Two reactions have similar ∆H°rxn values (∆H°rxn (1) ≈ ∆H°rxn (2)), but reaction (1) has a much smal — Thermodynamics Chemistry Question

Two reactions have similar ∆H°rxn values (∆H°rxn (1) ≈ ∆H°rxn (2)), but reaction (1) has a much smaller standard entropy change than reaction (2) (∆S°rxn (1) << ∆S°rxn (2)). At 298 K, which statements about these two reactions must be correct?
I. Reaction (1) must have a larger equilibrium constant (Keq (1) > Keq (2)).
II. Reaction (1) must have a larger Arrhenius prefactor (A(1) > A(2)).