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11.11: Phase Transitions: Sublimation and Deposition

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Phase Transitions: Sublimation and Deposition

11.11: Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes and a vivid purple vapor forms. The reverse of sublimation is called deposition, a process in which gaseous substances condense directly in the solid-state, bypassing the liquid state. The formation of frost is an example of deposition.

Like vaporization, the process of sublimation requires an input of energy to overcome intermolecular attractions. Sublimation is, therefore, an endothermic phase transition. The enthalpy of sublimation, ΔHsub, is the energy required to convert one mole of a substance from the solid to the gaseous state. For example, the sublimation of carbon dioxide is represented by:


Likewise, the enthalpy change for the reverse process of deposition is equal in magnitude but opposite in sign to that for sublimation. Because deposition involves the formation of intermolecular forces, it is an exothermic phase transition.


Consider the extent to which intermolecular attractions must be overcome to achieve a given phase transition. Converting a solid into a liquid requires that these attractions be only partially overcome; transition to the gaseous state requires that they be completely overcome. As a result, the enthalpy of fusion for a substance is less than its enthalpy of vaporization. This same logic can be used to derive an approximate relation between the enthalpies of all phase changes for a given substance. Though not an entirely accurate description, sublimation may be conveniently modeled as a sequential two-step process of melting followed by vaporization in order to apply Hess’s Law. Viewed in this manner, the enthalpy of sublimation for a substance may be estimated as the sum of its enthalpies of fusion and vaporization.


This text is adapted from Openstax, Chemistry 2e, Section 10.3: Phase Transitions.


Phase Transitions Sublimation Deposition Ice Melting Dry Ice Gas Phase Solid To Gas Transition Intermolecular Forces Dispersion Forces Sublimation Point Molar Heat Of Sublimation Molar Enthalpy Of Sublimation Endothermic Process Vapor To Solid Transition Exothermic Phase Change

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