Name: heat exchange in an insulated system
Uploaded: 2025-05-22T09:05:48.000Z
Duration: 1 min 19 s
Channel: JoVE

K12 Standards

Tennessee Academic Standards

High School

Chemistry

Energy

CHEM1.PS3.2

Calorimetry

Kalorimetrie ist die Wissenschaft von der Messung der Wärme, die während eines physikalischen oder chemischen Prozesses unter eingeschränkten Bedingungen freigesetzt und absorbiert wird.
Das Prinzip der Kalorimetrie impliziert, dass, wenn zwei Körper von der Umgebung isoliert sind, die vom kalten Körper gewonnene Wärme gleich dem Wärmeverlust des heißen Körpers ist, d.h. ihre Summe ist gleich Null.
Wenn 30 Gramm null Grad Celsius heiße Eiswürfel in 150 Gramm Orangensaft bei 40 Grad Celsius aufgelöst werden, wie hoch wäre dann die Endtemperatur der Flüssigkeit, nachdem das ganze Eis geschmolzen ist? Die spezifische Hitze von Saft und Eis beträgt 4190 J/kg. K und 2100 J/kg. K bzw. die Schmelzwärme des Eises beträgt 334x103 J/kg.
Listen Sie zunächst die bekannten und unbekannten Größen auf.
Wenden Sie nun das Prinzip der Kalorimetrie auf Saft und Eis an.
Ordnen Sie die Begriffe neu an, um einen Ausdruck für die Endtemperatur zu finden.
Ersetzen Sie die Werte, um die Endtemperatur des Orangensaftes zu berechnen, die 21,86 Grad Celsius beträgt.

<ol>
	<li>OpenStax. (2019). Universitätsphysik Vol. 2. [Webversion]. Abgerufen von <a href="https://openstax.org/details/books/university-physics-volume-2">https://openstax.org/details/books/university-physics-volume-2</a>; Seiten 24-25.</li>
</ol>

kalorimetrie

Wenn Gegenstände mit unterschiedlichen Temperaturen in Kontakt gebracht werden, aber von allem anderen isoliert sind, erreichen sie thermisches Gleichgewicht. Ein Behälter, der den Wärmeübertrag nach innen oder außen verhindert, wird als Kalorimeter bezeichnet, und die Verwendung eines Kalorimeters zur Messung wird als Kalorimetrie bezeichnet. Diese Messungen beziehen sich im Allgemeinen auf Wärme oder spezifische Wärmekapazität. Der Begriff "Kalorimetrie-Problem" wird für jedes Problem verwendet, bei dem die angegebenen Objekte thermisch von ihrer Umgebung isoliert sind. Ein wichtiges Ziel bei der Lösung von Kalorimetrie-Problemen ist, dass während eines Wärmeübertrags zwischen Objekten, die von ihrer Umgebung isoliert sind, die von dem kälteren Objekt gewonnene Wärme der von dem heißeren Objekt verlorenen Wärme entsprechen muss, aufgrund des Energieerhaltungsprinzips.

Zum Beispiel nehmen wir eine Tasse Wasser, die in eine heiße Aluminiumpfanne auf dem Herd gegossen wird. Dabei wird die Pfanne auf einer isolierten Unterlagen platziert, und der Wärmeübertrag an die Luft wird in der kurzen Zeit, die benötigt wird, um das Gleichgewicht zu erreichen, vernachlässigt. Infolgedessen handelt es sich hierbei um ein Kalorimetrie-Problem, obwohl kein isolierender Behälter gegeben ist. Ursprünglich waren die Pfanne und das Wasser nicht im thermischen Gleichgewicht. Die Pfanne ist wärmer als das Wasser. Durch den Wärmeübertrag wird das thermische Gleichgewicht wiederhergestellt, sobald das Wasser und die Pfanne in Kontakt sind; er stoppt, sobald das thermische Gleichgewicht zwischen der Pfanne und dem Wasser erreicht ist. Die von der Pfanne verlorene Wärme entspricht der vom Wasser gewonnenen Wärme, was das grundlegende Prinzip der Kalorimetrie ist.

Kalorimetrie

Wenn Objekte mit unterschiedlichen Temperaturen miteinander in Kontakt gebracht werden, aber von allem anderen isoliert sind, erreichen sie ein thermisches Gleichgewicht. Ein...

