Name: chemical equilibrium and kc rules
Uploaded: 2025-08-11T09:37:07.000Z
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NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.5.2

The Equilibrium Constant

Das Gesetz der Massenwirkung führt die Gleichgewichtskonstante ein, um die Gleichgewichtskonzentrationen der Reaktanten und Produkte in Beziehung zu setzen.
Für eine ausgeglichene chemische Gleichung, in der A und B Reaktanten, C und D Produkte und die Kleinbuchstaben a, b, c und d ihre jeweiligen stöchiometrischen Koeffizienten sind, ergibt sich der Ausdruck der Gleichgewichtskonstante aus den molaren Konzentrationen der Produkte dividiert durch die molaren Konzentrationen der Reaktanten, die alle auf ihre stöchiometrischen Koeffizienten angehoben werden.
Die Gleichgewichtskonstante wird oft mit dem Symbol K oder Kc ausgedrückt, wobei der Index c die Gleichgewichtskonstante in Bezug auf die molare Konzentration angibt. Da es sich um ein Verhältnis der molaren Konzentrationen handelt, ist die Gleichgewichtskonstante einheitenlos.
Eine große Gleichgewichtskonstante viel größer als 1 bedeutet, dass der Zähler, d.h. die Konzentration der Produkte, größer ist als der Nenner, die Konzentration der Reaktanten. Dies deutet darauf hin, dass das Gleichgewicht zu den Produkten hin liegt und die Vorwärtsreaktion begünstigt.
Umgekehrt bedeutet eine kleine Gleichgewichtskonstante, die viel kleiner als 1 ist, dass der Nenner größer als der Zähler ist. Dies bedeutet, dass das Gleichgewicht in Richtung der Reaktanten liegt und die Umkehrreaktion begünstigt.
Bei einer Gleichgewichtskonstante der Größenordnung von 1 oder nahe 1 sind die relativen Konzentrationen der Reaktanten und Produkte nahezu gleich. Dies deutet darauf hin, dass weder die Reaktion, vorwärts noch rückwärts, begünstigt wird.
Modifikationen der chemischen Gleichung verändern auch die Gleichgewichtskonstante.
Wenn eine chemische Reaktion mit einer Gleichgewichtskonstante x umgekehrt wird, ist der Gleichgewichtskonstantenausdruck für die Umkehrreaktion der Kehrwert der Vorwärtsreaktion. Die neue Gleichgewichtskonstante wäre also 1 über x.
Wenn die Koeffizienten mit einem anderen Faktor n multipliziert werden, wird die Gleichgewichtskonstante auf denselben Faktor angehoben. Die neue Gleichgewichtskonstante wäre nun xn.
Wenn zwei oder mehr Einzelreaktionen addiert werden, ist die Gleichgewichtskonstante für die Gesamtreaktion das Produkt der einzelnen Gleichgewichtskonstanten. Die neue Gleichgewichtskonstante wäre also y × z.
Für ein heterogenes Gleichgewicht schließt der Gleichgewichtskonstantenausdruck reine feste oder reine flüssige Einheiten aus.
Zum Beispiel schließt der Gleichgewichtskonstantenausdruck für die Zersetzung von festem Ammoniumnitrat zu gasförmigem Distickstoffmonoxid und Wasserdampf Ammoniumnitrat – einen reinen Feststoff – aus.
Dies liegt daran, dass die relative molare Konzentration eines reinen Feststoffs oder einer Flüssigkeit während der Reaktion konstant bleibt.

die gleichgewichtskonstante

Betrachten Sie die Oxidation von Schwefeldioxid:

 <img alt="Eq1" src="/files/ftp_upload/11386/11386_Equation_1.png" style="text-align: center; height: 50px;">

 Bei einer Reaktion, die nur mit einer Mischung von Reaktanten beginnt, ist die Produktkonzentration zunächst gleich Null. Während sich die Reaktion in Vorwärtsrichtung dem Gleichgewicht nähert, nehmen die Reaktantenkonzentrationen ab und die Produktkonzentration zu. Wenn das Gleichgewicht erreicht ist, bleiben die Konzentrationen der Reaktanten und Produkte konstant.

