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

The values of $\Delta$ H $\degree$ _rxn and $\Delta$ S $\degree$ _rxn are shown for the following equilibrium reaction.What makes the equilibrium constant larger at lower temperatures? 2 NO₂ (g) ⇄ N₂ O₄ (g) $\Delta$ H $\degree$ = -58.02 kJ/mol, $\Delta$ S $\degree$ = -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 $\degree$ is dominant at all temperatures.
C) The negative value of $\Delta$ S $\degree$ is combined with the small value of T.
D) The negative value of $\Delta$ H $\degree$ is combined with the small value of T.