For the reaction 4Ag(s)+ O₂(g)→ 2Ag₂O(s),ΔH° = -61.14 kJ and ΔS° = -132 J/K at 25°C.Which of the following statements is true? Assume that ΔH° and ΔS° are essentially temperature independent. A)The change in entropy is the driving force at low temperatures. B)The reaction will be spontaneous at high temperatures,and the reverse reaction will be spontaneous at low temperatures. C)The reaction will not be spontaneous at any temperature. D)The reaction will be spontaneous at low temperatures,and the reverse reaction will be spontaneous at high temperatures. E)The reaction will be spontaneous at all temperatures.

Question

Quizplus · Accepted Answer

To determine if the reaction is spontaneous, we can use the Gibbs free energy equation: ΔG° = ΔH° - TΔS°. 
At low temperatures, the ΔH° term dominates and favors the reactants. At high temperatures, the TΔS° term dominates and favors the products. 
Since ΔH° is negative and ΔS° is also negative, the reaction will be spontaneous at low temperatures where the entropy term is favored. At high temperatures, the reaction will not be spontaneous and the reverse reaction will be spontaneous. Therefore, choice D is correct.

For the Reaction 4Ag(s)+ O2(g)→ 2Ag2O(s),ΔH° = -61

For the Reaction 4Ag(s)+ O₂(g)→ 2Ag₂O(s),ΔH° = -61