🤓 Based on our data, we think this question is relevant for Professor Evans' class at QC CUNY .

**Solution**: A. Using the thermodynamic data provided for dissolving Na 2SO4(s) in water, that is, for the chemical process
Na2SO4(s) → 2Na+(aq) + SO42-(aq) Calculate ΔH°.
B. When I calculated ΔS°, I got -11.84 J/K•mol. Using this value and your answer to part A, calculate ΔG° at 25°C.
C. Which term is responsible for the temperature dependence of ΔG: enthalpy (ΔH°), entropy (ΔS°), both, or neither (ΔG is not temperature dependent)?
Will increasing the temperature make ΔG larger (more positive), smaller (more negative), or have no effect?
D. So based on your answer to part C, will the solubility of Na 2SO4 increase or decrease with increasing temperature?