Education

Lehre

JoVE Core

Physics

Physik

Unit 1

Einheit 1

Temperature and Heat

Temperatur und Wärme

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

heat exchange in an insulated system

Calorimetry studies heat exchange in an insulated system. A calorimeter is a container that prevents heat transfer in or out. Scientists use calorimetry to measure heat and specific heat capacity.

A calorimetry problem is any situation where the objects are thermally isolated from their surroundings. The key idea comes from conservation of energy. During heat transfer, the heat gained by the colder object must equal the heat lost by the hotter object.

A simple example is water poured into a hot aluminum pan after it is taken off the stove. The pan sits on an insulated pad, and heat transfer to the air is neglected over the short time needed to reach equilibrium. Even without a special container, this setup still counts as a calorimetry problem.

At the start, the pan and the water are not in thermal equilibrium. The pan is hotter than the water. Heat flows until both reach the same temperature, and then the transfer stops. At that point, the heat lost by the pan equals the heat gained by the water.

Heat Exchange in an Insulated System

temperature and thermal equilibrium

Heat, Temperature, and Everyday Energy

Heat and temperature are key ideas in thermodynamics and in everyday life. People often connect temperature with hot and cold, but science gives it a more precise meaning. Temperature is the quantity measured with a thermometer. It is also linked to the average translational kinetic energy of particles. Heat is different from temperature. Heat is energy that moves from one place or material to another because there is a difference in temperature. That difference in temperature keeps heat...

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thermometers and temperature scales

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gas thermometers and the kelvin scale

Kelvin Temperature and Gas Thermometer Standards

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thermal expansion

Thermal Expansion in Air, Water, and Solids

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thermal stress

How Temperature Changes Create Stress

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Golden Gate Bridge Thermal Expansion

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heat flow and specific heat

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phase changes

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calorimetry

Calorimetry studies heat exchange in an insulated system. A calorimeter is a container that prevents heat transfer in or out. Scientists use calorimetry to measure heat and specific heat capacity. A calorimetry problem is any situation where the objects are thermally isolated from their surroundings. The key idea comes from conservation of energy. During heat transfer, the heat gained by the colder object must equal the heat lost by the hotter object. A simple example is water poured into a...

mechanisms of heat transfer i

Three Ways Heat Moves Between Objects

Heat transfer happens when there is a temperature difference. It can move fast, like through a cooking pan, or slowly, like through the walls of a picnic ice box. Heat transfer appears in many everyday situations, so it is hard to find a place where it does not occur. There are only three ways heat is transferred: conduction, convection, and radiation. A fireplace shows all three at once. Radiation carries most of the heat into the room. Conduction also moves heat into the room, but much more...

mechanisms of heat transfer ii

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conduction, convection and radiation: problem solving

conduction-convection-and-radiation-problem-solving

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radiation: applications

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Radiation Heat Transfer and Thermographs

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key terms and concepts

Explore calorimetry through thermal equilibrium, insulated systems, and heat transfer. See how a hot pan and cooler water reach the same temperature.

Heat Exchange in an Insulated System | JoVE K12

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Minnesota Academic Standards in Science

9-12

1.2.1 9C.4.2.1.2

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New Jersey Student Learning Standards for Science

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Quantifying Heat

Thermal Energy&#160;

Microscopically, thermal energy is the kinetic energy associated with the random motion of atoms and molecules. Temperature is a ...

Temperature and Thermal Equilibrium

Heat and temperature are essential concepts for everyone every day. The study of heat and temperature is part of an area of physics known as ...

Types of Kinetic Energy

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Heat Flow and Specific Heat

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Kinetic Molecular Theory: Molecular Velocities, Temperature, and Kinetic Energy

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Constant Pressure Calorimetry

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Contrast the concepts of temperature and heat flow in macroscopic and microscopic terms. Understand that thermal energy is a form of energy and temperature is a measure of average kinetic energy of a particle. EXPLANATION: Students have been exposed to the types of energy (potential, kinetic, thermal, and chemical) and energy transfer (working, heating, and radiating) in the sixth grade. At that time, students classified energy types in systems and transformations. The focus in Chemistry 1 should be on understanding that measuring the temperature of a system is a way to quantify the thermal energy (average kinetic energy) of the particles in that system. Heating is a mechanism that transfers energy to or from a system. Students should also explore absolute vs relative scales of temperature mechanisms. Students should recognize that energy will always flow from objects with greater thermal energy to areas with lesser thermal energy, but rates of energy flow are a property of the materials being heated. The degree to which the temperature changes as an object is also a physical property of a material. Activities may include collecting or analyzing pressure vs temperature data, then considering why a graph of collected data does not pass through the origin. (Heat capacity and conductivity will only be assessed qualitatively.)

