[scientific]

Question is
The equation ΔG = ΔH - TΔS tells us that an exothermic reaction will be associated with which of the following?
1. Negative ΔH
2. Positive ΔH
3. More disordered positive ΔS
4. A spontaneous reaction
5. More ordered negative ΔS

I thought it was just 1, but my answer guide says it is associated with 1, 3 and 4. However, I thought that exothermicity was determined by *only* ΔH.

I know the line of thinking is--if ΔH is negative, then I understand the ΔG spontaneous at low temp or always depending on ΔS. But I think the question is worded oddly... is there a better way to rephrase it to help me understand? Is there some guideline I'm missing? Or is there like some "general" rule that exothermic reactions "generally" spontaneous or something??

[Corribus]

I am guessing the question means exergonic, not exothermic. Strictly speaking an exothermic process/reaction refers only to the enthalpy change, not the Gibbs energy change.