∆Hvap
Definition
∆Hvap refers to the heat of vaporization, which is the amount of energy required to convert one gram of a substance from its liquid phase to its gaseous phase at constant temperature and pressure.
Analogy
Think of ∆Hvap as the energy needed for water molecules to break free from their liquid state and become independent gas molecules, just like a group of friends breaking apart and going their separate ways.
Related terms
Boiling Point: The temperature at which a substance changes from its liquid phase to its gaseous phase at atmospheric pressure.
Condensation: The process in which a substance changes from its gaseous phase to its liquid phase, releasing heat in the process.
Evaporation: The process in which a substance changes from its liquid phase to its gaseous phase at temperatures below its boiling point, without reaching boiling point.
"∆Hvap" appears in:
Practice Questions (3)
How much energy does it take to convert 36 g liquid water to water vapor given the following data about water? ∆Hfus = 334 J/g, ∆Hvap = 2260 J/g
Find energy needed to convert 36 g ice to water vapor given the following data about water: ∆Hfus = 334 J/g, ∆Hvap = 2260 J/g.
Given the following data about gold: ∆Hfus = 13.2 kJ/mol, ∆Hvap = 310.9 kJ/mol, what would be the enthalpy change when gold transitions from a liquid to a solid phase?
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