SolidVapor

Solidvapor is not a standard term in established science literature. When used, it typically refers to aspects of the solid–vapor boundary, especially sublimation, the direct transition of a solid to a gas, or the vapor phase produced when a solid material sublimates. In phase diagrams, the behavior of solids at elevated temperatures and low pressures is described by sublimation lines and the associated vapor pressures.

Sublimation occurs when a solid’s vapor pressure becomes sufficient to enable gas formation at a given temperature and pressure. The rate of sublimation depends on temperature, surface area, and the material’s latent heat of sublimation. Solids with relatively high vapor pressures or lower sublimation temperatures sublimate more readily; examples include dry ice (solid carbon dioxide), which sublimates at room temperature, and solid iodine, which sublimates upon heating to form iodine vapor.

Applications and related phenomena associated with the solid–vapor boundary include sublimation purification, where impurities are left behind as a pure solid while the desired compound sublimes and recondenses elsewhere, and certain coating or deposition techniques that rely on sublimation of a solid phase to form a thin film. In many practical contexts, the concept is discussed using vapor pressures, sublimation rates, and the latent heat of sublimation rather than under the umbrella term “solidvapor.”

Measurement and theory involve vapor pressure–temperature relationships for solids, often described by Clausius–Clapeyron-type relations or empirical correlations to estimate the sublimation curve and the latent heat of sublimation. At ambient conditions, most solids have very low vapor pressures, making sublimation negligible unless temperature is increased or pressure is reduced.