Chemistry: Heat of Sublimation and Hydrogem Bonds Problem

AI Thread Summary
The discussion focuses on calculating the change in enthalpy for the sublimation of water, with a reported value of 46.7 kJ/mol. Participants seek clarification on the ΔH value from Exercise 24, which is identified as -21 kJ/mol. There is confusion regarding the relationship between intermolecular forces in ice and hydrogen bonding, with requests for guidance on estimating the contribution of hydrogen bonds to these forces. The conversation highlights the need for a deeper understanding of the thermodynamic principles involved in phase changes and intermolecular interactions. Overall, the thread emphasizes the complexities of calculating enthalpy changes and the role of hydrogen bonding in ice.
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Homework Statement


Using the heats of fusion and vaporization for water, calculate the change in enthalpy for the sublimation of water:

H2O(s) --> H2O(g

Using the delta H value given in Exercise 24 and the number of hydrogen bonds formed to each water molecule, estimate what portion of the intermolecular forces in ice can be accounted for by hydrogen bonding.

Homework Equations

The Attempt at a Solution


I have already figured out the first portion of the problem, finding the change in enthalpy of sublimation ( I got 46.7 kJ/mol ), but I'm really not sure as to how to attack the portion of IMF and hydrogen bonding. Any help is greatly appreciated.
 
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And what was the ΔH value given in the exercise 24? ΔH of what?
 
Borek said:
And what was the ΔH value given in the exercise 24? ΔH of what?
I believe it's -21 kJ/mol
 
ΔH of what?
 
Borek said:
ΔH of what?
of the reaction H20 (g) + HOH (g) -> H2O --- HOH (in ice)
 
What is ΔH of the desublimation?
 

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