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4. What is the expected value for the heat of sublimation of acetic acid if its heat of fusion is 10.8 kJ/mol and its heat of vaporization is 24.3 kJ/mol?

4. What is the expected value for the heat of sublimation of acetic acid if its heat of fusion is 10.8 kJ/mol and its heat of vaporization is 24.3 kJ/mol?

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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**Question 4:** What is the expected value for the heat of sublimation of acetic acid if its heat of fusion is 10.8 kJ/mol and its heat of vaporization is 24.3 kJ/mol? --- **Explanation:** In thermodynamics, the heat of sublimation is the sum of the heat of fusion and the heat of vaporization. Given the values: - Heat of fusion = 10.8 kJ/mol - Heat of vaporization = 24.3 kJ/mol The heat of sublimation can be calculated as follows: \[ \text{Heat of sublimation} = \text{Heat of fusion} + \text{Heat of vaporization} = 10.8 \, \text{kJ/mol} + 24.3 \, \text{kJ/mol} = 35.1 \, \text{kJ/mol} \] Therefore, the expected value for the heat of sublimation of acetic acid is 35.1 kJ/mol.
Transcribed Image Text:**Question 4:** What is the expected value for the heat of sublimation of acetic acid if its heat of fusion is 10.8 kJ/mol and its heat of vaporization is 24.3 kJ/mol? --- **Explanation:** In thermodynamics, the heat of sublimation is the sum of the heat of fusion and the heat of vaporization. Given the values: - Heat of fusion = 10.8 kJ/mol - Heat of vaporization = 24.3 kJ/mol The heat of sublimation can be calculated as follows: \[ \text{Heat of sublimation} = \text{Heat of fusion} + \text{Heat of vaporization} = 10.8 \, \text{kJ/mol} + 24.3 \, \text{kJ/mol} = 35.1 \, \text{kJ/mol} \] Therefore, the expected value for the heat of sublimation of acetic acid is 35.1 kJ/mol.
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