The Values Of $\Delta$ H°_rxn And $\Delta$ S°_rxn Are Shown for the Following Equilibrium Reaction

The values of $\Delta$ H°_rxn and $\Delta$ S°_rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature?
2NO₂(g) $\leftrightarrows$ N₂O₄(g) $\Delta$ H $\degree$ = -58.02 kJ/mol, $\Delta$ S°=-176.5 J/mol .K

A) The negative value of $\Delta$ H $\degree$ is dominant at all temperatures.
B) The negative value of $\Delta$ S° is dominant at all temperatures.
C) The negative value of $\Delta$ S° is combined with the small value of T.
D) The negative value of $\Delta$ 0H $\degree$ is combined with the small value of T.