Sublimation (phase transition): Difference between revisions

Revision as of 12:28, 5 January 2021

Revision as of 12:31, 5 January 2021

Line 11:

Sublimation is caused by the absorption of heat which provides enough energy for some molecules to overcome the [[intermolecular force|attractive forces]] of their neighbors and escape into the vapor phase. Since the process requires additional energy, it is an [[endothermic]] change. The [[enthalpy of sublimation]] (also called heat of sublimation) can be calculated by adding the [[enthalpy of fusion]] and the [[enthalpy of vaporization]].

{{Table of Phase Transitions}}

[[File:Comparison carbon dioxide water phase diagrams.svg|thumb|upright=2|Comparison of phase diagrams of carbon dioxide (red) and water (blue) showing the carbon dioxide sublimation point (middle-left) at 1 atmosphere. As dry ice is heated, it crosses this point along the bold horizontal line from the solid phase directly into the gaseous phase. Water, on the other hand, passes through a liquid phase at 1 atmosphere.]]

Line 120:

*[[Freezer burn]] – common process involving sublimation

*[[Phase diagram]]

==Table==

{{Table of phase transitions}}

{{Clear}}

Line 134:

{{States of matter}}

[[Category: Alchemical processes]]

[[Category: Atmospheric thermodynamics]]

[[Category: Chemical processes]]

[[Category: Gases]]

[[Category: Laboratory techniques]]

[[Category: Phase transitions]]

[[Category:Separation processes]]