Name: how specific heat affects temperature
Uploaded: 2019-03-11T09:21:01.000Z
Duration: 1 min 16 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

Specific Heat

- [Instructeur] Stoffen absorberen warmte verschillend, en bezitten specifieke warmtecapaciteiten. Wat een maat is voor de warmte-energie die nodig is om voor een bepaalde massa de temperatuur met één graad te veranderen. Water heeft een hogere specifieke warmtecapaciteit dan de nabijgelegen rotsen door een lagere molaire massa dan het silicone, waaruit zandsteen is opgemaakt.

Omdat water meer moleculen per gram heeft, kan het meer energie absorberen, waardoor het langer duurt voordat de temperatuur veranderd. Zand zal sneller opwarmen omdat er minder siliconenmoleculen zijn. Water is dus goed in het reguleren van extreme omgevingstemperaturen.

Kustgebieden hebben bijvoorbeeld meer tijd nodig om overdag op te warmen en 's nachts om af te koelen, terwijl door land ingesloten plaatsen zonder nabije waterinvloeden snel opwarmen en afkoelen, wat leidt tot extremere temperaturen.

soortelijke warmte

De soortelijke warmtecapaciteit van een stof verwijst naar de hoeveelheid energie die nodig is om de temperatuur van één gram van die stof met één graad Celsius te verhogen. De soortelijke warmtecapaciteit wordt vaak uitgedrukt in calorieën (cal), grammen (g) en graden Celsius (°C), maar kan ook worden uitgedrukt in joules (J), kilogrammen (kg) en Kelvin (K), onder andere eenheden.

Bijvoorbeeld, om de temperatuur van één gram water met 1°C te verhogen, is één calorie warmte-energie nodig, wat kan worden geschreven als 1 cal/g-°C, of 4186 J/kg/K. Water heeft een hoge soortelijke warmtecapaciteit. Het absorbeert een grote hoeveelheid warmte om de temperatuur te verhogen en geeft op dezelfde manier veel warmte af wanneer het afkoelt. Daarom duurt het relatief lang voor water om op te warmen of af te koelen.

Aan de andere kant hebben metalen een lage warmtecapaciteit en worden snel warm en snel weer koud. Bijvoorbeeld, vast goud heeft een soortelijke warmtecapaciteit van ongeveer 0,03 cal/g/°C of 129 J/kg/K, wat veel minder is dan water.



<h4>Water heeft een hoge soortelijke warmte</h4>



Wanneer water wordt gekookt, wordt er veel energie opgenomen om de waterstofbruggen tussen de watermoleculen te verbreken. Dit resulteert in de willekeurige beweging van de watermoleculen. Evenzo, wanneer het water afkoelt, beginnen waterstofbruggen zich te vormen tussen de watermoleculen wanneer het water afkoelt, waardoor ze dichter bij elkaar komen. Er komt een enorme hoeveelheid warmte vrij tijdens dit proces.



<h4>Matiging van omgevings-temperaturen</h4>



De hoge warmtecapaciteit van water helpt extreme omgevings-temperaturen te matigen. Steden in de buurt van grote waterlichamen hebben kleinere temperatuurveranderingen zowel dagelijks als seizoensgebonden. Overdag absorbeert het nabijgelegen water warmte-energie, wat het omringende land afkoelt. 's Nachts geeft het water zijn warmte-energie weer af, waardoor het gebied warmer blijft. Steden die verder van grote waterlichamen liggen, kunnen grote schommelingen in dagelijkse en seizoensgebonden temperaturen ervaren. Aangezien zand en rotsen een lagere warmtecapaciteit hebben, warmen ze overdag snel op en geven ze 's nachts snel warmte af.

Soortelijke warmte

The specific heat capacity of a substance refers to the energy required to increase the temperature of one gram of that substance by one degree Celcius. ...

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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 cools. That is why water heats up and cools down slowly. Metals have a much lower heat capacity, so they warm up quickly and also lose heat quickly. Solid gold is one example, with a specific heat capacity of about 0.03 cal/g/°C or 129 J/kg/K.

Water’s high specific heat is linked to hydrogen bonds between water molecules. When water is boiled, it absorbs a large amount of energy to break these bonds, which lets the molecules move more freely. When water cools, hydrogen bonds form again and pull the molecules closer together. A large amount of heat is released during this process.

This property also helps control environmental temperatures. Areas near large bodies of water usually have smaller daily and seasonal temperature changes. During the day, the water absorbs heat and cools the nearby land. At night, the water gives off stored heat and keeps the area warmer.

Places far from large bodies of water can have much bigger swings in temperature. Sand and rocks have lower heat capacities, so they heat up quickly in the day. They also release heat quickly at night. This is why water helps moderate climate more than dry land does.

How Specific Heat Affects Temperature

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specific heat

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...

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key terms and concepts

Learn how specific heat capacity controls heating and cooling, why water changes temperature slowly, and how it helps moderate climate near oceans and lakes.

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How Specific Heat Affects Temperature

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