For the reaction 2SO₃(g)$\rightarrow$2SO₂(g)+ O₂(g) $\Delta$H_r^$\omicron$= +198 J.K^-¹.mol^-¹ at 298 K.Which statement is true for this reaction? A) The reaction is driven by the enthalpy. B) The reaction will not be spontaneous at low temperatures. C) $\Delta$G_r^$\omicron$will be negative at high temperatures. D) The reaction will not be spontaneous at any temperature. E) $\Delta$G_r^$\omicron$will be positive at high temperatures.

Question

Quizplus · Accepted Answer

EThe reaction has a positive $\Delta H$, indicating it absorbs heat. According to the Gibbs free energy equation $\Delta G = \Delta H - T\Delta S$, a positive $\Delta H$ can lead to a negative $\Delta G$ (spontaneous reaction) if the temperature is high enough to make the $T\Delta S$ term dominant. Thus, at high temperatures, the reaction may become spontaneous ($\Delta G$ becomes negative), which is stated in option C. Conversely, if $\Delta G$ is negative at high temperatures, it implies that at high temperatures, the entropy contribution ($T\Delta S$) can overcome the positive enthalpy, making $\Delta G$ positive at lower temperatures, as indicated in option E.

For the Reaction 2SO3(g) →\rightarrow→ 2SO2(g)+ O2(g) Δ\DeltaΔ Hr ο\omicronο = +198 J Δ\DeltaΔ

For the Reaction
2SO₃(g) $\rightarrow$ 2SO₂(g)+ O₂(g) $\Delta$ H_r^$\omicron$= +198 J $\Delta$