Name: heat transfer and specific heat
Uploaded: 2025-06-17T07:55:58.000Z
Duration: 2 min 46 s
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.2

Quantifying Heat

Innere Energie wird durch die Umwandlung von Hitze und Arbeit definiert. Aber wie wird Wärme gemessen? Jeder Stoff besitzt Wärmeenergie.Wenn ein System eine Temperaturdifferenz mit seiner Umgebung erlebt, fließen thermische Energieströme von der Materie der höheren Temperatur zur Materie der niedrigeren Temperatur. Diese thermische Energieübertragung wird auch als Wärmeübertragung bezeichnet und wird in Joule gemessen. Die Temperatur hingegen beschreibt eine Eigenschaft der thermischen Energie und wird in Celsius oder Kelvin gemessen.Die Temperatur ist also substanzunabhängig, im Gegensatz zu Wärme, die von der Anzahl und Art der Molekülen in einem System abhängig ist. Wärme kann mit einer Technik namens Kalorimetrie gemessen werden, die das Verhältnis zwischen der Wärme und der Veränderung der Temperatur eines Systems nutzt. Wenn ein Stück Eisen bei 114 Grad Celsius in Wasser mit Raumtemperatur getaucht wird, strömt Wärme vom Eisen zum Wasser bis sie die gleiche Temperatur haben.Sobald es keinen Netto-Wärmestrom mehr gibt, befinden sie sich im thermischem Gleichgewicht. In einem isolierten System gewinnt das Wasser genau so viel Wärme, wie das Eisen verliert. Aber die Endtemperatur beträgt nur ein Grad über der Anfangstemperatur des Wassers, während das Eisen um 93 Grad Celsius abgekühlt ist.Die Menge der übertragenen Wärme ist proportional zur Temperaturänderung delta T.Die Proportionalitätskonstante C oder die Wärmekapazität"ist die Wärmemenge, die benötigt wird, um die Temperatur eines Systems um ein Kelvin oder ein Grad Celsius zu erhöhen. Die Wärmekapazität hängt von der Art des Stoffes ab:ein System mit einer großen Wärmekapazität wie Wasser muss mehr Wärme absorbieren, um seine Temperatur zu erhöhen als ein System mit einer geringeren Wärmekapazität, wie z.B.Eisen. Die Wärmekapazität hängt auch von der Masse der Substanz ab.Spezifische Wärmekapazität, Cs, oder molare Wärmekapazität, Cm, beschreibt die benötigte Wärmemenge um die Temperatur von 1 Gramm oder 1 Mol einer Substanz um 1 Grad Celsius zu erhöhen. Daher wird die Einheit entweder in Joules/angegeben, oder als Joules/Wenn also spezifische Wärmekapazitäten und Temperaturänderung eines Systems bekannt sind, kann der Wert für Wärme aus ihrem Produkt berechnet werden.

