Name: open, closed, and isolated systems
Uploaded: 2023-04-30T12:31:03.000Z
Duration: 1 min 6 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Energy

HS-PS3-1

Thermodynamic Systems

In der Thermodynamik werden die zu beobachtenden Objekte als System betrachtet, und alle umgebenden Objekte, die sich außerhalb der Systemgrenze befinden, sind die Umgebung.
Ein Auto, einschließlich des Kraftstoffs in seinem Kraftstofftank, kann als System betrachtet werden. Die Straße ist zusammen mit der Umgebung die Umgebung.
Steht das Auto, tauscht es keine Materie oder Energie mit der Umwelt aus. Ein solches System wird als isoliertes System bezeichnet.
Wenn der Automotor zündet, lassen die Kraftstoffverbrennung die Abgase aus, die Räder spüren die Reibungskraft durch die Straße und bewegen das Auto vorwärts. Hier werden sowohl Materie als auch Energie mit der Umgebung ausgetauscht, so dass das Auto in Bewegung als offenes System betrachtet werden kann.
Wenn der Motor des Autos ausgeschaltet wird, hält die Reibungskraft zwischen den Rädern des Autos und der Straße das Auto allmählich an. Hier wird nur Energie zwischen dem System und der Umgebung ausgetauscht. Ein solches System wird als geschlossenes System bezeichnet.

<ol>
 <li>Young, H.D., Freedman, RA Universitätsphysik mit moderner Physik. San Francisco, Kalifornien: Pearson. 624 (2012).</li>
 <li>OpenStax. Universitätsphysik Vol.2. Seite 110 [Webversion]. Abgerufen von <a href="https://openstax.org/books/university-physics-volume-2/pages/3-1-thermodynamic-systems.">https://openstax.org/books/university-physics-volume-2/pages/3-1-thermodynamic-systems.</a>.</li>
</ol>

thermodynamische systeme

Ein thermodynamisches System ist eine Gruppe von Objekten, deren thermodynamische Eigenschaften von Interesse sind. Das System wird als in seiner Umgebung oder der Umwelt eingebettet betrachtet. Das System und seine Umgebung können Wärme austauschen und sich gegenseitig Arbeit zuführen, wenn sie durch eine Grenze voneinander getrennt sind. Die unmittelbare Umgebung des Systems interagiert jedoch direkt mit ihm und hat daher einen viel stärkeren Einfluss auf sein Verhalten und seine Eigenschaften.

Betrachten wir ein Beispiel: Tee kocht in einem Wasserkocher. Der Tee und der Wasserkocher zusammen bilden ein System. Wenn der Deckel des Wasserkochers offen gehalten wird, entweicht Dampf aus dem kochenden Tee in die Umgebung, was ein Beispiel für ein offenes System ist. Wenn jedoch der Deckel des Wasserkochers geschlossen wird, kann der Dampf nicht entweichen, d.h. keine Materie kann entweichen, aber die Energie in Form von Wärme wird mit der Umgebung ausgetauscht. Daher wird es zu einem geschlossenen System.

Wenn der heiße Tee jedoch in eine Thermoskanne gegossen wird, kann weder Materie noch Energie für eine bestimmte Zeit mit der Umgebung ausgetauscht werden. Diese Art von System wird zu einem isolierten System.

In Wirklichkeit kann kein System unendlich isoliert sein. Im Fall einer Thermoskanne wird der Tee schließlich abkühlen, was darauf hinweist, dass ein Energieaustausch zwischen dem System und der Umgebung stattgefunden hat.

Wenn der Tee in der Thermoskanne die gleiche Temperatur wie die Umgebung erreicht, befinden sich das System und die Umgebung im thermischen Gleichgewicht.

In der Mechanik wird das Gleichgewicht durch das Gleichgewicht zwischen den Kräften und den Drehmomenten im System definiert. In der Thermodynamik ist es jedoch wichtig, die Wärmeübertragungsprozesse zwischen dem System und der Umgebung zu untersuchen, die zum thermischen Gleichgewicht des Systems führen. Das Konzept des thermischen Gleichgewichts führt letztlich zum Nullten Hauptsatz der Thermodynamik. Dieses Gesetz ist gleichermaßen auf die verschiedenen Teile eines geschlossenen Systems anwendbar und erfordert, dass die Temperatur überall im System gleich sein muss, wenn das System das thermische Gleichgewicht erreicht hat.

Thermodynamische Systeme

Ein thermodynamisches System ist eine Menge von Objekten, deren thermodynamische Eigenschaften von Interesse sind. Das System wird als in seine Umgebung eingebettet betrachtet oder ...

Education

Lehre

JoVE Core

Physics

Physik

Unit 1

Einheit 1

The First Law of Thermodynamics

Der erste Hauptsatz der Thermodynamik

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

open, closed, and isolated systems

A thermodynamic system is the part of the world that scientists study for its heat and energy behavior. It sits inside a surrounding environment, or surroundings. The system and the surroundings can exchange heat and do work across the boundary that separates them. The immediate surroundings affect the system most strongly because they interact with it directly.

