6 In class, we showed how the melting of water is a spontaneous process above the melting point and below the melting point it is a nonspontaneous process. This question asks you to carry out a similar analysis for boiling point water which is 373 K. H₂O(1) → H₂O(g) Using the Gibbs Free energy equation AG = AH-TAS, show that boiling water a. b. at 1 atm is nonspontaneous at 95 °C (368 K). i. Note 1. Temperature needs the be converted to K. ii. Note 2. For AH, use AHvap = +40.8 kJ/mol or 40800 J/mol Note 3. ASvap = 109.1 J/K* mol iii. Show that the boiling water is spontaneous at 105 °C (378 K).

6 In class, we showed how the melting of water is a spontaneous process above the melting point and below the melting point it is a nonspontaneous process. This question asks you to carry out a similar analysis for boiling point water which is 373 K. H₂O(1) → H₂O(g) Using the Gibbs Free energy equation AG = AH-TAS, show that boiling water a. b. at 1 atm is nonspontaneous at 95 °C (368 K). i. Note 1. Temperature needs the be converted to K. ii. Note 2. For AH, use AHvap = +40.8 kJ/mol or 40800 J/mol Note 3. ASvap = 109.1 J/K* mol iii. Show that the boiling water is spontaneous at 105 °C (378 K).

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 2RQ: What is the second law of thermodynamics? For any process, there are four possible sign combinations...

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