quantifizierung von wärme

<h4>Wärmeenergie </h4> Mikroskopisch gesehen ist thermische Energie die kinetische Energie, die mit der zufälligen Bewegung von Atomen und Molekülen verbunden ist. Die Temperatur ist ein quantitatives Maß für „heiß“ oder „kalt“ und hängt von der Höhe der Wärmeenergie ab. Wenn sich die Atome oder Moleküle in einem Objekt schnell bewegen oder vibrieren, haben sie eine höhere durchschnittliche kinetische Energie (KE) (oder eine höhere thermische Energie), das Objekt wird als „heiß“ wahrgenommen und besitzt eine hohe Temperatur. Wenn sich die Atome und Moleküle langsam bewegen, haben sie eine niedrigere durchschnittliche KE (oder eine niedrigere thermische Energie), das Objekt wird als „kalt“ wahrgenommen und wird eine niedrigere Temperatur haben.  Unter der Annahme, dass keine chemischen Reaktionen oder Phasenänderungen (z. B. Schmelzen oder Verdampfen) stattfinden, führt die Erhöhung der Wärmeenergie eines Systems zu einem Temperaturanstieg, während die Verringerung der Wärmeenergie zum absinken der Temperatur führt. <h4>Wärme</h4> Wärme (q) ist die Übertragung von Wärmeenergie zwischen zwei Körpern unterschiedlicher Temperatur. Der Wärmefluss erhöht die Wärmeenergie eines Körpers und verringert die Wärmeenergie des anderen. Wärme fließt spontan von heiß nach kalt (d. h. nur in eine Richtung) und dieser Prozess setzt sich so lange fort, bis beide Systeme die gleiche Temperatur haben. Wärmeänderungen werden durch Temperaturänderungen gemessen.  Die SI-Einheit für Wärme, Arbeit und Energie ist das Joule. Ein Joule (J) ist definiert als die Energiemenge, die verbraucht wird, wenn eine Kraft von 1 Newton ein Objekt entlang der Strecke von einem Meter bewegt. Es ist nach dem englischen Physiker James Prescott Joule benannt. Ein Joule entspricht 1 kg m2/s2 und wird auch als 1 Newtonmeter bezeichnet. Ein Kilojoule (kJ) sind 1000 Joule. Um die Definitionen zu vereinheitlichen, wurde eine Kalorie auf 4,184 Joule festgelegt. <h4>Wärmeübertragung</h4> Die Wärmekapazität (C) eines Stoffes ist die Wärmemenge (q), die er aufnimmt oder abgibt, wenn er eine Temperaturänderung (ΔT) von 1 Grad C (bzw. 1 Kelvin) erfährt: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-01.png" style="height: 40px;"> Die Wärmekapazität wird sowohl durch die Art als auch die Menge der betreffenden Substanz, welche die Wärme aufnimmt oder abgibt bestimmt. Daher ist die Wärmekapazität eine extensive Größe – ihr Wert ist proportional zur Menge des Stoffes. Wird beispielsweise die Wärmekapazität von zwei unterschiedlich schweren gusseisernen Bratpfannen betrachtet ist offensichtlich, dass die Wärmekapazität der schweren Pfanne größer als die der kleinen Pfanne ist, obwohl beide aus dem gleichen Material bestehen. Ist die Masse der großen Pfanne beispielsweise fünfmal größer als die Masse der kleinen Pfanne ist somit auch die Wärmekapazität fünfmal so hoch. Mehr Masse bedeutet, dass mehr Atome in der größeren Pfanne vorhanden sind und somit mehr Energie benötigt wird, um alle diese Atome zu einer schnelleren Schwingen zu bringen. Die Wärmekapazität der kleinen Bratpfanne aus Gusseisen lässt sich durch die Beobachtung errechnen, dass 18.140 J Energie (q) erforderlich sind, um die Temperatur der Pfanne um 50,0 °C (ΔT) zu erhöhen: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-02.png" style="height: 40px;"> Die größere Bratpfanne aus Gusseisen besteht zwar aus dem gleichen Material, benötigt aber 90.700 J Energie (q), um ihre Temperatur um 50,0 °C (ΔT) zu erhöhen. Die größere Pfanne hat eine (proportional) größere Wärmekapazität, da die größere Materialmenge eine (proportional) größere Energiemenge erfordert, um die gleiche Temperaturänderung zu erzielen: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-03.png" style="height: 40px;"> Die spezifische Wärmekapazität (c) einer Substanz, allgemein als „spezifische Wärme“ bezeichnet, ist die Wärmemenge, die erforderlich ist, um die Temperatur von 1 Gramm einer Substanz um 1 Grad Celsius (oder 1 Kelvin) zu erhöhen:  <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-04.png" style="height: 40px;"> Die spezifische Wärmekapazität hängt nur von der Art des Stoffes, der Wärme aufnimmt oder abgibt ab. Es handelt sich um eine intensive Größe, sie ist also nicht von der Menge des Stoffes abhängig. Die kleine Bratpfanne aus Gusseisen hat beispielsweise eine Masse von 808 g. Die spezifische Wärme von Eisen (dem Material, aus dem die Pfanne hergestellt wird) beträgt daher: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-05.png" style="height: 40px;"> Die große Bratpfanne hat eine Masse von 4040 g. Anhand der Daten dieser Pfanne können wir auch die spezifische Wärme von Eisen berechnen: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-06.png" style="height: 40px;"> Die große Pfanne ist zwar massiver ist als die kleine Pfanne aber da beide aus dem gleichen Material bestehen, liefern sie den gleichen Wert für die spezifische Wärme (also für das Konstruktionsmaterial Eisen). Zu beachten ist, dass die spezifische Wärme in Energie pro Temperatur und Masse gemessen wird und eine intensive Größe ist, die aus dem Verhältnis zweier extensiver Größen (Wärme und Masse) ermittelt wird. Die molare Wärmekapazität, ebenfalls eine intensive Eigenschaft, ist die Wärmekapazität pro Mol eines bestimmten Stoffes und hat die Einheit J/mol⋅°C. Wasser hat eine relativ hohe spezifische Wärme (etwa 4,2 J/g⋅°C im flüssigen Zustand und 2,09 J/g⋅°C im festen Zustand); Die meisten Metalle haben eine viel geringere spezifische Wärme (normalerweise weniger als 1 J/g⋅°C). Wenn man die Masse (m) eines Stoffes und seine spezifische Wärme (c) kennt, kann man die Wärmemenge q bestimmen, die von dem Stoff aufgenommen oder abgegeben wurde, indem man die Temperaturänderung (ΔT) während des Wärmegewinnes oder -verlustes misst: <img alt="Eq7" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-07v3.png" style="height: 20px;"> <img alt="Eq8" src="https://www.jove.com/files/core/CDNSource/lessons/794/794_Equations-08v4.png" style="height: 20px;"> Wenn ein Stoff Wärmeenergie aufnimmt, steigt seine Temperatur, seine Endtemperatur ist höher als seine Anfangstemperatur, Tfinal − Tinitial hat einen positiven Wert und der Wert von q ist positiv. Wenn ein Stoff Wärmeenergie abgibt, sinkt seine Temperatur, die Endtemperatur ist niedriger als die Anfangstemperatur, Tfinal − Tinitial hat einen negativen Wert und der Wert von q ist negativ. Hervorzuheben ist, dass die Beziehungen zwischen Wärme, spezifischer Wärme, Masse und Temperaturänderung zur Bestimmung jeder dieser Größen (nicht nur der Wärme) verwendet werden kann, wenn die anderen drei bekannt sind oder abgeleitet werden können. Dieser Text wurde angepasst von <a href="https://openstax.org/books/chemistry-2e/pages/5-1-energy-basics">OpenStax Chemistry 2e, Section 5.1: Energy Basics</a> and <a href="https://openstax.org/books/chemistry-2e/pages/5-3-enthalpy">OpenStax Chemistry 2e, Section 5.3: Enthalpy</a>.

