There are three states of matter: solids, liquids and gases. In many cases, the same element can exist in all three states.
When matter changes from one state to another it is called a phase transition. Examples include:
- Gas to solid phase transitions are known as "deposition."
- Gas to liquid phase transitions are known as "condensation."
- Liquid to gas phase transitions are known as "vaporization."
- Liquid to solid phase transitions are known as "freezing."
- Solid to liquid phase transitions are known as "melting."
- Solid to gas phase transitions are known as "sublimation." In most cases, solids turn into gases only after an intermediate liquid state.
There are many examples of matter going through each of these transitions.
Examples of Gas to Solid (Deposition)
Under certain circumstances, gas can transform directly into a solid. This process is called deposition.
- Water vapor to ice - Water vapor transforms directly into ice without becoming a liquid, a process that often occurs on windows during the winter months.
- Physical vapor to film - Thin layers of material known as "film" are deposited onto a surface using a vaporized form of the film.
Examples of Gas to Liquid (Condensation)
- Water vapor to dew - Water vapor turns from a gas into a liquid, such as dew on the morning grass.
- Water vapor to liquid water - Water vapor fogs up glasses when moving into a warm room after being in the cold
- Water vapor to liquid water - Water vapor forms water droplets on the glass of a cold beverage.
Examples of Liquid to Gas (Vaporization)
- Water to steam - Water is vaporized when it is boiled on the stove to cook some pasta, and much of it forms into a thick steam.
- Water evaporates - Water evaporates from a puddle or a pool during a hot summer’s day.
Examples of Liquid to Solid Phase Transition (Freezing)
- Water to ice - Water becomes cold enough that it turns into ice. In fact, every known liquid (except for helium) is known to freeze in low enough temperatures.
- Liquid to crystals - Most liquids freeze by a process that is known as "crystallization," whereby the liquid forms into what is known in the scientific world as a "crystalline solid."
Examples of Solid to Liquid (Melting)
- Solid to liquid - Melting occurs when something that is solid turns back into a liquid; it is the opposite of freezing.
- Ice to water - Ice melts back into water when it is left out at temperatures above the freezing point of 32 degrees.
- Rocks to lava - Rocks in volcanoes can be heated until they are molten lava.
- Metal to molten liquid - Metals such as steel and bronze can be molten down. They can also be reformed as solids.
Examples of Solid to Gas (Sublimation)
- Dry Ice - Solid carbon dioxide is known as "dry ice" and sublimates at room temperature.
- Freeze-drying - Water can be sublimated in a food product by using a vacuum.
Now you have some examples of gas to solid and can better understand how transitions occur between different states of matter.
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Examples of Gas to Solid
By YourDictionaryThere are three states of matter: solids, liquids and gases. In many cases, the same element can exist in all three states.
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In chemistry, sublimation is the process by which a substance undergoes conversion from the solid phase to the gas phase, without going through an intermediate liquid phase. Iodine crystals and solidified carbon dioxide are examples of substances that sublimate at room temperature and regular atmospheric pressure. By contrast, at normal pressures, most chemical compounds and elements possess three different states—solid, liquid, and gas—at different temperatures. In these cases, the transition from the solid to the gaseous state requires an intermediate liquid state. The antonym (opposite process) of sublimation is called deposition. The formation of frost is an example of meteorological deposition.
Examples of sublimation
As mentioned above, carbon dioxide (CO2) is a common example of a chemical compound that sublimates at atmospheric pressure—a block of solid CO2 (dry ice) at room temperature and one atmosphere pressure will turn into gas without first becoming a liquid. Iodine is another substance that visibly sublimates at room temperature. In contrast to CO2, though, it is possible to obtain liquid iodine at atmospheric pressure by heating it.
Snow and other water ices also sublimate, although more slowly, at below-freezing temperatures. This phenomenon, used in freeze drying, allows a wet cloth to be hung outdoors in freezing weather and retrieved later in a dry state. Naphthalene, a common ingredient in mothballs, also sublimes slowly. Arsenic can also sublimate at high temperatures.
Some materials, such as zinc and cadmium, sublimate at low pressures. In high-vacuum applications, this phenomenon may be problematic.
Principles of sublimation
Sublimation is a phase transition that occurs at temperatures and pressures below what is called the "triple point" of the substance (see phase diagram). The process is an endothermic change—that is, a change in which heat is absorbed by the system. The enthalpy of sublimation can be calculated as the enthalpy of fusion plus the enthalpy of vaporization.
Sublimation is a technique used by chemists to purify compounds. Typically a solid is placed in a vessel which is then heated under vacuum. Under this reduced pressure the solid volatilizes and condenses as a purified compound on a cooled surface, leaving the non-volatile impurities behind. This cooled surface often takes the form of a "cold finger" (shown in the diagram above). Once heating ceases and the vacuum is released, the sublimed compound can be collected from the cooled surface. Usually this is done using a sublimation apparatus.
Frost-free freezers are the result of having a fan and air circulation inside the freezer. The sub-zero temperature combined with the air circulation that keeps the air arid, significantly accelerates the sublimation process. This keeps freezer walls and shelves free of ice, although ice-cubes will continually sublimate.
Dye sublimation is also often used in color printing on a variety of substrates, including paper. A small heater is used to vaporize the solid dye material, which then solidifies upon the paper. As this type of printer allows extremely fine control of the primary color ratios it is possible to obtain a good quality picture even with relatively low printer resolution, as compared to other printer types of similar resolution. Standard black and white laser printers are capable of printing on plain paper using a special "transfer toner" containing sublimation dyes which can then be permanently heat transferred to T-shirts, hats, mugs, metals, puzzles and other surfaces.
In alchemy, sublimation typically refers to the process by which a substance is heated to a vapor, then immediately collects as sediment on the upper portion and neck of the heating medium (typically a retort or alembic). It is one of the 12 core alchemical processes.
In the Fast-Freeze, Deep-Etch technique, samples (for example, tissue samples) are rapidly frozen in liquid nitrogen and transferred to a vacuum device in which surface ice is sublimed. This effectively etches the sample surface, revealing the preserved 3D structure of the hydrated material. A rotary shadowed surface replica can then be obtained via electron microscopy.
Sublimation is also used to create freeze-dried substances, for example tea, soup or drugs in a process called lyophilization, which consists of freezing a solution or suspension and heating it very slowly under medium to high vacuum—specifically, a pressure lower than the vapor pressure of the solvent at its melting point. This can be well below the melting point of water if there are organic solvents or salts in the sample being freeze-dried. The resulting solid is usually much easier to dissolve or resuspend than one that is produced from a liquid system, and the low temperatures involved cause less damage to sensitive or reactive substances.
- ↑ Note that the pressure referred to here is the vapor pressure of the substance, not the total pressure of the entire system.
- Brady, James E., and Fred Senese. Chemistry: Matter and Its Changes. Wiley, 2004. ISBN 0471215171
- Clugston, Mike. Advanced Chemistry. Oxford: Oxford University, 2000. ISBN 0199146330
- Smiley, Robert A., and Harold L. Jackson. Chemistry and the Chemical Industry: A Practical Guide for Non-Chemists, 2002. CRC Press. ISBN 1587160544
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1 Cooling water in. 2 Cooling water out. 3 Vacuum/gas line. 4 Sublimation chamber. 5 Sublimed material deposited on the cold finger. 6 Crude material. 7 External heating.