The correct thermodynamic conditions for the spontaneous reaction at all temperatures is:

Solution & Explanation

\textbf{Answer:} (C) $\Delta H<0$ and $\Delta S>0$ \textbf{Solution:} Gibbs energy change: $\Delta G=\Delta H-T\Delta S$. For a reaction to be spontaneous at all temperatures, $\Delta G$ must be negative for every value of $T$. This requires $\Delta H<0$ (so the enthalpy term is negative) and $\Delta S>0$ (so $-T\Delta S$ is also negative at every temperature). With both contributions negative, $\Delta G<0$ regardless of $T$.