Consider the dissolution of NaBr and NaI. The values provided here will be helpful for answering the following questions. ΔH∘solnΔHsoln∘ (kJ/mol) ΔS∘solnΔSsoln∘ Jmol•KNaBr –0.860 57.0NaI –7.50 74.0 Write a balanced equilibrium equation for the dissolution of NaI in water. Include phases. Which of the following explains why the entropy change is greater for the dissolution of NaI compared to the dissolution of NaBr?Choose one: A. The interactions between bromide ions with other bromide ions is stronger than the interactions between iodide ions with other iodide ions. B. The cation forms stronger ion-dipole networks with water in NaBr than NaI because of the weaker bond to Br.C. The more negative change in enthalpy observed with NaI implies greater dissociation and hence greater entropy.D. Iodide has weaker ion-dipole interactions with water than bromide. E. The bromide ion has a more negative charge than the iodide ion. Therefore, because of the greater charge, it forms a stronger ion-dipole network with water. Calculate the change in free energy if 1.02 moles of NaI is dissolved in water at 25.0°C. kJ What is the dissolution of 1.00 mol of NaBr at 298.15 K?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 92QRT

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Consider the dissolution of NaBr and NaI. The values provided here will be helpful for answering the following questions.

ΔH∘solnΔHsoln∘ (kJ/mol) ΔS∘solnΔSsoln∘ Jmol•K

NaBr –0.860 57.0

NaI –7.50 74.0

Write a balanced equilibrium equation for the dissolution of NaI in water. Include phases.

Which of the following explains why the entropy change is greater for the dissolution of NaI compared to the dissolution of NaBr?

Choose one: A. The interactions between bromide ions with other bromide ions is stronger than the interactions between iodide ions with other iodide ions. B. The cation forms stronger ion-dipole networks with water in NaBr than NaI because of the weaker bond to Br.C. The more negative change in enthalpy observed with NaI implies greater dissociation and hence greater entropy.D. Iodide has weaker ion-dipole interactions with water than bromide. E. The bromide ion has a more negative charge than the iodide ion. Therefore, because of the greater charge, it forms a stronger ion-dipole network with water.

Calculate the change in free energy if 1.02 moles of NaI is dissolved in water at 25.0°C.

kJ

What is the dissolution of 1.00 mol of NaBr at 298.15 K?

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