 Wenn die Reaktion nur mit den vorhandenen Produkten beginnt, verläuft die Reaktion in umgekehrter Richtung zum Gleichgewicht hin. Die Produktkonzentration nimmt mit der Zeit ab und die Reaktantenkonzentrationen steigen, bis die Konzentrationen im Gleichgewicht konstant werden.

 Das Massenwirkungsgesetz besagt, dass das Verhältnis der Produktkonzentration zur Konzentration der Reaktanten im Gleichgewicht, erhöht auf ihre jeweiligen stöchiometrischen Koeffizienten, einer Konstante entspricht, die als Gleichgewichtskonstante K oder Kc bezeichnet wird. Somit wird der Ausdruck der Gleichgewichtskonstante für die obige Reaktion wie folgt geschrieben: 

 <img alt="Eq2" src="/files/ftp_upload/11386/11386_Equation_2.png" style="text-align: center; height: 100px;">

 Dabei gibt der Index „c“ an, dass die Gleichgewichtskonstante die molare Konzentration von Reaktanten und Produkten berücksichtigt.

 Die Größe der Gleichgewichtskonstante spiegelt explizit die Zusammensetzung einer Reaktionsmischung im Gleichgewicht wider. Eine Reaktion mit einem großen K erreicht das Gleichgewicht, wenn der größte Teil des Reaktanten in das Produkt umgewandelt wurde, wohingegen ein kleiner K anzeigt, dass die Reaktion das Gleichgewicht erreicht, nachdem nur sehr wenig Reaktant umgewandelt wurde. Es ist wichtig zu bedenken, dass die Größe von K keinen Hinweis darauf gibt, wie schnell oder langsam das Gleichgewicht erreicht wird. Manche Gleichgewichte stellen sich so schnell ein, dass sie nahezu augenblicklich erfolgen, andere so langsam, dass im Laufe von Tagen, Jahren oder länger keine wahrnehmbare Veränderung zu beobachten ist. Die Gleichgewichtskonstante einer Reaktion kann verwendet werden, um das Verhalten von Gemischen vorherzusagen, die ihre Reaktanten und/oder Produkte enthalten. Wie der oben beschriebene Schwefeldioxid-Oxidationsprozess zeigt, verläuft eine chemische Reaktion in jede Richtung, die zum Erreichen eines Gleichgewichts erforderlich ist.

 Gekoppelte Gleichgewichte 

 <ul style="padding-left: 35px; list-style-type: disc;">
 Viele Gleichgewichtssysteme beinhalten zwei oder mehr gekoppelte Gleichgewichtsreaktionen, denen ein oder mehrere Reaktanten- oder Produktspezies gemeinsam sind. Der K-Wert für ein System mit gekoppelten Gleichgewichten kann mit den K-Werten der einzelnen Reaktionen in Beziehung gesetzt werden. Bei diesem Ansatz sind drei grundlegende Manipulationen erforderlich, die im Folgenden beschrieben werden:
 <li>Wenn man die Richtung einer chemischen Gleichung ändert, werden im Wesentlichen die Identitäten von „Reaktanten“ und „Produkten“ vertauscht, sodass die Gleichgewichtskonstante für die umgekehrte Gleichung einfach der Kehrwert derjenigen für die Vorwärtsgleichung ist.</li>
 <li>Eine Änderung der stöchiometrischen Koeffizienten in einer Gleichung um einen Faktor x führt zu einer exponentiellen Änderung der Gleichgewichtskonstante um denselben Faktor.</li>
 <li>Die Addition von zwei oder mehr Gleichgewichtsgleichungen ergibt eine Gesamtgleichung, deren Gleichgewichtskonstante das mathematische Produkt der K-Werte der einzelnen Reaktion ist.</li>
 </ul>

 Gleichgewichtskonstanter Ausdruck für heterogene Gleichgewichte

 Bei heterogenen Gleichgewichten, an denen Reaktanten und Produkte in zwei oder mehr verschiedenen Phasen beteiligt sind, sind die Konzentrationen reiner Feststoffe oder reiner Flüssigkeiten nicht im Gleichgewichtskonstantenausdruck enthalten, wie das folgende Beispiel zeigt: <img alt="Eq3" src="/files/ftp_upload/11386/11386_Equation_3.png" style="text-align: center; height: 150px;"> Dies liegt daran, dass die relativen Konzentrationen für reine Flüssigkeiten und reine Feststoffe während der Reaktion konstant bleiben. 

 Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/13-2-equilibrium-constants">Openstax, Chemistry 2e, Section 13.2 Equilibrium Constants</a>

Die Gleichgewichtskonstante

Betrachten Sie die Oxidation von Schwefeldioxid:

Bei einer Reaktion, die nur mit einem Gemisch von Reaktanten beginnt, beträgt die Produktkonzentration zunächst ...

Education

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JoVE Core

Chemie

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Chemical Equilibrium

Chemisches Gleichgewicht

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

chemical equilibrium and kc rules

Chemical equilibrium and the equilibrium constant Kc describe how reactants and products are balanced in a reaction. In the oxidation of sulfur dioxide, a mixture that starts with reactants only has no product at first. As the reaction moves forward toward equilibrium, reactant concentrations decrease and product concentration increases. When equilibrium is reached, the concentrations of both stay constant.

A reaction can also begin with only products present. In that case, the reaction moves in reverse toward equilibrium. The product concentration falls with time, and the reactant concentrations rise until both become constant. This shows that a chemical reaction will move in whatever direction is needed to reach equilibrium.

The law of mass action links equilibrium to a constant value. It states that the ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients, equals the equilibrium constant, K or Kc. The subscript c means the expression uses molar concentration. The size of K shows the mixture makeup at equilibrium. A large K means most reactant has changed to product before equilibrium is reached. A small K means only a little reactant changes to product. The value of K does not tell how fast equilibrium is reached.

Some equilibria form very quickly. Others take so long that no visible change may be seen for days, years, or longer. The equilibrium constant can still be used to predict how a mixture with reactants and/or products will behave. For coupled equilibria, two or more equilibrium reactions share one or more species. The K value for the overall system can be found from the K values of the separate reactions. Reversing a chemical equation changes K to its reciprocal. Multiplying the stoichiometric coefficients by a factor x changes K by that same factor as an exponent. Adding equilibrium equations gives an overall K equal to the product of the individual K values.

For heterogeneous equilibria, the reactants and products are in different phases. Pure solids and pure liquids are not included in the equilibrium constant expression. Their concentrations stay constant during the reaction, so they do not change the value of K. This rule is an important part of writing equilibrium expressions correctly.

Chemical Equilibrium and Kc Rules

the equilibrium constant

Chemical equilibrium and the equilibrium constant Kc describe how reactants and products are balanced in a reaction. In the oxidation of sulfur dioxide, a mixture that starts with reactants only has no product at first. As the reaction moves forward toward equilibrium, reactant concentrations decrease and product concentration increases. When equilibrium is reached, the concentrations of both stay constant. A reaction can also begin with only products present. In that case, the reaction moves...

le chatelier's principle: changing concentration

le-chatelier-s-principle-changing-concentration

Shifting Equilibrium by Changing Concentration

Chemical equilibrium is a dynamic balance. At equilibrium, the forward and reverse reactions happen at equal rates. If the system is stressed in a way that changes one rate more than the other, it is no longer at equilibrium and will shift until balance is restored. This behavior is described by Le Châtelier’s principle. Changes in concentration are a major stress on an equilibrium system. Reaction rates depend mainly on concentration and temperature. For that reason, changing the amount of a...

