Silver oxide decomposes on heating: 2 Ag₂O(s) → 4 Ag(s) + O₂(g). The standard enthalpy of formation of Ag₂O(s) is -31.05 kJ mol⁻¹. The standard molar entropies are Ag(s) 42.55, O₂(g) 205.1 and Ag₂O(s) 121.3 J K⁻¹ mol⁻¹. Taking Δ H° and Δ S° as constant, above what temperature is the decomposition spontaneous under standard conditions?

ChemistryMediumHigh School (11–12)Chemical Thermodynamics › Entropy, Gibbs Energy and Spontaneity JEE Main

Silver oxide decomposes on heating: $2\,\text{Ag}_2\text{O}(s) \rightarrow 4\,\text{Ag}(s) + \text{O}_2(g)$ . The standard enthalpy of formation of $\text{Ag}_2\text{O}(s)$ is $-31.05\ \text{kJ mol}^{-1}$ . The standard molar entropies are $\text{Ag}(s)$ $42.55$ , $\text{O}_2(g)$ $205.1$ and $\text{Ag}_2\text{O}(s)$ $121.3\ \text{J K}^{-1}\ \text{mol}^{-1}$ . Taking $\Delta H^\circ$ and $\Delta S^\circ$ as constant, above what temperature is the decomposition spontaneous under standard conditions?

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← A rigid, insulated flask of volume 4.0 L holds 0.50 mol of an ideal gas at 300 K. It is joined by a tap to a second rigid, insulated flask of volume 6.0 L that is empty. The tap is opened and the gas spreads through both flasks. Which statement about this change is correct? (w is the work done on the gas; take R = 8.314 J K⁻¹ mol⁻¹.)A student pours 60.0 mL of 1.50 M nitric acid into 140.0 mL of 0.500 M potassium hydroxide solution in an insulated cup with a lid. Both start at the same temperature, and the mixture warms by 4.54 K. The cup itself takes up 48 J for each kelvin. The solutions have a density of 1.00 g mL⁻¹ and a specific heat of 4.18 J g⁻¹ K⁻¹. What is the size of the enthalpy of neutralisation, in kJ mol⁻¹ of water formed, to the nearest integer? →

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