Name: measuring reaction rates
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 2 min 53 s
Channel: JoVE

K12 Standards

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Chemistry and Physics

IPC.7

IPC.7.F

Reaction Rate

Eine chemische Reaktion beinhaltet die chemische Umwandlung von Reaktanten in Produkte. Mit fortschreitender Reaktion nimmt die Konzentration der Reaktanten ab, während die Konzentration der Produkte zunimmt. Diese Varianz in den Konzentrationen von Reaktanten und Produkten kann in einem Diagramm als Funktion der Zeit dargestellt werden.
Die Geschwindigkeit, mit der eine Reaktion abläuft, wird als Reaktionsgeschwindigkeit bezeichnet. Er misst die Geschwindigkeit des Verschwindens von Reaktanten oder die Geschwindigkeit des Auftretens von Produkten und wird in Einheiten der Molarität pro Sekunde ausgedrückt. 
Die durchschnittliche Reaktionsgeschwindigkeit kann aus der Änderung der Konzentrationen von Reaktanten oder Produkten während eines bestimmten Zeitraums berechnet werden. Der molare Konzentrationswert wird in Klammern angegeben, t steht für den Zeitraum und das Delta-Symbol steht für die "Änderung in".
Da Reaktanten während einer chemischen Reaktion erschöpft werden, ist der Wert der Konzentrationsänderung der Reaktanten immer negativ. Daher wird eine in Form von Reaktanten berechnete Reaktionsgeschwindigkeit durch ein negatives Vorzeichen ergänzt, um den Gesamtwert positiv zu machen.
Die Reaktionsgeschwindigkeit ist während einer Reaktion nicht gleichmäßig. Die Geschwindigkeit zu Beginn der Reaktion, zum "Zeitpunkt Null", wird als Anfangsreaktionsgeschwindigkeit bezeichnet. Wenn die Konzentrationen der Reaktanten abnehmen, nimmt die Reaktionsgeschwindigkeit ab oder die Reaktion verlangsamt sich.
Die Reaktionsgeschwindigkeit zu einem bestimmten Zeitpunkt oder die momentane Reaktionsgeschwindigkeit wird gemessen, indem die Steigung einer Tangente berechnet wird, die zur Reaktionskurve gezogen wird, entweder für Reaktanten oder Produkte zum interessierenden Zeitpunkt.
Der Steigungswert oder die momentane Rate zu einem bestimmten Zeitpunkt ist für alle Reaktanten und Produkte gleich.
Die Reaktionsgeschwindigkeit einer chemischen Reaktion spiegelt auch die tatsächlichen stöchiometrischen Koeffizienten von Reaktanten und Produkten wider.
Für jede ausgeglichene Reaktion, bei der ein Mol von A mit b Mol von B reagiert und c Mol von C und d Mol von D erzeugt, kann die Reaktionsgeschwindigkeit mit der generischen Formel ausgedrückt und berechnet werden: −1/a × Δ[A]/Δt = −1/b × Δ[B]/Δt. Diese Werte sind identisch mit +1/c × Δ[C]/Δt, was mit +1/d × Δ[D]/Δt identisch ist.
Die Bestimmung der Reaktionsgeschwindigkeit ist von grundlegender Bedeutung für die Untersuchung der chemischen Kinetik, die hilft zu verstehen, wie schnell ein Medikament, ein Katalysator oder eine synthetische Reaktion funktioniert, damit sie besser kontrolliert und in ihrer Funktion optimiert werden kann.

reaktionsrate

Die Reaktionsgeschwindigkeit ist die Änderung der Menge eines Reaktanten oder Produkts pro Zeiteinheit. Reaktionsgeschwindigkeiten werden daher durch Messung der Zeitabhängigkeit einer Eigenschaft bestimmt, die mit den Reaktanten- oder Produktmengen in Zusammenhang stehen kann. Geschwindigkeiten von Reaktionen, die beispielsweise gasförmige Substanzen verbrauchen oder erzeugen, lassen sich bequem durch Messung von Volumen- oder Druckänderungen bestimmen.

