the following graph was obtained.

$lnK=\frac{-H^0}{RT}+\frac{S^o}{R}$

Given the above relationship, use the graph to identify which of the following statements are "true" or "false" in this specific case.

All statements refer to the forward reaction $($proceeding left to right, as given$)$ corresponding to the equilibrium constant $K.$

The reaction is spontaneous at low temperatures but not at the highest temperatures.

$?S$ for the reaction is negative.

$?G$ is negative at low temperatures but becomes positive at higher temperatures.

As the temperature is increased, the equilibrium position shifts in favour of the reactants.

The reaction is exothermic.