The Values of and are Shown

Multiple Choice

The values of and are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? H  58.02 kJ/mol, S 176.5 J/mol  K

A) The negative value of H  is dominant at all temperatures.
B) The negative value of S  is dominant at all temperatures.
C) The negative value of S  is combined with the small value of T.
D) The negative value of H  is combined with the small value of T.