AP Chemistry
9.6 Free Energy of Dissolution
9.5 Free Energy and Equilibrium
9.3 Gibbs Free Energy and Thermodynamic Favorability
9.2 Absolute Entropy and Entropy Change
A student investigates the dissolution equilibrium of lithium sulfate in water:
\[ \text{Li}_2\text{SO}_4(s) \rightleftharpoons 2\,\text{Li}^+(aq) + \text{SO}_4^{2-}(aq) \]
Thermodynamic data at \(298\text{ K}\) are provided in the table below.
Which of the following correctly predicts and explains the effect of increasing temperature on the solubility of \(\text{Li}_2\text{SO}_4(s)\) in water?
\[ \text{Li}_2\text{SO}_4(s) \rightleftharpoons 2\,\text{Li}^+(aq) + \text{SO}_4^{2-}(aq) \]
Thermodynamic data at \(298\text{ K}\) are provided in the table below.
| Substance | \(\Delta H_f^\circ\text{ (kJ/mol)}\) | \(S^\circ\text{ (J/(mol}\cdot\text{K))}\) |
|---|---|---|
| \(\text{Li}_2\text{SO}_4(s)\) | \(-1436\) | \(114\) |
| \(\text{Li}^+(aq)\) | \(-278\) | \(13\) |
| \(\text{SO}_4^{2-}(aq)\) | \(-909\) | \(20\) |
Which of the following correctly predicts and explains the effect of increasing temperature on the solubility of \(\text{Li}_2\text{SO}_4(s)\) in water?
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