If a reaction has a $\Delta$ H $\lt$ 0 and $\Delta$ S $\lt$ 0, under which conditions would the reaction be spontaneous in the forward direction?
A) low temperatures
B) high temperatures
C) high pressure
D) low pressure

Question

Quizplus · Accepted Answer

When both ΔH and ΔS are negative, a reaction is spontaneous at low temperatures. This is because the negative ΔH (exothermic reaction) becomes more significant at lower temperatures, making the Gibbs free energy (ΔG = ΔH - TΔS) negative, which indicates spontaneity.

If a Reaction Has A Δ\DeltaΔ H <\lt< 0 And Δ\DeltaΔ S <\lt< 0, Under Which Conditions Would the Reaction Be Spontaneous in \Delta

If a Reaction Has A $\Delta$ H $\lt$ 0 And $\Delta$ S $\lt$ 0, Under Which Conditions Would the Reaction Be Spontaneous in \Delta