Name: arrhenius equation in reaction speed
Uploaded: 2023-04-30T18:28:32.000Z
Duration: 2 min 28 s
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Chemistry

Matter And Its Interactions

HS-PS1-5

effect-of-temperature-change-on-reaction-rate

Effect of Temperature Change on Reaction Rate

Das Geschwindigkeitsgesetz einer Reaktion definiert die Beziehung zwischen einer Reaktantenkonzentration und der Reaktionsgeschwindigkeit in Form einer Geschwindigkeitskonstante "k".
Die Geschwindigkeitskonstante beschreibt die Beziehung zwischen Temperatur und kinetischen Parametern in Bezug auf die Kollision, Orientierung und Aktivierungsenergie reagierender Moleküle über die Arrhenius-Gleichung. "A" ist eine Konstante, die als Arrhenius-Faktor oder Frequenzfaktor bezeichnet wird. "e" ist ein exponentieller Faktor, der die in Joule pro Mol gemessene Aktivierungsenergie, die Gaskonstante und die Temperatur in Kelvin integriert.
Die Temperaturabhängigkeit der Parameter kann mit dem Kollisionsmodell erklärt werden, das besagt, dass reagierende Moleküle mit ausreichender Energie in der richtigen Ausrichtung kollidieren sollten, um eine chemische Reaktion auszulösen.
Der Frequenzfaktor besteht aus zwei Komponenten: der Kollisionsfrequenz und dem Orientierungsfaktor. Die Kollisionshäufigkeit ist die Anzahl der molekularen Kollisionen pro Zeiteinheit, während der Orientierungsfaktor die Wahrscheinlichkeit von Kollisionen mit günstiger Orientierung beschreibt.
Dennoch führt nur ein kleiner Bruchteil der Kollisionen zu einer Reaktion. Dies liegt daran, dass die reagierenden Moleküle eine Energiebarriere, die sogenannte Aktivierungsenergie, überwinden müssen, um sich in Produkte umzuwandeln.
Nur die Moleküle, die mit ausreichender kinetischer Energie kollidieren, haben genügend potentielle Energie, um Bindungen zu biegen, zu dehnen oder zu brechen, um sich in ein hochenergetisches Zwischenprodukt umzuwandeln, das als Übergangszustand oder aktivierter Komplex bezeichnet wird. Der kurzlebige, instabile aktivierte Komplex verliert Energie und bildet stabile Produkte, deren Gesamtenergie geringer ist als die der Reaktanten.
Der Exponentialfaktor in der Arrhenius-Gleichung stellt den Anteil der erfolgreichen Kollisionen dar, die zu Produkten führen. Ein Temperaturanstieg beeinflusst sowohl den Frequenzfaktor als auch den Exponentialfaktor.
Bei erhöhten Temperaturen bewegen sich Moleküle schneller, kraftvoller und mit höheren thermischen Energien, was zu günstigeren Kollisionen führt.
Bei den meisten Reaktionen führt ein Temperaturanstieg zu einer höheren Frequenz und exponentiellen Faktoren, was zu einem Anstieg der Geschwindigkeitskonstante führt, was sich folglich in einer beschleunigten Reaktionsgeschwindigkeit niederschlägt.

einfluss der temperaturänderung auf die reaktionsgeschwindigkeit

Die Arrhenius Gleichung,

setzt die Aktivierungsenergie und die Geschwindigkeitskonstante k für viele chemische Reaktionen in Beziehung.

<img alt="Figure1" src="/files/ftp_upload/11698/11698_Equation1.svg" style="text-align: center; height: 30px;">

In dieser Gleichung ist R die ideale Gaskonstante, die einen Wert von 8,314 J/mol·K hat, T ist die Temperatur in Kelvin, E_a ist die Aktivierungsenergie in Joule pro Mol, e ist die Konstante 2,7183 und A ist eine als Frequenzfaktor bezeichnete Konstante, die mit der Häufigkeit der Zusammenstöße und der Ausrichtung der reagierenden Moleküle zusammenhängt.

Der Frequenzfaktor A spiegelt wider, wie gut die Reaktionsbedingungen korrekt ausgerichtete Kollisionen zwischen den Reaktantenmolekülen begünstigen. Eine erhöhte Wahrscheinlichkeit effektiv ausrichtungsabhängig Kollisionen führt zu größeren Werten für A und schnelleren Reaktionsgeschwindigkeiten.

