Recall that the **standard Gibbs free energy change of a reaction (ΔG˚ _{rxn})** is given by the following equation:

$\overline{){\mathbf{\u2206}}{{\mathbf{G}}}_{\mathbf{r}\mathbf{x}\mathbf{n}}{\mathbf{\xb0}}{\mathbf{=}}{\mathbf{\u2206}}{{\mathbf{H}}}_{\mathbf{r}\mathbf{x}\mathbf{n}}{\mathbf{\xb0}}{\mathbf{-}}{\mathbf{T}}{\mathbf{\u2206}}{{\mathbf{S}}}_{\mathbf{r}\mathbf{x}\mathbf{n}}{\mathbf{\xb0}}}$

We know that for a particular reaction, **ΔH = 120.5 kJ** and** ΔS = 758.2 J/K at T = 298 K. **

For a particular reaction, ΔH = 120.5 kJ and ΔS = 758.2 J/K. What is ΔG for this reaction at 298 K?