A kettle of boiling tea shows how this works in everyday life. The tea and the kettle together form the system. If the lid is open, steam escapes into the surroundings. That makes it an open system because matter can leave.

If the lid is closed, steam cannot escape. Matter stays inside, but heat can still pass between the system and the surroundings. In that case, the kettle acts as a closed system. If the hot tea is poured into a thermos, then neither matter nor energy can be exchanged for a time. That is an isolated system.

In reality, no system stays isolated forever. The tea in the thermos will eventually cool down, which shows that energy exchange still occurred with the surroundings. When the tea and the surroundings reach the same temperature, they are in thermal equilibrium. In thermodynamics, this idea is more important than the force and torque balance used in mechanics.

Thermal equilibrium also leads to the Zeroth Law of Thermodynamics. This law applies to the different parts of a closed system as well. It states that if a system has reached thermal equilibrium, the temperature must be the same everywhere inside it.

Open, Closed, and Isolated Systems

thermodynamic systems

A thermodynamic system is the part of the world that scientists study for its heat and energy behavior. It sits inside a surrounding environment, or surroundings. The system and the surroundings can exchange heat and do work across the boundary that separates them. The immediate surroundings affect the system most strongly because they interact with it directly. A kettle of boiling tea shows how this works in everyday life. The tea and the kettle together form the system. If the lid is open,...

work done during volume change

Gas Work in a Piston Cylinder

Gas work in a piston cylinder describes how pressure and volume change are related in thermodynamics. In mechanics, work happens when a force moves an object. In thermodynamics, work done on a system can be estimated when the system changes volume during a process. A gas can be trapped in a cylinder with a movable piston at one end. When the gas expands from volume V1 to volume V2, it pushes on the piston and moves it by a small distance dr. If the pressure on the piston face is p and the...

path between thermodynamics states

Path Dependence in Gas Work

Work done by an ideal gas can depend on the path it takes between two thermodynamic states. The transcript compares two routes from state A to state C for the same gas. In both cases, the gas expands from volume V1 to volume V2, but the work is not the same. Along path AC, the gas stays at constant temperature T. It expands from V1 to V2. The work done by the gas is found from the pressure-volume relation for an ideal gas. After substituting pressure as nRT/V and integrating, the work for this...

heat and free expansion

Two Gas Paths to the Same Volume

Heat added to a thermodynamic system can lead to the same final state through different paths. The path matters because work and heat depend not only on the initial and final states, but also on the steps in between. In this topic, an ideal gas is used to show two different ways to reach the same volume. In the first case, the gas is in a cylinder with a piston and is heated at a constant temperature. As the gas molecules absorb energy, the gas expands slowly in a controlled isothermal process.

internal energy

How Internal Energy Changes in Gas Systems

Internal energy is the energy stored inside a thermodynamic system. It is the sum of the kinetic and potential energies of the molecules or other particles in the system. Molecular kinetic energy includes translational motion, rotation, and vibration. Molecular potential energy comes from interactions between molecules. A system’s location and overall motion do not affect its internal energy. For an ideal monatomic gas, each particle is a single atom. That means there is no rotational or...

first law of thermodynamics

Heat, Work, and Internal Energy

Heat, work, and internal energy are linked by the first law of thermodynamics. This law is a generalized form of energy conservation. It explains how energy changes when heat is added to or removed from a system, and when the system does work or has work done on it. The change in internal energy equals the heat transferred into the system minus the work done by the system. Added heat increases internal energy. For that reason, heat is taken as positive when it enters the system and negative...

first law of thermodynamics: problem-solving

first-law-of-thermodynamics-problem-solving

First Law of Thermodynamics: Solving Problems

The first law of thermodynamics links internal energy, heat, and work. It states that the change in internal energy of a system equals the net heat transfer into the system minus the net work done by the system. This is a general form of energy conservation, and it can be used for any thermodynamic process. To solve a first-law problem, start by identifying the thermodynamic system. Then list the initial and final states of the process. Next, identify the known and unknown quantities. It is...

cyclic processes and isolated systems

Net Work in a Cyclic Thermodynamic Process

A cyclic thermodynamic process returns a system to its initial state. In a cycle, the change in internal energy is zero. An isolated system is different because it has zero heat exchange and zero work, so its internal energy stays constant. For a non-isolated system, the internal energy change is zero only when the process is cyclic. The first law of thermodynamics relates internal energy, heat transfer, and work. It states that the change in internal energy is the difference between the net...

isothermal processes

Isothermal Expansion and Heat Transfer

An isothermal process is a thermodynamic process that happens at constant temperature. During the process, heat slowly flows into the system or out of the system so thermal equilibrium is maintained. Phase changes are common examples of isothermal processes. Water can evaporate into steam at a constant temperature, and water can also freeze into ice at a constant temperature. An ideal gas can also undergo isothermal expansion or compression. Here, an ideal gas in an isolated cylinder expands...

