2. For a reaction at constant pressure, the standard Gibbs energies at two temperatures are: Δ_rG°(298K) = −12.0 kJ mol⁻¹, Δ_rG°(348K) = −5.0 kJ mol⁻¹. Using the Gibbs-Helmholtz equation:

what can be concluded about the sign of Δ_rH°? (assuming that ΔrH° does not depend on T)
(A) Δ_rH° = 0
(B) Δ_rH° ＞ 0 (endothermic) and Δ_rH° is around +54 kJ mol⁻¹
(C) Δ_rH° ＜ 0 (exothermic)
(D) Cannot be inferred from ΔrG°(T)
(E) Δ_rH° ＞ 0 (endothermic) and Δ_rH° is around +5.4 kJ mol⁻¹