homogeneous equilibria for gaseous reactions

homogeneous-equilibria-for-gaseous-reactions

Relating Kc and Kp in Gas Equilibria

Gas-phase equilibrium can be written using either concentration or pressure. The equilibrium constant may be shown as Kc, which uses molar concentration, or as Kp, which uses partial pressure of the reactants and products. The link between Kc and Kp comes from the ideal gas equation and the definition of molarity. Molarity is the number of moles divided by volume. In the ideal gas equation, P stands for partial pressure, V for volume, n for number of moles, R for the gas constant, and T for...

calculating the equilibrium constant

Finding Kc from Equilibrium Data

The equilibrium constant, Kc, can be found from the equilibrium concentrations of reactants and products. When those concentrations are known, the calculation is straightforward. The values are placed into the Kc expression for the reaction. One example uses nitrogen dioxide and dinitrogen tetroxide. When 0.10 mol NO2 is added to a 1.0-L flask at 25 °C, the concentrations change until equilibrium is reached. At equilibrium, [NO2] is 0.016 M and [N2O4] is 0.042 M, and these values are used to...

reaction quotient

Using Q to Track Equilibrium Changes

Reaction quotient Q helps track how far a reversible reaction has moved toward equilibrium. For a balanced reaction such as m A + n B ⇌ x C + y D, Q comes directly from the stoichiometric coefficients in the equation. When concentrations are used, the expression is written as Qc. For gases, a similar form uses partial pressures. These expressions use relative concentration and pressure values, not absolute values. That means reaction quotients are dimensionless and have no units. As a reaction...

dynamic equilibrium

Chemical Equilibrium in Reversible Reactions

Chemical equilibrium in reversible reactions happens when a reaction moves in both directions at the same time. A reversible reaction uses a double arrow to show that products can turn back into reactants. At equilibrium, the concentrations of reactants and products stay constant over time because the forward and reverse reaction rates are equal. The video uses the reversible decomposition of colorless dinitrogen tetroxide to brown nitrogen dioxide as an example. At time zero, there is finite...

calculating equilibrium concentrations

Equilibrium Concentrations from an ICE Table

Equilibrium concentrations can be found from initial concentrations and an equilibrium constant. This skill matters in many areas of science and technology, including pharmaceutical product formulation and dosing. After a drug is ingested or injected, it may take part in several chemical equilibria that change its final concentration in the body system of interest. Scientists use these quantitative equilibrium relationships to help calculate a dosage that will produce the desired therapeutic...

le chatelier's principle: changing volume (pressure)

le-chatelier-s-principle-changing-volume-pressure

Gas Equilibrium Under Volume Changes

Gas-phase equilibrium can shift when the volume of the system changes. In these reactions, a change in pressure changes concentration because the partial pressure of an ideal gas is proportional to its molar concentration. That means pressure changes affect equilibrium in the same way as concentration changes. When the volume of a gas mixture changes, the concentrations of reactants and products change together. Since every gas in the equilibrium occupies the same space, the same volume change...

le chatelier's principle: changing temperature

le-chatelier-s-principle-changing-temperature

Le Chatelier's Principle in Heating and Cooling

Le Chatelier's principle helps explain how chemical equilibrium responds to heating and cooling. A system at equilibrium will shift to restore balance after a temperature change, but the equilibrium constant, K, will not stay the same. Instead, the mixture reaches a new equilibrium with a different composition. This temperature effect is different from a concentration change, which shifts equilibrium without changing K. To understand why temperature matters, the reaction can be written with...

the small x assumption

Estimating Equilibrium with Small Changes

A small equilibrium constant can make equilibrium calculations easier. In these reactions, the equilibrium position favors the reactants. When the initial reactant concentration is high and the Kc value is small, the change in concentration may be negligible. In that case, the equilibrium concentration is close to the initial concentration. This idea helps simplify weak acid and weak base problems. Chemists can assume that some equilibrium concentrations are equal to the initial concentrations.

key terms and concepts

Explore chemical equilibrium, Kc, and the law of mass action. Learn how concentration changes, reaction direction, and mixed-phase equilibria shape equilibrium expressions.

Chemical Equilibrium and Kc Rules | JoVE K12

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Chemical Reactions

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New York State Science Learning Standards

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Chemical Equilibrium and Kc Rules

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