CHEM1.PS3.1

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When objects at different temperatures are placed in contact with each other but isolated from everything else, they attain thermal equilibrium. A ...

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Differential Scanning Calorimetry

Source: Danielle N. Beatty and Taylor D. Sparks, Department of Materials Science and Engineering, The University of Utah, Salt Lake City, UT
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Draw and interpret heating and cooling curves and phase diagrams. Analyze the energy changes involved in calorimetry by using the law of conservation of energy quantitatively (use of $q=mc\Delta T)$ and qualitatively. EXPLANATION: This is one of two standards where students are to investigate changes in a specific types of energy: In this case, thermal energy and phase energy. Starting as early as kindergarten, students are introduced to solid and liquid phases of matter. By third grade, students are considering the particulate nature of matter to discuss physical properties of the different phases. In fifth grade, students discuss phase changes from the perspective of the arrangement of particles. Chemistry 1 is the first time that students make a connection between phase changes and energy changes. Students commonly struggle with the idea that substances can be heated, but that heating does not always result in a change in temperature. Models of phase energies associated with the arrangement of particles aid in dispelling these misconceptions. Comparisons should identify similarities in energies in solids and liquids as compared to vastly different energy in gases. Discussions of heat of fusion/vaporization and calculations to enrich these discussions are appropriate. Finally, students should be able to quantify relationships in which heating creates a change in the thermal energy of a sample. Activities may include determining energy released when an object is burned to change the temperature of a substance in a closed system. (Note that this standard is limited to calculations of energy associated with changes in thermal energy, and not energies associated with phase transformations.)

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Activation Energy

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Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

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Bond Dissociation Energy and Activation Energy

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Distinguish between endothermic and exothermic reaction by constructing potential energy diagrams and explain the differences between the two using chemical terms (e.g. activation energy). Recognize when energy is absorbed or given off depending on the bonds formed and bonds broken. EXPLANATION: This is one of two standards where students are to investigate changes in a specific type of energy: In this case, chemical energy. Students should recognize that the formation of bonds releases energy, while the breaking of bonds is endothermic. Synthesis reactions to form metal oxides can provide observations if carried out taking proper precautions. Clear changes to masses and physical properties provide evidence of a reaction. (Specific discussions of enthalpy of formation are beyond the scope of this standard, but the topic may be useful for enrichment discussions about reactions where bonds are both broken and formed.)

CHEM1.PS3.3

Conservation of Energy: Application

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Conservation of Energy Approach to System Analysis

Source: Ricardo Mejia-Alvarez and Hussam Hikmat Jabbar, Department of Mechanical Engineering, Michigan State University, East Lansing, MI
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First Law of Thermodynamics

Energy Conservation

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Conservation of Mechanical Energy

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Energy and Work

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Conservative Forces

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Non-conservative Forces

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Energy Diagrams - I

The dynamics of a mechanical system can be easily understood by interpreting a potential energy diagram. Since energy is a scalar quantity, the ...

Energy Diagrams - II

Energy diagrams are important to understand the dynamics of a system. The topology of an energy diagram helps illustrate the equilibrium points of the ...

Analyze energy changes to explain and defend the law of conservation of energy. EXPLANATION: Standards PS3.2 and PS3.3 identify the energy types most commonly associated with chemical reactions and build on sixth grade discussions of energy storage and transfer types. In Chemistry 1, students will synthesize an understanding of law of conservation of energy by being able to distinguish system from surroundings, and recognizing that tracking energy requires both the system and surrounding energies to be considered. Students can consider interactions such as a beverage warming/cooling, a refrigerator cooling food, the function of Freon in cooling systems, or a car's cooling system as examples where multiple systems interact.

CHEM1.PS3.4

Heat Exchange in an Insulated System

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