凍結と超冷却を組み合わせたアイソコリックプロセス
Cristina Bilbao-Sainz1, Boris Rubinsky2
1U.S. Department of Agriculture, Western Regional Research Center, 800 Buchanan St., Albany, CA, 94710, USA. cristina.bilbao@usda.gov.
NPJ science of food
|August 23, 2025
まとめ
この研究は,超冷却保存のための多相イソコア系を導入し,氷核化のリスクを軽減します. 生物学的物質の低温貯蔵を可能にするため,凍結水からの圧力変化を使用しています.
科学分野:
- 熱力学について
- 生物保存
- 材料科学
背景:
- 超冷却保存は,氷結晶の形成なしに低温で生物学的物質を維持することを目的としています.
- 氷の核形成の確率は温度に依存し,同位体系におけるポアソン分布に従っている.
- 既存の方法は,低温と核化のリスクのバランスをとる上で課題に直面しています.
研究 の 目的:
- 多相同位体システムの熱力学分析と設計を提示する.
- 氷の核を最小限に抑えながら 低温で保存できるように
- 生物保存の質を高め,汚染を減らすための戦略を策定する.
主な方法:
- 半透性膜を持つ多相同位体系を用いる.
- コンパートメント内の同位体溶液に物質を閉じ込める.
- 圧力の変化を誘導するために凍結する周囲の水相を使用します.
- 凍った水の平衡状態に比べて内部のコンパートメントを超冷却する.
主要な成果:
- 超冷却状態を 通常の凍結点以下で達成する方法を実証した.
- 圧力による核形成の確率を制御するシステムの設計を紹介した.
- 微生物の汚染を減らすための保存条件を設定する.
- 氷の形成を避けることで 生物学的品質を保ちます
結論:
- 多相イソコアシステムは,高度な超冷却保存のための実行可能な戦略を提供します.
- この技術により,保存温度が低く,汚染のリスクが軽減されます.
- 設計は,優れた生物保存のための高圧環境の作成を容易にする.
さらに関連する動画
関連する概念動画
Phase Transitions: Melting and Freezing
13.1K
Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
13.1K
Sublimation
877
Sublimation is the direct transformation of a solid to a gaseous state. For instance, at standard pressure and room temperature, solid carbon dioxide sublimes to gaseous carbon dioxide. The phase diagram depicts the conditions required for sublimation. This process occurs at the solid-gas phase boundary and is not observed above the triple point of the substance. The reverse of sublimation is called deposition, where a gaseous substance condenses directly into a solid. Sublimation and...
877
Freezing Point Depression and Boiling Point Elevation
35.7K
Boiling Point Elevation
The boiling point of a liquid is the temperature at which its vapor pressure is equal to ambient atmospheric pressure. Since the vapor pressure of a solution is lowered due to the presence of nonvolatile solutes, it stands to reason that the solution’s boiling point will subsequently be increased. Vapor pressure increases with temperature, and so a solution will require a higher temperature than will pure solvent to achieve any given vapor pressure, including one...
The boiling point of a liquid is the temperature at which its vapor pressure is equal to ambient atmospheric pressure. Since the vapor pressure of a solution is lowered due to the presence of nonvolatile solutes, it stands to reason that the solution’s boiling point will subsequently be increased. Vapor pressure increases with temperature, and so a solution will require a higher temperature than will pure solvent to achieve any given vapor pressure, including one...
35.7K
Recrystallization: Solid–Solution Equilibria
1.2K
Recrystallization is a purification technique used to separate impurities from solid compounds. In this technique, no chemical reactions occur. Instead, it exploits physical properties only, specifically, the solubility differences between the desired compound and impurities, either at a single temperature or at different temperatures, and under other selected conditions. The solid-solution equilibrium (solubility equilibrium) of each component in the solution represents a binary phase...
1.2K
Phase Transitions: Sublimation and Deposition
17.9K
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...
17.9K
Isothermal Processes
4.0K
A thermodynamic process that occurs at constant temperature is called an isothermal process. Heat slowly flows into the system or out of the system to maintain thermal equilibrium. Processes involving phase changes like water evaporation into steam or freezing water into ice at a constant temperature are examples of Isothermal Processes.
An ideal gas can also undergo isothermal expansion or compression.
For example, consider 1 mole of an ideal gas inside an isolated cylinder at initial volume V...
An ideal gas can also undergo isothermal expansion or compression.
For example, consider 1 mole of an ideal gas inside an isolated cylinder at initial volume V...
4.0K


