Name: steam distillation and low-boiling separation
Uploaded: 2020-03-26T07:22:28.000Z
Duration: 3 min 54 s
Channel: JoVE

Quando uma mistura ideal de dois líquidos miscíveis é aquecida até a ebulição, a solução ferve a uma temperatura entre os pontos de ebulição de cada componente. Se esses líquidos tiverem pontos de ebulição muito diferentes, quando a mistura começar a ferver, o vapor é rico com as moléculas do componente mais volátil. Esse fenômeno é frequentemente usado para separar misturas usando destilação simples, onde uma mistura de dois líquidos miscíveis é aquecida e o vapor é então condensado de volta ao líquido e coletado.
À medida que o vapor rico com o componente mais volátil é coletado como destilado, a fase líquida torna-se rica com as moléculas do componente menos volátil. No entanto, essa técnica requer que a solução seja aquecida pelo menos até o ponto de ebulição do composto mais volátil e, muitas vezes, além disso.
No caso de compostos orgânicos sensíveis à temperatura, essa alta temperatura pode levar à decomposição das moléculas orgânicas em outra coisa. Então, como podemos separar esses tipos de compostos? Primeiro, vamos dar um passo para trás.
Lembre-se de que a pressão de um vapor em equilíbrio com sua fase condensada é chamada de pressão de vapor. Cada um dos componentes de uma mistura de líquidos tem sua própria pressão de vapor, que chamamos de pressão parcial. Sabemos que uma solução ferve quando a pressão total de vapor da solução é igual à pressão atmosférica. A pressão total de vapor é igual à soma das pressões parciais dos componentes.
Para uma mistura de líquidos miscíveis, o que significa que qualquer combinação de líquidos forma uma solução homogênea, as pressões parciais são calculadas a partir das pressões de vapor dos compostos puros multiplicadas por suas frações molares na solução. No entanto, para uma mistura heterogênea de líquidos imiscíveis, o que significa que os líquidos são insolúveis uns nos outros, as pressões parciais são simplesmente as pressões de vapor dos compostos puros.
Como cada componente da mistura heterogênea contribui para a pressão de vapor total independentemente dos outros componentes, a mistura ferve quando a pressão de vapor total, que é a soma das pressões parciais, é igual à pressão atmosférica. Isso ocorre a uma temperatura mais baixa do que os pontos de ebulição individuais de cada componente, porque a pressão total do vapor aumenta com a temperatura muito mais rápido do que você esperaria até mesmo para o componente mais volátil.
Podemos aproveitar esse fenômeno para realizar a destilação a vapor, que é usada para isolar um composto orgânico sensível à temperatura que se decompõe sob altas temperaturas e é insolúvel em água de substâncias não voláteis. A configuração de destilação a vapor é semelhante a uma configuração de destilação simples com a adição de um reservatório de água para reabastecer a água durante todo o processo.
À medida que a mistura ferve, tanto a água quanto o composto orgânico de interesse são vaporizados. A água e os vapores de compostos orgânicos viajam para o condensador, são condensados em líquido e coletados. Os líquidos imiscíveis são separados posteriormente. Apenas água e materiais não voláteis são deixados na mistura no frasco.
Neste laboratório, você configurará e realizará um experimento de destilação a vapor para extrair o óleo essencial dos componentes não voláteis de uma casca de laranja. Em seguida, você usará a extração líquido-líquido para extrair o óleo essencial da água em um solvente orgânico.

