJ K}^{-1}\text{ mol}^{-1}$ Temperature, $T = 298\text{ K}$ Substituting the values into the equation: $\Delta G^\circ = -382.64\text{ kJ mol}^{-1} - (298\text{ K} \times -0.1456\text{ kJ K}^{-1}\text{ mol}^{-1})$ $\Delta G^\circ = -382.64 - (-43.3888)$ $\Delta G^\circ = -382.64 + 43.3888 = -339.2512\text{ kJ mol}^{-1} \approx -339.3\text{ kJ mol}^{-1}$