 Die mathematische Darstellung der zeitlichen Änderung der Konzentration von Reaktanten und Produkten ist der Geschwindigkeitsausdruck für die Reaktion. Die Klammern geben molare Konzentrationen an und das Symbol Delta (Δ) gibt „Änderung in“ an.

 Beispielsweise ändert sich die Konzentration von Wasserstoffperoxid, H2O2, in einer wässrigen Lösung im Laufe der Zeit langsam, da es sich gemäß der Gleichung zersetzt:

 <img alt="Eq1" src="/files/ftp_upload/11373/11373_Equation_1.png" style="height: 50px;">

 Die Geschwindigkeit, mit der sich Wasserstoffperoxid zersetzt, kann als Änderungsrate seiner Konzentration ausgedrückt werden:

 <img alt="Eq2" src="/files/ftp_upload/11373/11373_Equation_2.png" style="height: 70px;">

 Somit stellt [H2O2]t1 die molare Konzentration von Wasserstoffperoxid zum Zeitpunkt t1 dar; ebenso stellt [H2O2]t2 die molare Konzentration von Wasserstoffperoxid zu einem späteren Zeitpunkt t2 dar; und Δ[H2O2] stellt die Änderung der molaren Konzentration von Wasserstoffperoxid während des Zeitintervalls Δt (d. h. t2 − t1) dar. Da die Reaktantenkonzentration mit fortschreitender Reaktion abnimmt, ist Δ[H2O2] eine negative Größe. Konventionell sind Reaktionsgeschwindigkeiten positive Größen, daher wird diese negative Konzentrationsänderung mit −1 multipliziert. 

 Durchschnittliche Reaktionsgeschwindigkeit und momentane Reaktionsgeschwindigkeit 

 Die Reaktionsgeschwindigkeiten variieren mit der Zeit und nehmen mit fortschreitender Reaktion ab. Eine durchschnittliche Reaktionsgeschwindigkeit über einen Zeitraum kann anhand der Konzentrationen zu Beginn und am Ende dieses Zeitraums berechnet werden, in dem sich die Reaktionsgeschwindigkeit ändert. Die Geschwindigkeit, mit der eine Reaktion zu einem bestimmten Zeitpunkt abläuft, wird als Momentangeschwindigkeit bezeichnet. Die momentane Geschwindigkeit einer Reaktion zum „Zeitpunkt Null“, wenn die Reaktion beginnt, ist ihre Anfangsgeschwindigkeit. 

 Die momentane Geschwindigkeit einer Reaktion kann auf zwei Arten bestimmt werden. Wenn die experimentellen Bedingungen die Messung von Konzentrationsänderungen über kurze Zeitintervalle ermöglichen, liefert die Berechnung der Durchschnittsraten einigermaßen gute Näherungen für die Momentanraten. Alternativ kann auch ein grafisches Verfahren verwendet werden. Beispielsweise kann im Beispiel der Zersetzung von Wasserstoffperoxid durch Auftragen der Konzentration von Wasserstoffperoxid gegen die Zeit die momentane Zersetzungsrate von H2O2 zu jedem Zeitpunkt „t“ aus der Steigung einer zu diesem Zeitpunkt an die Kurve gezogenen Tangente berechnet werden.

 <img alt="Image1" src="/files/ftp_upload/11373/11373_Image_1.png" style="height: 300px;">

 Dieses Diagramm zeigt eine Auftragung der Konzentration gegen die Zeit für eine 1.000 M Lösung von H2O2. Die Geschwindigkeit ist zu jedem Zeitpunkt gleich dem Negativ der Steigung einer Tangente an die Kurve zu diesem Zeitpunkt. Tangenten werden bei t = 0 h („Anfangsrate“) und bei t = 12 h („augenblickliche Rate“ bei 12 h) angezeigt.

