Answer: The following data compare the standard enthalpies

Chapter , Problem 113IE

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The following data compare the standard enthalpies and free energies of formation of some crystalline ionic substances and aqueous solutions of the substances:

Write the formation reaction for \(\mathrm{AgNO}_{3}(s)\). Based on this reaction, do you expect the entropy of the system to increase or decrease upon the formation of \(\mathrm{AgNO}_{3}(s)\)? (b) Use \(\Delta H_{f}^{0}\) and \(\Delta G_{f}^{0}\) of \(\mathrm{AgNO}_{3}(s)\) to determine the entropy change upon formation of the substance. Is your answer consistent with your reasoning in part (a)? (c) Is dissolving \(\mathrm{AgNO}_{3}(s)\) in water an exothermic or endothermic process? What about dissolving \(\mathrm{MgSO}_{4}\) in water? (d) For both \(\mathrm{AgNO}_{3}(s)\) and \(\mathrm{MgSO}_{4}\), use the data to calculate the entropy change when the solid is dissolved in water. (e) Discuss the results from part (d) with reference to material presented in this chapter and in the “A Closer Look” box on page 820.

Equation transcription:

Text transcription:

{AgNO}_{3}(s)

\Delta H_{f}^{0}

\Delta G_{f}^{0}

{MgSO}_{4}