From a pearson chemistry textbook I am studying, the boiling point and Hvap of both water and isopropanol is detailed. How is the Hvap of isopropanol so similar to water, yet has a lower boiling point? I read that as intermolecular forces are increased, so does the boiling point. Wouldn’t the same be true for the Hvap?
|Chemical|Boiling point Celsius|Hvap (Boiling Point)|Hvap (25C)|
|:-|:-|:-|:-|
|Water|100|40.7|44|
|Isopropanol|82.3|39.9|45.4|
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Because your reference is KJ/Mol. Isopropanol has a higher molar mass. when you evaporate 1 Mol of isopropanol you evaporate 60g and for 1 Mol water you evaporate only 18g.
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