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III. Calculate the change in free energy if 0.335 moles of NaI is dissolved in water at 25.0°C

III. Calculate the change in free energy if 0.335 moles of NaI is dissolved in water at 25.0°C

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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III. Calculate the change in free energy if 0.335 moles of NaI is dissolved in water at 25.0°C
10. Consider the dissolution of NaBr and Nal. The values provided here will be helpful for answering the following questions. | ΔΗ AS + soln (kJ/mol) soln mol-K NaBr -0.060 57.0 Nal -7.50 74.0 I. Write a balanced equilibrium equation for the dissolution of Nal in water. Include phases. II. Which of the following explains why the entropy change is greater for the dissolution of Nal compared to the dissolution of NaBr? A. The cation forms stronger ion-dipole networks with water in NaBr than Nal because of the weaker bond to Br. B. The interactions between bromide ions with other bromide ions is stronger than the interactions between iodide ions with other iodide ions. C. The more negative change in enthalpy observed with Nal implies greater dissociation and hence greater entropy. D. lodide has weaker ion-dipole interactions with water than bromide. E. The bromide ion has more negative charge than the iodide ion. Therefore, because of the greater charge, it forms a stronger ion-dipole network with water. III. Calculate the change in free energy if 0.335 moles of Nal is dissolved in water at 25.0°C. What is the dissolution of 1.00 mol of NaBr at 298.15 K? IV.
Transcribed Image Text:10. Consider the dissolution of NaBr and Nal. The values provided here will be helpful for answering the following questions. | ΔΗ AS + soln (kJ/mol) soln mol-K NaBr -0.060 57.0 Nal -7.50 74.0 I. Write a balanced equilibrium equation for the dissolution of Nal in water. Include phases. II. Which of the following explains why the entropy change is greater for the dissolution of Nal compared to the dissolution of NaBr? A. The cation forms stronger ion-dipole networks with water in NaBr than Nal because of the weaker bond to Br. B. The interactions between bromide ions with other bromide ions is stronger than the interactions between iodide ions with other iodide ions. C. The more negative change in enthalpy observed with Nal implies greater dissociation and hence greater entropy. D. lodide has weaker ion-dipole interactions with water than bromide. E. The bromide ion has more negative charge than the iodide ion. Therefore, because of the greater charge, it forms a stronger ion-dipole network with water. III. Calculate the change in free energy if 0.335 moles of Nal is dissolved in water at 25.0°C. What is the dissolution of 1.00 mol of NaBr at 298.15 K? IV.
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