Name: shifting equilibrium by changing concentration
Uploaded: 2020-09-24T15:06:50.000Z
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Le Chatelier's Principle: Changing Concentration

Ein System befindet sich im dynamischen Gleichgewicht, wenn die Geschwindigkeit der Vorwärtsreaktion der Geschwindigkeit der Rückreaktion entspricht. Obwohl die Reaktion immer noch in beide Richtungen abläuft, bleiben die Nettokonzentrationen von Reaktanten und Produkten konstant.
Wenn an diesem Punkt die Konzentration eines Reaktanten oder Produkts verändert wird, z. B. durch Zugabe von zusätzlichem Molekül A oder durch Entfernen eines Moleküls C, wird das Gleichgewicht gestört. Solche Veränderungen sind Belastungen für das System.
Nach dem Prinzip von Le Châtelier verschiebt sich die Gleichgewichtsposition, wenn ein Gleichgewichtssystem aufgrund einer Änderung der Konzentration, einer Änderung des Volumens oder des Drucks oder einer Temperaturänderung belastet wird, um die Belastung zu minimieren und das Gleichgewicht wiederherzustellen.
Um die Reaktion eines Systems auf Konzentrationsänderungen zu verstehen, betrachten Sie zwei miteinander verbundene Wassertanks, A und B. Anfangs ist der Wasserstand in den beiden Tanks gleich und das System befindet sich im Gleichgewicht. Dann wird Wasser in Tank B gegeben.
Dieser Stress lässt den Wasserstand im Tank B ansteigen und stört das Gleichgewicht. Um diese Belastung auszugleichen, fließt ein Teil des Wassers in Tank A, um das Gleichgewicht wiederherzustellen.
Wird hingegen Wasser aus Tank B entnommen, löst das Absenken des Wasserspiegels ebenfalls Stress aus.
Folglich fließt Wasser aus Tank A in Tank B, um das Gleichgewicht wiederherzustellen.
Für ein System im Gleichgewicht ist der Reaktionsquotient gleich der Gleichgewichtskonstante. Die Zugabe von mehr Reaktanten zum Gleichgewichtsgemisch verringert die Güte. Nach dem Prinzip von Le Châtelier minimiert das System diese Spannung, indem es die Gleichgewichtsposition in Richtung der Produkte verschiebt, um den zugesetzten Reaktanten zu verbrauchen und das Gleichgewicht wiederherzustellen. 
Ebenso führt das Entfernen eines Produkts aus dem Gleichgewichtsgemisch zu einer ähnlichen Reaktion, um das Gleichgewicht wiederherzustellen.
Im Gegensatz dazu erhöht das Hinzufügen weiterer Produkte die Q. Somit verschiebt sich die Gleichgewichtsposition in Richtung der Reaktanten, um das zugegebene Produkt zu verbrauchen und das Gleichgewicht wiederherzustellen.
Eine Änderung der Konzentration verschiebt die Gleichgewichtsposition, ohne den Wert von K zu verändern.

