# Problem: 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?

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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? What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.

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