Matter which has been pushed to temperatures and pressures beyond those of its critical point. This stage is characterized by the inability to distinguish whether the matter is a liquid or a gas, as a result, Supercritical fluids do not have a definite phase. Denoted as SCF. The following images represent the difference in densities between the phases and supercritical fluids.
In 1822 Baron Charles Cagniard de la Tour discovered supercritical fluids while conducting experiments involving the discontinuities of the sound of a flint ball in a sealed cannon barrel filled with various fluids at various temperatures ("Charles Cagniard de la Tour").
Notice the yellow and blue mix to create green area that follows the Coordinates of the critical point, that is where the supercritical fluids occur on the graph. Each element and molecule have unique critical points. The arrow shows how it is possible to go from a vapor to a liquid by using supercritical fluids, pressure and temperature. Notice how when pressure and temperature on a gas are increased into the supercritical range, and the temperature is lowered, the substance moves into the liquid phase.
A Chart of Common or Interesting Critical Points:
|Liquid||Critical Temperature (K)||Critical Pressure (atm)|
|Carbon Dioxide (CO2)||305||72.9|
Supercritical fluids can occur in nature. For example, in places like underwater volcanoes, specifically those located deep beneath the ocean's surface, supercritical water is formed because of the immense pressure due to the depth and the intense heat from the vents of the volcano. This water can lead to the formation of crystals used in some jewelry (Benner 680).
The atmospheric pressure of Venus is approximately 90 times greater than that of the Earth, with an average temperature of 467 degrees Celsius, and about 97% of its atmosphere is Carbon Dioxide. Therefore it would be reasonable to consider the atmosphere of Venus a supercritical fluid because both the pressure and temperature exceed that of Carbon Dioxide's critical point however this theory has not been proven. Examples similar to this one can be found throughout the solar system, particularly in the Gas Giants (Benner 680).
Supercritical fluids are useful in science today for purposes ranging from the extraction of floral fragrance from flowers and the process of creating decaffeinated coffee, to applications in food science and functional food ingredients, pharmaceuticals, cosmetics, polymers, powders, bio- and functional materials, nano-systems, natural products, biotechnology, fossil and biofuels, microelectronics and environment (Bottini 133). If you wish to read more into the different activities and breakthroughs concerning Supercritical Fluids many articles on research and more can be found at ScienceDirect.com.
Extraction using Supercritical Fluids is a fairly simple concept, and much more efficient than normal extraction methods, which require both heating and ventilation of the solution to the atmosphere. Supercritical fluids allow continuous extraction using common, inexpensive, and more importantly non-toxic materials, and only requires venting to separate the solvent from the material being removed. The extraction involves applying the supercritical solvent to whatever material is being eradicated, for example, coffee beans which are being decaffeinated, and allowing the solvent to remove the substance being extracted. Returning to the coffee bean example, supercritical CO2 would be applied to the beans, then when it had extracted the caffeine, the CO2 would be put through carbon filters, which would separate the caffeine from the solvent which can then be removed simply by venting because of its unique properties and similarities to vapor. Likewise, supercritical fluids can be used as solvents to apply substances like dyes to clothing, the process for this is more or less the reverse of extraction. The most commonly used solvents are supercritical Carbon Dioxide and Water because of their availability and low critical temperatures (Hardy).
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