das prinzip von le chatelier: konzentration ändern

Ein System im Gleichgewicht befindet sich in einem dynamischen Gleichgewichtszustand, wobei Vorwärts- und Rückreaktionen mit gleichen Geschwindigkeiten ablaufen. Wenn ein Gleichgewichtssystem einer Änderung der Bedingungen ausgesetzt ist, die sich unterschiedlich auf diese Reaktionsgeschwindigkeiten auswirkt (ein Stress), dann sind die Geschwindigkeiten nicht mehr gleich und das System befindet sich nicht im Gleichgewicht. Anschließend erfährt das System eine Nettoreaktion in Richtung einer größeren Geschwindigkeit (eine Verschiebung), die das Gleichgewicht wiederherstellt. Dieses Phänomen wird durch das Prinzip von Le Châtelier zusammengefasst: Wenn ein Gleichgewichtssystem unter Stress steht, erfährt das System als Reaktion auf den Stress eine Verschiebung, die das Gleichgewicht wiederherstellt. Die Reaktionsgeschwindigkeiten werden hauptsächlich durch Konzentrationen beeinflusst, wie durch das Geschwindigkeitsgesetz der Reaktion beschrieben, und durch die Temperatur, wie durch die Arrhenius-Gleichung beschrieben. Folglich sind Konzentrations- und Temperaturänderungen die beiden Spannungen, die ein Gleichgewicht verschieben können. Auswirkung einer Konzentrationsänderung Wenn ein Gleichgewichtssystem einer Konzentrationsänderung eines Reaktanten oder einer Produktart unterliegt, ändert sich die Geschwindigkeit der Vorwärts- oder Rückreaktion. Betrachten Sie als Beispiel die Gleichgewichtsreaktion: <img alt="Eq1" src="/files/ftp_upload/11391/11391_Equation 1v2.png" style="text-align: center; height: 48px;"> Wenn sich dieses System im Gleichgewicht befindet, sind die Geschwindigkeiten der Vorwärts- und Rückreaktion gleich. <img alt="Eq2" src="/files/ftp_upload/11391/11391_Equation 2.png" style="text-align: center; height: 50px;"> Wenn das System durch die Zugabe von Reaktanten, entweder N2 oder O2, belastet wird, führt der resultierende Konzentrationsanstieg dazu, dass die Geschwindigkeit der Vorwärtsreaktion zunimmt und die der Rückreaktion übersteigt: <img alt="Eq3" src="/files/ftp_upload/11391/11391_Equation 3.png" style="text-align: center; height: 50px;"> Das System erfährt eine vorübergehende Nettoreaktion in Vorwärtsrichtung, um das Gleichgewicht wiederherzustellen (das Gleichgewicht verschiebt sich nach rechts). Die gleiche Verschiebung ergibt sich, wenn etwas Produkt-NO aus dem System entfernt wird, was die Geschwindigkeit der Rückreaktion verringert, was wiederum zu demselben Ungleichgewicht in den Geschwindigkeiten führt. Die gleiche Logik kann verwendet werden, um die Linksverschiebung zu erklären, die sich aus der Entfernung von Reaktanten oder der Zugabe von Produkten zu einem Gleichgewichtssystem ergibt. Beide Belastungen führen zu einer erhöhten Geschwindigkeit der Rückreaktion <img alt="Eq4" src="/files/ftp_upload/11391/11391_Equation 4.png" style="text-align: center; height: 50px;"> und eine vorübergehende Nettoreaktion in die umgekehrte Richtung, um das Gleichgewicht wiederherzustellen. Alternativ zu dieser kinetischen Interpretation kann die Auswirkung von Konzentrationsänderungen auf Gleichgewichte anhand von Reaktionsquotienten rationalisiert werden. Wenn das System im Gleichgewicht ist, <img alt="Eq5" src="/files/ftp_upload/11391/11391_Equation 5.png" style="text-align: center; height: 70px;"> Wenn ein Reaktant hinzugefügt wird (wodurch der Nenner des Reaktionsquotienten erhöht wird) oder ein Produkt entfernt wird (wodurch der Zähler verringert wird), dann ist Qc < Kc und das Gleichgewicht verschiebt sich nach rechts. Beachten Sie, dass die drei verschiedenen Arten, diesen Stress hervorzurufen, zu drei unterschiedlichen Änderungen in der Zusammensetzung der Gleichgewichtsmischung führen. Wenn N2 hinzugefügt wird, verbraucht die Rechtsverschiebung O2 und produziert NO, wenn das Gleichgewicht wiederhergestellt ist, was zu einer Mischung mit einer höheren Konzentration an N2 und NO und einer geringeren Konzentration an O2 als zuvor führt. Wenn O2 hinzugefügt wird, weist die neue Gleichgewichtsmischung höhere Konzentrationen an O2 und NO und eine geringere Konzentration an N2 auf. Wenn schließlich NO entfernt wird, weist das neue Gleichgewichtsgemisch höhere Konzentrationen an N2 und O2 und eine geringere Konzentration an NO auf. Trotz dieser Unterschiede in der Zusammensetzung bleibt der Wert der Gleichgewichtskonstante nach der Belastung derselbe wie zuvor (gemäß dem Massenwirkungsgesetz). Die gleiche Logik kann auf Belastungen angewendet werden, bei denen Reaktanten entfernt oder Produkte hinzugefügt werden. In diesem Fall ist Qc > Kc und das Gleichgewicht verschiebt sich nach links. Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/13-3-shifting-equilibria-le-chateliers-principle">Openstax, Chemistry 2e, Section 13.3 Shifting Equilibria: LeChatelier’s Principle</a>.

Das Prinzip von Le Chatelier: Konzentration ändern

Ein Gleichgewichtssystem befindet sich in einem Zustand des dynamischen Gleichgewichts, in dem Vorwärts- und Rückwärtsreaktionen mit gleicher Geschwindigkeit ablaufen. Ist ein Gleichgewichtssystem ...

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Chemical Equilibrium

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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 reactant or product can move the equilibrium in one direction or the other.

Adding a reactant, such as N2 or O2 in the example reaction, increases the forward reaction rate. The forward rate then becomes greater than the reverse rate, so the equilibrium shifts right. Removing the product NO has the same effect because it lowers the reverse reaction rate and creates the same imbalance.

The opposite changes cause a left shift. Removing reactant or adding product increases the reverse reaction rate compared with the forward rate. The system then moves in the reverse direction until equilibrium is reached again.

This shift can also be explained with the reaction quotient, Qc, and the equilibrium constant, Kc. When reactant is added, Qc becomes less than Kc. When product is removed, Qc also becomes less than Kc, so the equilibrium shifts right. If reactant is removed or product is added, then Qc is greater than Kc and the equilibrium shifts left.

Although the final composition changes, the equilibrium constant stays the same after the stress is removed and the system rebalances. If N2 is added, the new mixture has more N2 and NO and less O2. If O2 is added, the mixture has more O2 and NO and less N2. If NO is removed, the mixture ends with more N2 and O2 and less NO. The same idea applies to shifts caused by removing reactant or adding product.

Shifting Equilibrium by Changing Concentration

shifting-equilibrium-by-changing-concentration

the equilibrium constant

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...

le chatelier's principle: 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

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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...

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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...

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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...

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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...

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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)

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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

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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...

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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

Learn how changing concentration shifts chemical equilibrium, including why adding or removing reactants or products moves the reaction left or right.

Shifting Equilibrium by Changing Concentration | JoVE K12

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Shifting Equilibrium by Changing Concentration

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