The table shows the variation of standard Gibbs energy with temperature for a reversible reaction.

The table shows the variation of standard Gibbs energy with temperature for a reversible reaction.

$\Delta G = \Delta H - T\Delta S$

$\Delta G^\ominus = -RT \ln{K}$

$$\begin{array}{|c|c|} \hline \text { Temperature } / \mathbf{K} & \Delta \mathbf{G}^{\boldsymbol{}} / \mathbf{~ k J ~} \mathbf{m o l}^{-1} \\ \hline 297 & 20.6 \\ \hline 355 & -1.9 \\ \hline 395 & -23.8 \\ \hline \end{array}$$

What can be concluded about the reaction?