 Relative Reaktionsgeschwindigkeiten

 Die Geschwindigkeit einer Reaktion kann als Konzentrationsänderung eines Reaktanten oder Produkts ausgedrückt werden. Für jede gegebene Reaktion sind diese Geschwindigkeitsausdrücke alle entsprechend der Reaktionsstöchiometrie miteinander verknüpft. Die Geschwindigkeit der allgemeinen Reaktion aA ⟶ bB kann als Abnahme der Konzentration von A oder als Zunahme der Konzentration von B ausgedrückt werden. Diese beiden Geschwindigkeitsausdrücke hängen durch die Stöchiometrie der Reaktion zusammen, wobei:

 <img alt="Eq3" src="/files/ftp_upload/11373/11373_Equation_3.png" style="height: 70px;">

 Beachten Sie, dass ein negatives Vorzeichen als Faktor einbezogen wurde, um die entgegengesetzten Vorzeichen der beiden Mengenänderungen zu berücksichtigen (die Reaktantenmenge nimmt ab, während die Produktmenge zunimmt).

 Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/12-introduction">Openstax, Chemistry 2e, Chapter 12 Introduction</a> and <a href="https://openstax.org/books/chemistry-2e/pages/12-1-chemical-reaction-rates#12163">Openstax, Chemistry 2e, Section 12.1: Chemical Reaction Rates.</a>

Reaktionsrate

Die Reaktionsgeschwindigkeit ist die Änderung der Menge eines Reaktanten oder Produkts pro Zeiteinheit. Die Reaktionsgeschwindigkeiten werden daher durch Messung der Zeit ...

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measuring reaction rates

Measuring reaction rates shows how fast reactants are used up or products are formed over time. The rate of reaction is the change in the amount of a reactant or product per unit time. Because of that, scientists measure how a property changes as the reaction proceeds and connect that change to reactant or product amounts.

For reactions that make or use a gas, the rate can be followed by changes in volume or pressure. A rate expression is the mathematical way to write how concentration changes over time. In this expression, brackets mean molar concentration, and the delta symbol means change in amount.

Hydrogen peroxide provides a clear example. As H2O2 decomposes in water, its concentration slowly decreases with time. The reaction rate can be written as the rate of change of the H2O2 concentration. If the concentration at time t1 is compared with the concentration at a later time t2, the change in concentration over the time interval Δt is found.

Because the reactant concentration goes down, Δ[H2O2] is negative. Reaction rates are reported as positive values, so the negative sign is reversed by multiplying by -1. This keeps the reaction rate positive even when the reactant amount is falling.

Reaction rates are not constant. They usually change as the reaction continues, so an average reaction rate is calculated over a time interval using the starting and ending concentrations. The rate at one exact moment is the instantaneous rate, and the instantaneous rate at time zero is the initial rate.

Instantaneous rate can be estimated in two ways. If concentration changes can be measured over very short time intervals, the average rate gives a good approximation. A graph can also be used. When concentration is plotted against time, the instantaneous rate at a given time equals the negative slope of a tangent line to the curve. In the hydrogen peroxide example, tangents can be drawn at t = 0 h for the initial rate and at t = 12 h for the instantaneous rate at 12 h.

The rate of a reaction can be written using either a reactant or a product. For a general reaction aA → bB, the decrease in A and the increase in B are linked by the reaction stoichiometry. The two rate expressions are related by that stoichiometry, and a negative sign is included to account for the reactant decreasing while the product increases.

Measuring Reaction Rates

reaction rate

Measuring reaction rates shows how fast reactants are used up or products are formed over time. The rate of reaction is the change in the amount of a reactant or product per unit time. Because of that, scientists measure how a property changes as the reaction proceeds and connect that change to reactant or product amounts. For reactions that make or use a gas, the rate can be followed by changes in volume or pressure. A rate expression is the mathematical way to write how concentration changes...

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Learn how reaction rates are measured using concentration, volume, pressure, average rate, and instantaneous rate with the hydrogen peroxide example.

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IPC.7.D

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Measuring Reaction Rates

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