The ΔH and ΔS for 2Ag2O(s) → 4Ag(s) + O2(g) are + 61.17 kJ mol-

1.	The ΔH and ΔS for 2Ag2O(s) → 4Ag(s) + O2(g) are + 61.17 kJ mol-1 and +132 JK-1 mol-1 respectively. Above what temperature will the reaction be spontaneous?
Answer» The reaction 2Ag₂O(s) → 4Ag(s) + O₂(g) will be spontaneous when ΔG is negative. Since ΔH is +ve and ΔS is also +ve, the reaction ΔG = ΔH - TΔS suggests that ΔG would be negative when ΔH = TΔS < 0 or T > \(\frac{\Delta H}{\Delta S}\) = \(\frac{61170 mol^{-1}}{132 JK^{-1}mol^{-1}}\) = 463.4 K The given reaction will be spontaneous above a temperature of 463.4 K.

The ΔH and ΔS for 2Ag2O(s) → 4Ag(s) + O2(g) are + 61.17 kJ mol-1 and +132 JK-1 mol-1 respectively. Above what temperature will the reaction be spontaneous?

Answer»

The reaction 2Ag₂O(s) → 4Ag(s) + O₂(g) will be spontaneous when ΔG is negative. Since ΔH is +ve and ΔS is also +ve, the reaction ΔG = ΔH - TΔS suggests that ΔG would be negative when

ΔH = TΔS < 0

or T > \(\frac{\Delta H}{\Delta S}\) = \(\frac{61170 mol^{-1}}{132 JK^{-1}mol^{-1}}\) = 463.4 K

The given reaction will be spontaneous above a temperature of 463.4 K.

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The ΔH and ΔS for 2Ag2O(s) → 4Ag(s) + O2(g) are + 61.17 kJ mol-1 and +132 JK-1 mol-1 respectively. Above what temperature will the reaction be spontaneous?

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