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

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Earth and Environmental Science

Earth's Systems

ESS.EES.3.1

Specific Heat

- [Anlatıcı] Maddeler ısıyı farklı şekillerde emer ve özgül ısı kapasitelerine, yani belirli bir kütle için ısıyı bir derece değiştirmek adına gereken ısı enerjisi ölçümüne sahiptirler.
 Bu miktara kalori adı da verilir.
 Su, kum taşını oluşturan silikondan daha düşük bir molar kütlesi olduğu için kayalardan daha yüksek bir özgül ısıya sahiptir.
Suda gram başına daha çok molekül olduğundan, daha fazla enerji emebilir, bu da ısı değiştirme süresini uzatır.
 Kum daha hızlı ısınır çünkü daha az silikon molekülü vardır.
 Böylece su, aşırı ortam ısılarını düzenlemede başarılıdır.
Örneğin kıyı kesimlerinin gün içinde ısınması, gece boyunca da soğuması daha uzun sürerken, yakında su etkisi bulunmayan karasal bölgeler daha hızlı ısınır ve soğur, daha aşırı sıcaklıklar görülür.

Özgül isı

Bir maddenin özgül ısı kapasitesi, bir gram maddenin bir derece ısıtılması için gereken enerji miktarını ifade eder. Su yüksek bir ısı kapasitesine sahiptir, bu nedenle sıcaklığını artırmak için çok fazla ısı gerekir. Benzer şekilde, suyun sıcaklığının düşmesi için de çok fazla ısı kaybetmesi gerekir, bu nedenle ısıtıldıktan sonra yavaşça soğur. Karşılaştırıldığında, metaller düşük ısı kapasitesine sahiptir — çabuk ısınırlar ve çabuk soğurlar.

Özgül ısı kapasitesi, bir gram maddenin sıcaklığını bir Santigrat derece (1 °C) yükseltmek için gereken enerji miktarı olarak tanımlanır. Örneğin, bir gram suyun sıcaklığını 1 °C arttırmak, bir kalorilik ısı enerjisi gerektirir. Özgül ısı kapasitesi genellikle gram, Santigrat derece ve kalori olarak gösterilir, ancak kilogram, Kelvin (K) ve joule (diğer birimler arasında) olarak da ifade edilebilir. Suyun özgül ısı kapasitesi bir kalori / gram °C veya 4186 joule / kilogram K’dir. Katı altının özgül ısı kapasitesi ~0,03 kalori / gram °C veya 129 joule / kilogram K’dır. Yani altın, sudan daha düşük özgül ısı kapasitesine sahiptir.

<h4>Pratik Doğa</h4>

Suyun yüksek ısı kapasitesi, aşırı ortam sıcaklıklarının ayarlanmasına yardımcı olur. Büyük su kütlelerinin yakınındaki kasabalarda hem günlük hem de mevsimsel olarak daha küçük sıcaklık değişiklikleri görülür. Gün boyunca, yakındaki su ısı enerjisini emerek çevredeki araziyi soğutur. Geceleri su, ısı enerjisini açığa çıkararak alanı daha sıcak tutar. Büyük su kütlelerinden uzak kasabalar, günlük ve mevsimsel sıcaklıklarda büyük dalgalanmalar yaşayabilir. Kum ve kayaların ısı kapasiteleri daha düşüktür, bu nedenle gün içinde hızlı bir şekilde ısınırlar ve geceleri ise hızla ısı yayarlar.

Uzayda su kaynar ve sonra donar. Bu, kısmen suyun yüksek ısı kapasitesinden kaynaklanmaktadır. Uzayda su, aşırı düşük basınç nedeniyle ilk önce kaynar. Bu gaz halinde, su buharı molekülleri daha da ayrıktır ve uzayın çok soğuk sıcaklıklarında hızlı bir şekilde ısıyı kaybedebilir. Su buharı daha sonra kristaller halinde donarlar —desüblimasyon adı verilen bir süreç.

Özgül Isı

Bir maddenin özgül ısı kapasitesi, o maddenin bir gramının sıcaklığını bir santigrat derece artırmak için gereken enerjiyi ifade eder. ...

Education

JoVE Core

Biology

Biyoloji

Fundamentals

Temel İlkeler

Chemistry of Life

Yaşamın Kimyası

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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

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redox reactions

Electron Transfer in Redox

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cohesion

Water Molecules and Surface Tension

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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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JoVE Core serisi, biyolojinin ana konseptlerini açıklayan 300 adet kısa ve kolay anlaşılabilir olan video dersleriyle ve günümüz laboratuvarlarında yürütülen gerçek araştırmaları gösteren 150'den fazla \"bilim insanları iş başında\" videolarıyla biyolojiye hayat vermektedir.

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CHEM.13

CHEM.13.D

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From Molecules to Organisms: Structures and Processes

9-12.B.1.4.b

Earth and Space Science

9-12.ESS.2.7.b

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Florida Department of Education

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SC.912.L.18

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How Specific Heat Affects Temperature

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