Free Energy of Dissolution Practice Test

A salt dissolves in water according to: $\text{MX}(s) \rightarrow \text{M}^+(aq)+\text{X}^-(aq)$. For this dissolution, $\Delta H_{\text{soln}}<0$ and $\Delta S_{\text{soln}}>0$. Under which conditions is the dissolution thermodynamically favored (i.e., $\Delta G<0$)?

A student dissolves solid $\text{NH}4\text{NO}3$ in water at $25^\circ\text{C}$. The solution becomes noticeably colder (so $\Delta H{\text{soln}} > 0$), and the ions disperse throughout the solvent (so $\Delta S{\text{soln}} > 0$). Under these conditions, is the dissolution thermodynamically favored?