Evaporation Process
Evaporation Process - Related Videos
06:43
Rotary Evaporation to Remove Solvent
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2023
Source: Dr. Melanie Pribisko Yen and Grace Tang — California Institute of Technology Rotary evaporation is a technique most commonly used in organic chemistry to remove a solvent from a higher-boiling point compound of interest. The rotary evaporator, or "rotovap", was invented in 1950 by the chemist Lyman C. Craig. The primary use of a rotovap is to dry and purify samples for downstream applications. Its speed and ability to handle large volumes of solvent make rotary evaporation a preferred...
06:39
A High Performance Impedance-based Platform for Evaporation Rate Detection
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Cited by 1 •
2016
This paper presents an impedance-based apparatus for evaporation rate detection of solutions. It offers clear advantages over a conventional weight loss approach: a fast response, high-sensitivity detection, a small sample requirement, multiple sample measurements, and easy disassembly for cleaning and reuse purposes.
08:58
Seedless Growth of Bismuth Nanowire Array via Vacuum Thermal Evaporation
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Cited by 1 •
2015
A protocol for seedless and high yield growth of bismuth nanowire arrays through vacuum thermal evaporation technique is presented.
14:01
Making Record-efficiency SnS Solar Cells by Thermal Evaporation and Atomic Layer Deposition
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Cited by 31 •
2015
Tin sulfide (SnS) is a candidate material for Earth-abundant, non-toxic solar cells. Here, we demonstrate the fabrication procedure of the SnS solar cells employing atomic layer deposition, which yields 4.36% certified power conversion efficiency, and thermal evaporation which yields 3.88%.
04:36
Tea Aroma Analysis Based on Solvent-Assisted Flavor Evaporation Enrichment
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Cited by 7 •
2023
Presented here is a method for enriching and analyzing the volatile components of tea extracts using solvent-assisted flavor evaporation and solvent extraction followed by gas chromatography-mass spectrometry, which can be applied to all types of tea samples.
FAQs
Intermolecular attractions determine how much energy surface molecules must gain before leaving the liquid. Stronger attractions make escape more difficult, while molecules with sufficient energy can enter the gas phase. This relationship helps explain why solvent behavior varies among chemical systems and why the strength of molecular interactions matters when interpreting evaporation during laboratory work.
Temperature affects the energy available to molecules at a liquid surface. As temperature changes, the number of molecules able to overcome intermolecular attractions and enter the gas phase also changes, altering the evaporation rate. In chemistry, this energy dependence is important for controlling solvent removal and understanding energy transfer during phase change.
Vapor pressure reflects a liquid’s tendency to contribute molecules to the gas phase, so it helps determine how readily evaporation occurs. The surrounding pressure also influences the process by changing the conditions for molecules leaving the surface. Considering both variables helps chemists anticipate solvent behavior and compare evaporation conditions in laboratory or industrial operations.
Temperature, exposed surface area, airflow, vapor pressure, and surrounding pressure all influence evaporation. Increasing or otherwise controlling these conditions can change how quickly a liquid is removed, although their effects depend on the chemical system. Managing these variables allows researchers to concentrate solutions or remove volatile solvents more deliberately during sample preparation and purification.
Evaporation concentrates a solution by removing its volatile solvent while leaving nonvolatile substances behind. As solvent loss proceeds, the remaining material occupies a larger proportion of the solution. Chemists use this approach when they need a more concentrated sample, and the resulting change in composition can prepare the material for later crystallization or analysis.
Controlled solvent removal supports several laboratory goals. Concentrating a solution can create conditions useful for crystallization, while removing a volatile solvent from a nonvolatile substance prepares a sample for subsequent handling or purification. The process is therefore valuable not only as a phase change but also as a practical method for changing composition in chemical experiments.