isochoric and isobaric processes

Constant Volume and Pressure in Thermodynamics

Thermodynamic processes can happen at constant volume or at constant pressure. An isochoric process is a constant-volume process. In this case, the volume does not change, so the work done by the system is zero. The first law of thermodynamics still applies, so any heat added or removed changes the internal energy of the system only. A simple example is heating 1000 g of water from 40 degrees celsius to 70 degrees celsius at constant volume. Because the process is isochoric, no work is done by...

heat capacities of an ideal gas i

Ideal Gas Heat Capacity at Constant Pressure

Heat capacity describes how much heat a substance absorbs for a given change in temperature. It is also called thermal capacity, and its SI unit is J/K. Specific heat capacity is the heat needed to raise the temperature of 1 kg of a substance by 1 K, and its SI unit is J/kg·K. The video also explains molar heat capacity. This is the amount of heat added or removed to change the temperature of 1 mole of a substance by 1 K. It can be measured at constant volume or constant pressure, and it is...

heat capacities of an ideal gas ii

Ideal Gas Heat Capacity Differences

Ideal gas heat capacities depend on whether the gas is heated at constant volume or constant pressure. At constant volume, the heat absorbed only raises the internal energy of the system. No work is done in this case. At constant pressure, the situation is different. The heat absorbed increases the internal energy and also does work. Molar heat capacity is the heat needed to raise the temperature of 1 mole of gas by 1 unit. Because some of the added heat goes into work, more heat is needed at...

heat capacities of an ideal gas iii

Ideal Gas Heat Capacity and Degrees of Freedom

Ideal gas heat capacity depends on degrees of freedom, which are the independent ways a gas molecule can move, rotate, and vibrate. If d is the number of degrees of freedom, the molar heat capacity at constant volume can be written in terms of d. The molar heat capacity at constant pressure can also be written using the relationship between the two heat capacities. The ratio of molar heat capacity at constant pressure to molar heat capacity at constant volume is called the ratio of heat...

adiabatic processes for an ideal gas

Gas Temperature Changes in Adiabatic Processes

Adiabatic processes change the temperature of an ideal gas without heat transfer. In an adiabatic compression, no heat is added, but work is done on the gas. That work raises the gas temperature. In an adiabatic expansion, the gas does work and its temperature drops. A common example is the compression of a gas-air mixture inside a car engine cylinder. The compression happens so quickly that there is no time for heat to move between the mixture and its surroundings. Even so, the work done on...

pressure and volume in an adiabatic process

pressure-and-volume-in-an-adiabatic-process

Free Expansion: Pressure, Volume, and Temperature

Free expansion shows how pressure, volume, and temperature behave when a gas expands without doing work. It is an adiabatic process, but it is not the same as adiabatic expansion. In free expansion, no work is done and the internal energy does not change. In adiabatic expansion, work is done and the internal energy changes. For an adiabatic process, the pressure-volume relation comes from the adiabatic condition. That relation does not apply to free expansion, even though the expansion is...

work done in an adiabatic process

Adiabatic Compression in an Engine Cylinder

Adiabatic compression in an engine cylinder changes the pressure, temperature, and volume of a gas-air mixture. In this setup, gasoline vapor is injected into the cylinder when the piston is in its expanded position. The mixture starts at 20 °C, 1.00 x 10^5 N/m^2, and 240 cm^3. The mixture is then compressed adiabatically to 40 cm^3. Adiabatic means no heat is exchanged with the surroundings during the process. For this calculation, the compression is treated as quasi-static, even though real...

thermodynamic potentials

Energy Forms in Thermodynamics

Thermodynamic potentials are energy-based state functions used to analyze a thermodynamic system. They help describe how a system changes under different conditions. The four main thermodynamic potentials are internal energy, enthalpy, Helmholtz free energy, and Gibbs free energy. These potentials can be written using two of the variables pressure, volume, temperature, and entropy. In each case, the rate of change of the potential with respect to the other two variables gives useful...

maxwell's thermodynamic relations

Using Maxwell's Relations in Thermodynamics

Maxwell's thermodynamic relations help solve problems in thermodynamics. They connect partial differentials for quantities that are hard to measure in the lab with quantities that are easier to measure. This makes them useful for working with temperature, pressure, volume, and entropy. These relations come from thermodynamic potentials and the symmetry of second derivatives. Thermodynamic potentials are exact differentials, so the order of second differentiation does not change the result.

joule-thomson effect

Gas Cooling and Heating in Throttling

Gas cooling and heating in throttling is explained by the Joule-Thomson effect, also called the Joule-Kelvin effect. It describes how a fluid changes temperature when it passes through a valve or porous plug in a thermally insulated system. This type of flow is called a throttling process. In the experiment, a high-pressure gas is forced through a throttle valve or porous plug into a lower-pressure region. The gas expands as it moves into the larger volume. Work is done on the gas as it is...

key terms and concepts

Learn how open, closed, and isolated thermodynamic systems exchange matter and energy, using a boiling tea kettle and thermos example for high school science.

Open, Closed, and Isolated Systems | JoVE K12

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Open and Closed Systems.

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HS-PS3-6

Open, Closed, and Isolated Systems

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