The dissolution of potassium chloride, \(\text{KCl}(s)\), in water is represented by the equation below.

\[\text{KCl}(s) \rightarrow \text{K}^+(aq) + \text{Cl}^-(aq)\]

For this process at \(300\text{ K}\), the standard enthalpy change, \(\Delta H^\circ\), is \(+17.0\text{ kJ/mol}_{\text{rxn}}\) and the standard entropy change, \(\Delta S^\circ\), is \(+70.0\text{ J/(mol}_{\text{rxn}}\cdot\text{K)}\). Based on these data, what is the standard Gibbs free energy change, \(\Delta G^\circ\), for the dissolution of \(\text{KCl}(s)\) at \(300\text{ K}\)?