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

Stoffe nehmen Wärme unterschiedlich auf und besitzen spezifische Wärmekapazitäten, ein Maß für die Wärmeenergie, die benötigt wird, um die Temperatur für eine gegebene Masse um ein Grad zu verändern.
 Diese Menge wird auch als Kalorie bezeichnet.
 Wasser hat eine höhere spezifische Wärme als das nahe gelegene Gestein, da es eine geringere molare Masse als das Silizium aufweist, das Sandstein bildet.
 Da Wasser mehr Moleküle pro Gramm enthält, kann es mehr Energie absorbieren, wodurch es länger dauert, bis sich seine Temperatur ändert.
 Sand erwärmt sich schneller, weil weniger Siliziummoleküle vorhanden sind.
 Somit kann Wasser extreme Umgebungstemperaturen gut regulieren.
 Beispielsweise brauchen Küstengebiete tagsüber länger, um sich aufzuwärmen, und nachts länger, um sich abzukühlen, während ländliche Gebiete ohne nahegelegenes Wasser von der Wärme und Kälte schneller beeinflusst werden und zu extremeren Temperaturen führen.

spezifische wärme

Die spezifische Wärmekapazität eines Stoffes bezieht sich auf die Energiemenge, die benötigt wird, um ein Gramm dieses Stoffes um ein Grad zu erwärmen. Wasser hat eine hohe Wärmekapazität, daher braucht man eine hohe Wärmezufuhr, um seine Temperatur zu erhöhen. Genauso muss Wasser viel Wärme abgeben, damit die Temperatur sinkt. Daher kühlt es nur langsam ab, wenn es einmal erhitzt wurden. Metalle haben im Vergleich dazu eine geringe Wärmekapazität. Sie erwärmen sich schnell und kühlen schnell ab.
 
 Die spezifische Wärmekapazität ist als die Energiemenge definiert, die benötigt wird, um die Temperatur eines Gramm einer Substanz um ein Grad Celsius (1 deg;C) zu erhöhen. Zum Beispiel erfordert die Erhöhung der Temperatur von einem Gramm Wasser um 1 deg;C eine Kalorie Wärmeenergie. Die spezifische Wärmekapazität wird oft in Gramm, Grad Celsius und Kalorien angegeben. Sie kann aber auch in Kilogramm, Kelvin (K) und Joule (neben anderen Einheiten) ausgedrückt werden. Die spezifische Wärmekapazität von Wasser beträgt eine Kalorie/Gramm Grad;C, oder 4186 Joule/Kilogramm K. Massives Gold hat eine spezifische Wärmekapazität von ~0,03 Kalorien/Gramm Grad;C, oder 129 Joule/Kilogramm K. Gold hat also eine niedrigere spezifische Wärmekapazität als Wasser.
 
 <h4>Praktische Natur</h4>
 
 Die hohe Wärmekapazität des Wassers hilft extreme Umgebungstemperaturen zu beeinflussen. Städte in der Nähe von großen Gewässern haben kleinere tägliche und jahreszeitliche Temperaturschwankungen. Tagsüber absorbiert das Wasser in der Nähe Wärmeenergie und kühlt so das umliegende Land. Nachts gibt das Wasser seine Wärmeenergie wieder ab und hält das Gebiet dadurch wärmer. In Städten, die weit von großen Gewässern entfernt sind, können große tägliche und jahreszeitliche Temperaturschwankungen auftreten. Sand und Felsen haben eine geringere Wärmekapazität, so dass sie sich tagsüber schnell aufheizen und nachts die Wärme wieder schnell abgeben.
 
 Im Weltraum kocht Wasser erst und gefriert dann. Dies geschieht zum Teil wegen der hohen Wärmekapazität von Wasser. Im Weltraum siedet Wasser zuerst wegen des extrem niedrigen Drucks. In diesem gasförmigen Zustand sind die Moleküle im Wasserdampf weiter voneinander entfernt und verlieren bei den sehr kalten Temperaturen des Weltraums schnell Wärme. Der Wasserdampf gefriert dann zu Kristallen—ein Prozess, der Resublimation genannt wird.

Spezifische Wärme

Die spezifische Wärmekapazität eines Stoffes bezieht sich auf die Energie, die erforderlich ist, um die Temperatur eines Gramms dieses Stoffes um ein Grad Celsius zu erhöhen. ...

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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

the periodic table and organismal elements

the-periodic-table-and-organismal-elements

Periodic Table Basics for Living Things

The periodic table helps explain which elements living things need and how those elements are related. Elements are the smallest units of matter that cannot be broken down further by chemical processes. There are 118 known elements, but not all occur naturally, and even fewer are essential for life. Living matter is made mostly of carbon, nitrogen, hydrogen, and oxygen. Together, these elements make up most of the human body and are also found in all life on Earth. Smaller amounts of calcium,...

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covalent bonds

Electronegativity and Covalent Bond Polarity

Covalent bonds form when two atoms share electrons to fill their valence shells. The way those shared electrons are pulled depends on electronegativity, which is an atom’s ability to attract electrons in a bond. When atoms have similar electronegativities, they form nonpolar covalent bonds. When their electronegativities differ, the bond is polar because the electrons are shared unevenly. The number of covalent bonds an atom can make depends on its valence electrons. Oxygen has six valence...

ionic bonds

Ionic Compounds and Electrolytes

Ionic compounds form when atoms gain or lose electrons to reach a more stable electron configuration. The charged particles that result are called ions. Ionic bonds are electrostatic attractions between oppositely charged ions. The most reactive elements include those with one valence electron, such as potassium, and those that need one more valence electron, such as chlorine. Ions that lose electrons become positive cations. Ions that gain electrons become negative anions. Cations and anions...

hydrogen bonds

Hydrogen Bonds in Water

Hydrogen bonds in water are weak attractions between atoms that are already part of other chemical bonds. One atom is electronegative, such as oxygen, and carries a partial negative charge. The other is a hydrogen atom that is bonded to another electronegative atom and has a partial positive charge. These attractions form because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom like oxygen or nitrogen. The electrons in that bond are shared unequally.

van der waals interactions

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...

elements and compounds

Elements, Compounds, and Bonding

Elements and compounds are the two main kinds of pure substances. A pure substance contains only one kind of matter. An element contains only one type of atom. A compound contains two or more types of atoms joined by a chemical bond. Elements can be atomic or molecular, depending on their basic units. They are unique forms of matter with specific chemical and physical properties. Ordinary chemical reactions cannot break an element into a smaller substance. There are 118 elements, but only 98...

molecular shapes

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...

pH Scale in Everyday Solutions

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chemical reactions

Atoms, Bonds, and Chemical Reactions

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,...

redox reactions

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.

states of water

Water Phase Changes and Ice Density

Water changes between solid, liquid, and gas states as temperature and molecular motion change. In this lesson, the focus is on how water freezes, melts, vaporizes, and returns to liquid or solid form. The balance between intermolecular forces, which pull molecules together, and kinetic energy, which pushes them apart, controls each state. Water freezes when intermolecular forces become stronger than kinetic energy. Unlike most substances, ice is less dense than liquid water. This happens...

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...

vaporization

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...

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

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

How Specific Heat Affects Temperature | JoVE K12

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From Molecules to Organisms: Structures and Processes

9-12.B.1.4.b

Earth and Space Science

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How Specific Heat Affects Temperature

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