The reaction 4 Ag(s)+ O₂(g)→ 2 Ag₂O(s)favors Ag₂O at low temperature,but it favors Ag and O₂ at high temperatures.How can this be explained in terms of ΔH and ΔS?

Question

Quizplus · Accepted Answer

The reaction is exothermic (ΔH is negative) and results in a decrease in entropy (ΔS is negative) because it goes from more moles of gas to fewer moles of solid. At low temperatures, the negative ΔH dominates, favoring the formation of Ag₂O. At high temperatures, the negative ΔS becomes more significant, favoring the reactants Ag and O₂.

The Reaction 4 Ag(s)+ O2(g)→ 2 Ag2O(s)favors Ag2O at Low

The Reaction 4 Ag(s)+ O₂(g)→ 2 Ag₂O(s)favors Ag₂O at Low