Quantifizierung von Wärme

Wärmeenergie 

Mikroskopisch gesehen ist thermische Energie die kinetische Energie, die mit der zufälligen Bewegung von Atomen und Molekülen verbunden ist. Die Temperatur ist ein ...

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KEY TERMS AND CONCEPTS

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heat transfer and specific heat

Heat transfer and specific heat explain how thermal energy moves and how materials respond to it. Thermal energy is the kinetic energy linked to the random motion of atoms and molecules. Temperature is a measure of how hot or cold a substance is, and it depends on how much thermal energy those particles have.

When atoms and molecules move or vibrate faster, their average kinetic energy is higher. That means the object has more thermal energy and a higher temperature. When they move more slowly, the thermal energy is lower and the temperature drops. If no chemical reaction or phase change, such as melting or vaporizing, occurs, adding thermal energy raises temperature and removing it lowers temperature.

Heat, written as q, is the transfer of thermal energy between two bodies at different temperatures. Heat flow increases the thermal energy of one body and decreases the thermal energy of the other. It moves spontaneously from hot to cold and continues until both substances reach the same temperature. Changes in heat are tracked by changes in temperature.

The SI unit for heat, work, and energy is the joule. One joule is the energy used when a force of 1 newton moves an object 1 meter. It is also equal to 1 kg m^2/s^2, or 1 newton-meter. A kilojoule is 1000 joules, and one calorie is defined as 4.184 joules.

Heat capacity, C, tells how much heat a body absorbs or releases when its temperature changes by 1 degree C, or 1 kelvin. It depends on both the type of substance and the amount present, so it is an extensive property. A large cast iron frying pan has a heat capacity five times greater than a small one because it has five times more mass. More mass means more atoms, so more energy is needed to make all of them vibrate faster.

