For the reaction 2SO₂(g)+ O₂(g)→ 2SO₃(g),ΔH° and ΔS° are both negative at 298 K,and the process is spontaneous at 298 K.Which of the following statements must also be true? A)The change in entropy is the driving force of the reaction. B)ΔG is positive for the reaction at 298 K. C)The direction of the reaction may be reversed at high temperatures. D)ΔG is temperature independent. E)At high temperature,ΔH becomes positive.

Question

Quizplus · Accepted Answer

If both ΔH° and ΔS° are negative, the reaction is spontaneous only at low temperatures. At high temperatures, the entropy term, TΔS°, may become larger than the enthalpy term, ΔH°, making ΔG° positive, meaning the reaction will not be spontaneous in the forward direction. Therefore, the direction of the reaction may be reversed at high temperatures, and statement C must be true.

For the Reaction 2SO2(g)+ O2(g)→ 2SO3(g),ΔH° and ΔS° Are Both

For the Reaction 2SO₂(g)+ O₂(g)→ 2SO₃(g),ΔH° and ΔS° Are Both