Name: energy forms in thermodynamics
Uploaded: 2023-09-18T17:11:17.000Z
Duration: 1 min 26 s
Channel: JoVE

K12 Standards

Florida Department of Education

High School

Physical Science

SC.912.P.10

SC.912.P.10.2

Thermodynamic Potentials

Potencjały termodynamiczne to funkcje stanu, które opisują stan układu jako funkcję zmiennych termodynamicznych.
Energia wewnętrzna jest funkcją entropii i objętości. Temperaturę i ciśnienie można wyrazić jako częściową różnicę energii wewnętrznej odpowiednio przy stałej objętości i entropii.
Entalpia jest równa sumie energii wewnętrznej układu oraz iloczynu jego ciśnienia i objętości. Różnicowanie i podstawianie dU zmniejsza entalpię w funkcji entropii i ciśnienia. Tak więc temperaturę i objętość uzyskuje się jako częściowe różnice entalpii.
Energia swobodna Helmholtza jest podawana jako energia wewnętrzna pomniejszona o iloczyn temperatury i entropii układu. Dla nieskończenie małej zmiany równanie staje się funkcją objętości i temperatury. Tak więc entropia i ciśnienie są określane za pomocą częściowej różnicy energii swobodnej Helmholtza.
Zastąpienie energii wewnętrznej entalpią przekształca energię swobodną Helmholtza w energię swobodną Gibbsa. Różnicowanie i upraszczanie jeszcze bardziej redukuje równanie do funkcji temperatury i ciśnienia. Podobne obliczenia wyrażają entropię i objętość jako cząstkową pochodną energii swobodnej Gibbsa.

<ol>
	<li>Blundell, SJ i Blundell, KM (2010). Pojęcia w fizyce cieplnej. Wydanie drugie. Nowy Jork, USA: Oxford University Press. s. 172.</li>
	<li>Rex, A (2017). Fizyka termiczna Finna. Wydanie trzecie. Boca Raton, Floryda: CRC Press. str. 163.</li>
</ol>

potencjały termodynamiczne

Potencjały termodynamiczne to funkcje stanu niezwykle przydatne w analizie układu termodynamicznego. Mają wymiary energetyczne. Cztery ważne potencjały termodynamiczne to energia wewnętrzna, entalpia, energia swobodna Helmholtza i energia swobodna Gibbsa. Te potencjały termodynamiczne można wyrazić za pomocą dwóch z następujących zmiennych: ciśnienia, objętości, temperatury i entropii. Te dwie zmienne wyraża się jako szybkość zmian potencjału termodynamicznego w odniesieniu do pozostałych dwóch zmiennych.

Energia wewnętrzna opiera się na udziale cząsteczek' energia potencjalna i kinetyczna układu. Jest to funkcja entropii i objętości. Dlatego pozostałe dwie zmienne, tj. temperaturę i ciśnienie, można wyrazić jako cząstkową różnicę energii wewnętrznej, odpowiednio przy stałej objętości i entropii.

Entalpia odnosi się do zawartości ciepła w systemie i jest funkcją entropii i ciśnienia. Jeśli entropia i ciśnienie są stałe, zmiana entalpii jest równa ciepłu przekazanemu do układu. W przypadku odwracalnego procesu izobarycznego entalpia reprezentuje ciepło pochłonięte przez układ. Wyrażenia temperatury i objętości można uzyskać z pochodnej cząstkowej entalpii odpowiednio względem entropii i ciśnienia.

Bezpłatna energia Helmholtza mierzy „użyteczną” energię praca uzyskana w zamkniętym układzie termodynamicznym przy stałej temperaturze i objętości. System działa na swoje otoczenie, dopóki jego energia swobodna Helmholtza nie osiągnie minimum. Entropię i ciśnienie można wyrazić jako pochodną cząstkową energii swobodnej Helmholtza odpowiednio względem temperatury i ciśnienia.

Darmowa energia Gibbsa jest wykorzystywana w problemach, w których ważnymi zmiennymi są ciśnienie i temperatura. Mierzy maksymalną pracę wykonaną w układzie termodynamicznym, gdy temperatura i ciśnienie są stałe. Wyrażenia entropii i objętości można uzyskać poprzez częściowe różniczkowanie energii swobodnej Gibbsa odpowiednio w odniesieniu do temperatury i ciśnienia.

Potencjały termodynamiczne

Potencjały termodynamiczne to funkcje stanu, które są niezwykle przydatne w analizie układu termodynamicznego. Mają one wymiary energii. Czwórka ...

Education

JoVE Core

Physics

Fizyka

Unit 1

Jednostka 1

The First Law of Thermodynamics

Pierwsza zasada termodynamiki

KEY TERMS AND CONCEPTS

Kluczowe terminy i pojęcia

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 information about the system. This makes thermodynamic potentials a practical way to connect energy changes with measurable conditions.

Internal energy comes from the potential and kinetic energy of the molecules inside a system. It is a function of entropy and volume. From internal energy, temperature and pressure can be found using partial derivatives at constant volume and constant entropy, respectively.

Enthalpy describes the heat content of a system. It is a function of entropy and pressure. When entropy and pressure stay constant, the change in enthalpy equals the heat transferred to the system. For a reversible isobaric process, enthalpy shows the heat absorbed by the system. Temperature and volume can also be obtained from the partial derivatives of enthalpy with respect to entropy and pressure.

Helmholtz free energy measures the useful work from a closed thermodynamic system at constant temperature and volume. The system does work on its surroundings until this free energy reaches a minimum. Entropy and pressure can be written as partial derivatives of Helmholtz free energy with respect to temperature and pressure.

Gibbs free energy is useful when pressure and temperature are the key variables. It gives the maximum work done in a thermodynamic system when temperature and pressure are constant. Entropy and volume can be found from the partial derivatives of Gibbs free energy with respect to temperature and pressure.

Energy Forms in Thermodynamics

thermodynamic systems

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,...

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

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

Explore the four thermodynamic potentials—internal energy, enthalpy, Helmholtz free energy, and Gibbs free energy—and how they relate to heat, work, and state variables.

Energy Forms in Thermodynamics | JoVE K12

physics

JoVE Core Physics introduces the theory and application of fundamental physics topics, including kinematics, dynamics, fluid mechanics, statics, waves, and acoustics, with concise and easy-to-understand animated videos. Additionally, the scientist-in-action videos demonstrate the application of related concepts in classical and original research experiments performed in today's laboratories worldwide.

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Work Done During Volume Change

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Path Between Thermodynamics States

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SC.912.P.10.6

A. Energy is involved in all physical and chemical processes. It is conserved, and can be transformed from one form to another and into work. At the atomic and nuclear levels energy is not continuous but exists in discrete amounts. Energy and mass are related through Einstein's equation E=mc2.

B. The properties of atomic nuclei are responsible for energy-related phenomena such as radioactivity, fission and fusion.

C. Changes in entropy and energy that accompany chemical reactions influence reaction paths. Chemical reactions result in the release or absorption of energy.

D. The theory of electromagnetism explains that electricity and magnetism are closely related. Electric charges are the source of electric fields. Moving charges generate magnetic fields.

E. Waves are the propagation of a disturbance. They transport energy and momentum but do not transport matter.

Energy Forms in Thermodynamics

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