Name: vaporization, boiling, and evaporation
Uploaded: 2019-03-11T09:21:01.000Z
Duration: 1 min 18 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Earth and Environmental Science

Earth's Systems

ESS.EES.3.1

Vaporization

- [Verteller] Verdamping is de overgang van een vloeistof naar een gas of damp. Bijvoorbeeld, wanneer warmte-energie aan het water wordt toegevoegd, bereikt het zijn kookpunt en wordt het stoom. De hoeveelheid energie die nodig is om een bepaalde hoeveelheid vloeistof bij een constante temperatuur te verdampen, wordt de verdampingswarmte genoemd.

Daarnaast kan verdamping ook plaatsvinden aan het oppervlak van een vloeistof in een proces dat evaporatie wordt genoemd. Ditmaal wordt kinetische energie bijgedragen door de zon en de wind. Als de energie de intermoleculaire krachten overstijgt, kunnen moleculen loskomen en damp worden, een belangrijk middel voor het afkoelen bij dieren door middel van zweet.

Omdat zweet vooral water is, verdampen deze moleculen. Wanneer ze ontsnappen, volgt de warmte-energie die in de moleculen is opgeslagen, waardoor de collectieve temperatuur van de resterende druppels daalt en het lichaam koeler wordt. Verdamping is ook een belangrijke factor in de transpiratie van planten.

Met de steun van cohesie en adhesie, helpt de verdamping van water aan het oppervlak van bladeren om nabijgelegen moleculen omhoog te trekken, waardoor water van de wortels naar de bladeren wordt gebracht.

verdamping

De fysieke vorm van een stof verandert door de temperatuur te verhogen. Bijvoorbeeld, door de temperatuur van een vloeistof te verhogen, wordt de vloeistof verdampt (omgezet in damp). Dit proces wordt verdamping genoemd —een oppervlaktefenomeen. Voor verdamping om plaats te vinden, moet de kinetische energie groter zijn dan de intermoleculaire krachten die de moleculen bij elkaar houden. De hoeveelheid energie die nodig is om een hoeveelheid vloeistof te verdampen bij een gegeven druk en constante temperatuur wordt de verdampingswarmte genoemd. Wanneer vloeibaar water verdampt, verandert het in stoom.

Het verwarmen van een vloeistof tot het kookpunt is een methode van verdamping. Koken vindt plaats wanneer dampbellen zich onder het oppervlak van de vloeistof vormen. Het kookpunt varieert afhankelijk van de atmosferische druk. Bij hogere atmosferische druk is meer energie nodig om het kookpunt te bereiken. Op zeeniveau kookt water bij het normale of atmosferische kookpunt (100 ⁰C of 212 ⁰F). Op grotere hoogtes is er minder energie nodig om water te laten koken. Zo kookt water op ongeveer 71 ⁰C (160 ⁰F) op de top van de Mount Everest.

Sublieme verdamping, een ander type verdamping, vindt plaats onder het kookpunt. In dit proces ontsnappen watermoleculen die voldoende kinetische energie hebben om de intermoleculaire krachten te overwinnen, van het wateroppervlak als damp. De resterende watermoleculen hebben een lagere kinetische energie. Als dit op grote schaal gebeurt, neemt de algehele kinetische energie van de vloeistofmassa af, wat de vloeistof afkoelt. Zweten maakt gebruik van het fenomeen van verdamping om de lichaamstemperatuur te verlagen. Wanneer zweet van het lichaam verdampt, is het resterende zweet koeler en helpt het om warmte van het lichaam op te nemen.

De verdampingscapaciteit van water wordt ook door planten gebruikt om water omhoog door de plant te verplaatsen. Op een milieuschaal is de verdamping van water de motor die de watercyclus aandrijft en een groot deel van het weer en het klimaat op aarde beïnvloedt.

Verdamping

The physical form of a substance changes by changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

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vaporization, boiling, and evaporation

Vaporization changes a liquid into vapor when temperature adds enough kinetic energy to overcome intermolecular forces. It is a surface phenomenon, which means it starts at the liquid’s surface. The energy needed to vaporize a set amount of liquid at a given pressure and constant temperature is called the heat of vaporization.

Water shows this process clearly. When liquid water is vaporized, it becomes steam. One way this happens is boiling, which occurs when vapor bubbles form beneath the surface of the liquid. The boiling point changes with atmospheric pressure. With more pressure, more energy is needed to reach the boiling point.

At sea level, water boils at the normal, or atmospheric, boiling point of 100 °C, or 212 °F. At higher elevations, water needs less energy to boil. For example, water boils at about 71 °C, or 160 °F, on Mount Everest. Evaporation is another form of vaporization, but it happens below the boiling point.

During evaporation, water molecules with enough kinetic energy escape from the surface as vapor. The molecules left behind have lower kinetic energy. If evaporation happens on a large scale, the liquid loses overall kinetic energy and cools. Sweat uses this effect to lower body temperature. As perspiration evaporates, the cooler sweat helps absorb heat from the body. Plants also use water’s evaporative properties to move water upward through the plant. On a larger scale, evaporation drives the water cycle and helps shape Earth’s weather and climate.

