In which case must a reaction be spontaneous at all temperatures?

Question

Quizplus · Accepted Answer

For a reaction to be spontaneous at all temperatures, the Gibbs free energy change (ΔG) must be negative at all temperatures. ΔG can be calculated using the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, T is the temperature in Kelvin, and ΔS is the entropy change. 
In choice D, (ΔH) is negative and (ΔS) is positive, which means that at high temperatures, the TΔS term can balance out the negative ΔH term to yield a negative ΔG value. This reaction is therefore spontaneous at all temperatures.

In Which Case Must a Reaction Be Spontaneous at All Δ\DeltaΔ

In Which Case Must a Reaction Be Spontaneous at All $\Delta$