The small cast iron frying pan in the example takes 18,140 J of energy to rise by 50.0 °C. The larger pan needs 90,700 J to rise by the same amount. Even though both pans are made of the same material, the larger one needs proportionally more energy because it contains more matter.

Specific heat capacity, often called specific heat, is the heat needed to raise 1 gram of a substance by 1 degree Celsius, or 1 kelvin. It depends only on the kind of substance, so it is an intensive property. Using the mass and temperature change of the small pan, the specific heat of iron can be calculated. The large pan gives the same result, even though its mass is greater.

Specific heat is measured in units of energy per temperature per mass. Because it is a ratio of heat and mass, it is intensive even though those two quantities are extensive. The molar heat capacity is another intensive property. It is the heat capacity per mole of a substance and has units of J/mol·°C.

Water has a relatively high specific heat, about 4.2 J/g·°C for liquid water and 2.09 J/g·°C for solid water. Most metals have much lower specific heats, usually less than 1 J/g·°C. If the mass of a substance, its specific heat, and its temperature change are known, the amount of heat entering or leaving it can be found. A positive q means thermal energy is gained and temperature rises. A negative q means thermal energy is lost and temperature falls.

Heat Transfer and Specific Heat

energy basics

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Internal Energy, Heat, and Work

Internal energy is the total of all possible kinds of energy in a substance. It is often written as U, and sometimes as E. For a system that changes energy, the important value is the change in internal energy, or ΔU. ΔU is the difference between the final internal energy and the initial internal energy. The exact values of U final and U initial are usually not known, but the first law of thermodynamics only requires ΔU. A positive ΔU means the system gained energy from the surroundings. A...

quantifying heat

Heat transfer and specific heat explain how thermal energy moves and how materials respond to it. Thermal energy is the kinetic energy linked to the random motion of atoms and molecules. Temperature is a measure of how hot or cold a substance is, and it depends on how much thermal energy those particles have. When atoms and molecules move or vibrate faster, their average kinetic energy is higher. That means the object has more thermal energy and a higher temperature. When they move more...

quantifying work

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enthalpy

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thermochemical equations

Heat Changes in Chemical Equations

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hess's law

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enthalpies of reaction

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key terms and concepts

Learn how heat moves between objects, why temperature changes, and how heat capacity and specific heat help measure thermal energy in materials.

Heat Transfer and Specific Heat | JoVE K12

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Modes of Heat Transfer

Classifying Matter by State

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Classifying Matter by Composition

Matter: Pure Substances and Mixtures
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Physical and Chemical Properties of Matter

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Physical Properties of Matter

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Intermolecular Forces

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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Surface Tension, Capillary Action, and Viscosity

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded ...

States of Matter and Phase Changes

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Phase Transitions

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Phase Transitions: Vaporization and Condensation

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Vapor Pressure

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Clausius-Clapeyron Equation

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Phase Transitions: Melting and Freezing

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Phase Transitions: Sublimation and Deposition

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Heating and Cooling Curves

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Phase Diagrams

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Use models to explain how changes in energy affect the arrangement and movement of the particles in solids, liquids, and gases, as well as the relative strengths of their intermolecular forces.

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Energy Basics

Chemical reactions, such as those that occur when you light a match, involve changes in energy as well as matter.

Chemical changes and their accompanying ...

First Law of Thermodynamics

Energy Conservation

Energy can be converted from one form into another, but all of the energy present before a change occurs always exists in some form ...

Internal Energy

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Thermal Energy&#160;

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Quantifying Work

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Enthalpy

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Thermochemical Equations

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Constant Pressure Calorimetry

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Constant Volume Calorimetry

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Using Differential Scanning Calorimetry to Measure Changes in Enthalpy

Source: Laboratory of Dr. Terry Tritt &#8212; Clemson University
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Hess's Law

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Standard Enthalpy of Formation

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Enthalpies of Reaction

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Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

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Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

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Basic Postulates of Kinetic Molecular Theory: Particle Size, Energy, and Collision

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Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

The test of the kinetic molecular theory (KMT) and its postulates is its ability to explain and describe the behavior of a gas. The various gas laws ...

Use mathematics and computational thinking to explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitatively and quantitatively.

PS.Chm.7.3

Understand the relationship among pressure, temperature, volume, and phase.

Heat Transfer and Specific Heat

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