Der Exponentialterm e−Eₐ/RT beschreibt die Auswirkung der Aktivierungsenergie auf die Reaktionsgeschwindigkeit. Gemäß der kinetischen Molekulartheorie ist die Temperatur der Materie ein Maß für die durchschnittliche kinetische Energie ihrer Atome oder Moleküle – eine niedrigere Aktivierungsenergie führt zu einem größeren Anteil ausreichend energiereicher Moleküle und einer schnelleren Reaktion.

Der Exponentialterm beschreibt auch den Einfluss der Temperatur auf die Reaktionsgeschwindigkeit. Eine höhere Temperatur stellt einen entsprechend größeren Anteil an Molekülen dar, die über ausreichend Energie (RT) verfügen, um die Aktivierungsbarriere (E_a) zu überwinden. Dies führt zu einem höheren Wert für die Geschwindigkeitskonstante und einer entsprechend schnelleren Reaktionsgeschwindigkeit.

Die minimale Energie, die erforderlich ist, um bei einer Kollision zwischen Reaktanten ein Produkt zu bilden, wird Aktivierungsenergie (E_a) genannt. Der Unterschied zwischen der erforderlichen Aktivierungsenergie und der kinetischen Energie, die durch kollidierende Reaktantenmoleküle bereitgestellt wird, ist ein Hauptfaktor, der die Geschwindigkeit einer chemischen Reaktion beeinflusst. Wenn die Aktivierungsenergie viel größer ist als die durchschnittliche kinetische Energie von Molekülen, erfolgt die Reaktion langsam, da nur wenige sich schnell bewegende Moleküle über genügend Energie zur Reaktion verfügen. Wenn die Aktivierungsenergie viel kleiner ist als die durchschnittliche kinetische Energie der Moleküle, ist ein großer Teil der Moleküle ausreichend energiereich und die Reaktion läuft schnell ab.

Reaktionsdiagramme werden in der chemischen Kinetik häufig verwendet, um verschiedene Eigenschaften einer interessierenden Reaktion zu veranschaulichen. Es zeigt, wie sich die Energie eines chemischen Systems ändert, wenn es eine Reaktion durchläuft und Reaktanten in Produkte umwandelt.

Dieser Text wurde angepasst von<a href="https://openstax.org/books/chemistry-2e/pages/12-5-collision-theory">Openstax, Chemistry 2e, Abschnitt 12.5: Collision Theory.</a>

Einfluss der Temperaturänderung auf die Reaktionsgeschwindigkeit

Die Arrhenius-Gleichung,

setzt die Aktivierungsenergie und die Geschwindigkeitskonstante k für viele chemische Reaktionen in Beziehung.
In dieser Gleichung ist R das ideale Gas ...

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arrhenius equation in reaction speed

The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster.

In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor.

The frequency factor, A, describes how often reacting molecules collide and how well they are oriented during those collisions. Better orientation increases the chance of effective collisions. That leads to larger A values and faster reaction rates.

The exponential term, e−Ea/RT, shows how activation energy affects the reaction rate. Kinetic molecular theory says that temperature measures the average kinetic energy of atoms or molecules. When activation energy is lower, more molecules have enough energy to react, and the reaction is faster.

The same exponential term also shows the effect of temperature. At higher temperature, a larger fraction of molecules has enough energy, RT, to get over the activation barrier, Ea. This increases the rate constant and speeds up the reaction.

Activation energy is the minimum energy needed to form products during a collision between reactants. If Ea is much larger than the average kinetic energy of the molecules, only a few fast-moving molecules can react, so the reaction is slow. If Ea is much smaller than the average kinetic energy, many molecules can react, so the reaction proceeds quickly.

Reaction diagrams are often used in chemical kinetics to show how a system’s energy changes as reactants turn into products. They help visualize the energy barrier and the path from reactants to products. This text is adapted from Openstax, Chemistry 2e, Section 12.5: Collision Theory.

Arrhenius Equation in Reaction Speed

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effect of temperature change on reaction rate

The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster. In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor. The frequency factor, A, describes how often reacting molecules collide and how well...

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key terms and concepts

Explore how the Arrhenius equation links temperature, activation energy, and collision orientation to reaction speed in high school chemistry.

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Arrhenius Equation in Reaction Speed

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