So, I was just rearranged :delta:S to :delta:H/ :delta:S = T
I realized I could probably solve for temperature with that. eg. "heat of vaporization"
So I looked up the thermodynamic data for water and subtracted the :delta:S and :delta:H of the liquid state from the gas state. My result is close. I just would have expected it to be closer. Do you think the error is in the thermodynamic data or should I just be expecting more of an approximation with this stuff? The answer I got was 371.40K. Yes I know it's only a degree and a half off. Just curious why.
ChemBuddy | 
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Topic: Thermodynamics (Read 2410 times)