destilação a vapor

Steam Distillation

<h4>Destilação a vapor </h4>
A destilação a vapor é uma técnica de separação que aproveita a propriedade de baixo ponto de ebulição de misturas imiscíveis. É predominantemente usado para separar moléculas orgânicas sensíveis à temperatura de um contaminante não volátil. A molécula orgânica deve ser imiscível em água.
Na destilação a vapor, a mistura imiscível é aquecida até a ebulição, causando a destilação da água e dos compostos orgânicos voláteis. Isso significa que a mistura gasosa sobe até um condensador, que então condensa o vapor em líquido para que possa ser coletado. Em contraste com a destilação simples, a destilação a vapor usa um reservatório de água para reabastecer a água na mistura aquecida durante todo o processo. O componente orgânico imiscível é destilado lentamente junto com a água, enquanto o componente não volátil permanece na mistura aquecida. Uma vez que o componente orgânico é destilado, ele pode ser separado da água usando extração líquido-líquido.
<h4>Pressão de vapor de uma mistura</h4>
Para uma mistura miscível que forma uma solução homogênea, a pressão de vapor de cada componente depende da pressão de vapor do componente puro e sua fração molar na mistura líquida de acordo com a lei de Raoult.
pA = pA*xA
em que pA é a pressão de vapor de um componente líquido numa mistura líquida miscível, pA* é a pressão de vapor do líquido puro e xA é a fracção molar desse líquido na mistura, que é igual a nA/nt. nA é o número de moles do líquido individual na mistura, e nt é o número total de moles de todos os líquidos da mistura.
A pressão de vapor total acima da mistura líquida miscível é igual à soma da pressão de vapor parcial de cada componente nela, o que é conhecido como lei de Dalton. A pressão de vapor de um líquido aumenta com a temperatura à medida que mais moléculas ganham energia cinética para escapar da fase líquida para a fase gasosa. Em uma mistura miscível contendo dois líquidos, a pressão total pode ser descrita como:
P = pA + pB
onde pA e pB são as pressões de vapor do líquido A líquido B, respectivamente, acima da mistura. P é a pressão total de vapor de ambos os líquidos acima da mistura. A combinação das equações descreve a relação entre a pressão de vapor total da solução e a fração molar dos componentes individuais:
P = pA*xA + pB*xB
Em uma mistura imiscível, onde os componentes formam uma mistura heterogênea, as pressões de vapor de cada componente contribuem independentemente para a pressão total de vapor. Assim, a pressão total de vapor é igual à soma das pressões individuais de vapor puro. Em uma mistura imiscível composta por dois líquidos, a pressão total é definida como a pressão de vapor do primeiro líquido mais a pressão de vapor do segundo líquido.
P = pA* + pB*
<h4>Ponto de ebulição de uma mistura imiscível</h4>
À medida que um líquido é aquecido, a pressão do vapor aumenta. Cada componente de uma mistura tem seu próprio ponto de ebulição. Em uma mistura de líquidos miscíveis, a ebulição ocorre a uma temperatura entre os pontos de ebulição dos líquidos constituintes.
Para uma mistura imiscível, a ebulição ocorre a uma temperatura muito mais baixa do que os pontos de ebulição dos componentes individuais. Como cada componente individual contribui de forma independente, menos calor é necessário para aumentar a pressão total do vapor para a pressão atmosférica.
Por exemplo, considere a mistura imiscível de benzeno e água. O ponto de ebulição do benzeno à pressão atmosférica normal é de 80,1 ° C e o ponto de ebulição da água à pressão atmosférica normal é de 100 ° C. A solução ferve quando a pressão total de vapor atinge 760 mm Hg (pressão atmosférica normal). A 69,3 °C, a pressão de vapor da água é de 227 mm Hg e a pressão de vapor de benzeno é de 533 mm Hg, o que no total equivale aos 760 mm Hg necessários para ferver. Isso está bem abaixo do ponto de ebulição de qualquer componente individual.
<h4>Referências</h4>
<ol>
	<li style="font-size:17px">Kotz, J.C., Treichel Jr, P.M., Townsend, J.R. (2012). Química e Reatividade Química. Belmont, CA: Brooks / Cole, Cengage Learning.</li>
	<li style="font-size:17px">Silderberg, M.S. (2009). Química: A Natureza Molecular da Matéria e da Mudança. Boston, MA: Colina McGraw.</li>
</ol>

Destilação a vapor

Destilação a vapor 
A destilação a vapor é uma técnica de separação que aproveita a propriedade de baixo ponto de ebulição de misturas imiscíveis. É predominantemente ...

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steam distillation and low-boiling separation

Steam distillation is a separation method for temperature-sensitive organic compounds. It works best when the organic compound is immiscible in water, meaning the two liquids do not mix. The method helps remove the organic molecule from a non-volatile contaminant without using the higher temperatures needed for many other separations.

In steam distillation, the immiscible mixture is heated until both water and the volatile organic compound distill together. The vapor rises to a condenser, where it cools and becomes a liquid that can be collected. Unlike simple distillation, this setup uses a water reservoir to keep replacing water in the heated mixture during the process.

The organic component is carried over slowly with the water, while the non-volatile component stays behind in the heated flask. After distillation, the organic product can be separated from the water by liquid-liquid extraction. This makes steam distillation useful for isolating sensitive organic materials from unwanted impurities.

The same low-boiling behavior can be explained by vapor pressure. For a miscible mixture, each liquid follows Raoult’s law, so its vapor pressure depends on the pure liquid vapor pressure and its mole fraction. The mole fraction is the number of moles of one liquid divided by the total number of moles in the mixture. The total vapor pressure above a miscible mixture follows Dalton’s law and equals the sum of the partial vapor pressures.

As temperature rises, vapor pressure increases because more molecules gain enough kinetic energy to escape into the gas phase. In a two-liquid miscible mixture, the total pressure can be written as P = pA + pB, or as P = pA*xA + pB*xB when Raoult’s law is included. In an immiscible mixture, the components act independently, so the total pressure is the sum of the vapor pressure of the first liquid and the vapor pressure of the second liquid.

This independent vapor-pressure behavior is why immiscible mixtures boil at lower temperatures than either pure liquid. In a miscible mixture, boiling usually happens between the boiling points of the components. In an immiscible mixture, less heat is needed to reach atmospheric pressure, so the boiling point drops well below the boiling points of the individual liquids.

A benzene-water mixture shows this effect clearly. Benzene boils at 80.1 °C, and water boils at 100 °C at normal atmospheric pressure. The mixture boils when the total vapor pressure reaches 760 mm Hg. At 69.3 °C, water contributes 227 mm Hg and benzene contributes 533 mm Hg, which adds up to 760 mm Hg. That means the mixture boils at a temperature below either pure component.

Steam Distillation and Low-Boiling Separation

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Steam Distillation and Low-Boiling Separation

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