Question

The direct transition from a solid to a gas may occur through which of the following processes?

a. a solid transitions in a liquid
-This happens when the internal energy of the solid increases (usually due to the application of heat or pressure), which in turn increases the substance's temperature up to the melting point.

b. equilibrium curve.
-The most common is the liquid-vapor critical point, where you cannot tell the difference between the liquid and gaseous phases.

c. releases energy
-An example of deposition is the formation of frost. In cold temperatures, water vapor undergoes deposition to form a thin layer of solid ice on plants and grass.

d. Sublimation
-Through sublimation, a substance changes from a solid to a gas without ever passing through a liquid phase. Dry ice, solid CO2, provides a common example of sublimation.

Answer 1

The direct transition from a solid to a gas is called sublimation, exemplified by dry ice turning into gas without becoming liquid, whereas the reverse process is deposition, such as frost forming on cold surfaces.

Step-by-step explanation:

The direct transition from a solid to a gas is known as sublimation. This process occurs when a solid changes into a gaseous state without passing through the liquid phase. For example, dry ice, which is solid carbon dioxide (CO2), sublimes at room temperature and standard pressure, demonstrating this phenomenon. The visible fog is actually water droplets formed by the cooling effect of the dry ice. Another example is the sublimation of snow and ice at temperatures below their melting point, which can be sped up by wind and lower atmospheric pressure at high altitudes. Conversely, the reverse process, where a gas transitions directly into a solid, is called deposition, with the formation of frost as a familiar instance. These phase changes are part of physical transformations that either absorb energy (endothermic) or release energy (exothermic).