Vaporization, Boiling, and Evaporation

the periodic table and organismal elements

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Hydrogen Bonds in Water

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Intermolecular Forces in Polar Solutions

Intermolecular forces are the attractions and repulsions that act between atoms and molecules. These electrostatic forces come from particles with permanent, partial, or temporary charges. For neutral atoms and molecules, the main types are ion-dipole, dipole-dipole, and dispersion forces, which are together called van der Waals forces. Polar molecules have a partial positive end and a partial negative end. That separation of charge creates a dipole. In water, oxygen is more electronegative...

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Elements, Compounds, and Bonding

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Electron Geometry and Lone Pairs

Electron geometry and lone pairs help explain why molecules take specific shapes. The arrangement of electron groups around a central atom controls the molecular geometry. Valence electrons form bonding pairs, which sit mainly between bonded atoms, or lone pairs, which belong to one atom only. Electron pairs in the valence shell spread out to reduce repulsion. They do this by maximizing the distance between one another. A diatomic molecule has two regions of electron density, and these are...

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pH measures how acidic or basic a water-based solution is. It depends on the concentration of hydronium ions, H3O+, in the solution. In one liter of pure water at neutral pH, there are 1×10−7 moles of hydronium ions. Because hydronium ion levels can vary over a very wide range, measuring pH directly in moles is not practical. The pH scale converts hydronium ion concentration into a negative logarithm. Pure water has a pH of 7 and is neutral. Most solutions fall between 0 and 14, but some, such...

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Chemical reactions rearrange atoms to form new substances. In a reaction, the starting materials are called reactants, and the new substances are called products. The atoms stay the same type and number, but their bonds change, so the substances become different compounds. During a chemical reaction, bonds between atoms break and form again. This means the shared electrons are rearranged. Some reactions happen on their own, while others need an energy source such as heat or light. In biology,...

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Electron Transfer in Redox

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cohesion

Water Molecules and Surface Tension

Water molecules stick to each other through cohesion. Water is neutral overall, but it is a polar molecule. The oxygen atom in one water molecule has a partial negative charge, and it can bind with a hydrogen atom that has a partial positive charge in another water molecule. This forms a hydrogen bond. Each water molecule can form up to four hydrogen bonds with other water molecules, and these bonds give water its cohesive nature. Cohesion helps water form droplets on a surface. Water does not...

adhesion

Water Climbing by Adhesion

Water can climb or stick to surfaces because of adhesion, which is the attraction between different kinds of molecules. In water, this is easy to see on polar surfaces such as glass or cellulose in plants. The positive hydrogen side of water is more attracted to the negative oxygen in silica than to nearby water molecules. This attraction helps explain capillary action. If a narrow glass tube is placed in a beaker of water, water molecules attach to the tube’s surface and the water level rises.

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Water Phase Changes and Ice Density

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specific heat

How Specific Heat Affects Temperature

Specific heat capacity describes how much energy a substance needs to rise by 1 degree Celsius for each gram. It is often written with calories, grams, and degrees Celsius, but it can also be shown in joules, kilograms, and Kelvin. For water, 1 gram needs 1 calorie to increase by 1°C, which is also written as 1 cal/g-°C or 4186 J/kg/K. Water has a high specific heat capacity, so it takes in a large amount of heat before its temperature changes much. It also gives off a lot of heat when it...

vaporization

Vaporization changes a liquid into vapor when temperature adds enough kinetic energy to overcome intermolecular forces. It is a surface phenomenon, which means it starts at the liquid’s surface. The energy needed to vaporize a set amount of liquid at a given pressure and constant temperature is called the heat of vaporization. Water shows this process clearly. When liquid water is vaporized, it becomes steam. One way this happens is boiling, which occurs when vapor bubbles form beneath the...

solvents

Water as a Biological Solvent

Water acts as a biological solvent in many living systems. A solvent is a substance, usually a liquid, that dissolves another substance called a solute. When a solvent and a solute mix, they form a solution, which is a uniform mixture of both parts. Water is called a universal biological solvent because its polar structure helps it dissolve many other polar compounds. Polarity means that one side of the molecule has a slight positive charge and the other side has a slight negative charge.

carbon skeletons

Carbon Backbones in Biomolecules

Carbon backbones give biological molecules their structure and flexibility. Living things are built from macromolecules that contain carbon atoms, and organic compounds are defined by a carbon backbone. Carbon is tetravalent, so each carbon atom can bond with four other atoms. Its valence electrons are stable, so carbon rarely becomes an ion. As carbon chains get longer, they can form ring structures, double bonds, and branching side chains. Carbon-carbon bonds create the carbon skeleton.

key terms and concepts

Explore how heat changes liquids into vapor, including boiling, evaporation, boiling point changes with pressure, cooling from sweat, and the water cycle.

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Vaporization, Boiling, and Evaporation

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