Assuming ΔH and ΔS are constant with respect to temperature,under what conditions will a chemical reaction be spontaneous at all temperatures?
A)ΔH is negative,and ΔS is positive.
B)ΔH is positive,and ΔS is negative.
C)ΔS = 0,and ΔH is positive.
D)ΔH = 0,and ΔS is negative.
E)none of these

Question

Quizplus · Accepted Answer

According to the Gibbs free energy equation, ΔG = ΔH - TΔS. For a reaction to be spontaneous at all temperatures, ΔG must be negative at all temperatures. This can only occur if ΔH is negative (exothermic reaction) and ΔS is positive (increased entropy).

Assuming ΔH and ΔS Are Constant with Respect to Temperature,under