How Does ΔH Change with Temperature for Water to Vapor Conversion?

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The discussion centers around the enthalpy changes associated with the phase transitions of water. It highlights that the formation of water vapor at standard state releases -241 KJ/mol, while liquid water formation releases -284 KJ/mol. A key point raised is the energy required to convert liquid water at 25°C to vapor, which is 44 KJ/mol. The inquiry focuses on whether this energy requirement changes with temperature and seeks a formula for the variation of enthalpy change (ΔH) with temperature. The conversation suggests a need for understanding the relationship between temperature and enthalpy in phase changes.
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So when they said that to produce water vapor at standard state it releases -241 KJ/mol
and liquid water -284 KJ/mol

You can't create water vapor at standard temperature but I assume they used Hess' law
Anyway, my question is when you change from water to vapor you need 44KJ/mol

So that would be the energy required to change from 25 C liquid to 25 C vapor.
Does it change for example when you want to change it from another temperature?
 
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Yes. Do you know a formula for the variation of ΔH with temperature?
 

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