Name: reaction order from concentration
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 3 min 3 s
Channel: JoVE

K12 Standards

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Chemistry and Physics

IPC.7

IPC.7.F

Concentration and Rate Law

Die Geschwindigkeit einer Reaktion hängt oft von den Reaktantenkonzentrationen ab. Für jede Reaktion kann die Beziehung zwischen der Reaktionsgeschwindigkeit und den Reaktantenkonzentrationen mathematisch mit Hilfe eines Geschwindigkeitsgesetzes oder der Geschwindigkeitsgleichung ausgedrückt werden. 
In einem Geschwindigkeitsgesetz ist k die Proportionalitätskonstante oder die Geschwindigkeitskonstante, und n ist die Reaktionsordnung in Bezug auf einen einzelnen Reaktanten, dessen Wert oft eine ganze Zahl ist. In den Geschwindigkeitsgesetzen für Multireaktantenreaktionen ist die Gesamtreaktionsordnung die Summe aller Reaktantenordnungen.
Für jeden Reaktanten werden die Reaktionsgeschwindigkeit, die Geschwindigkeitskonstante, die Konzentration und die Reaktionsreihenfolge experimentell bestimmt. Das Geschwindigkeitsgesetz drückt die Beziehung zwischen all diesen Parametern aus. 
Einzelne Reaktantenordnungen nehmen in der Regel die Werte 0, 1 oder 2 an, und basierend auf der Gesamtreaktionsordnung können chemische Reaktionen als Reaktionen nullr., erster oder zweiter Ordnung kategorisiert werden.
Eine chemische Reaktion mit einem einzelnen Reaktanten oder einer unimolikularen Reaktion, bei der die Reaktionsgeschwindigkeit während ihrer gesamten Dauer konstant bleibt, ist eine Reaktion nullter Ordnung. Die Reaktantenordnung in einer Reaktion nullter Ordnung ist Null, und gemäß dem Geschwindigkeitsgesetz wird die Reaktantenkonzentration auf die nullte Potenz erhöht.
Da der Wert einer beliebigen Zahl, die zur nullten Potenz angehoben wird, eins ist, ist die Reaktionsgeschwindigkeit einer Reaktion nullter Ordnung gleich der Geschwindigkeitskonstante und daher unabhängig von der Reaktantenkonzentration. Daher verlangsamt sich die Reaktionsgeschwindigkeit in einer Reaktion nullter Ordnung auch bei abnehmender Konzentration des Reaktanten nicht.
Eine unimolekulare chemische Reaktion, bei der die Reaktionsgeschwindigkeit direkt proportional zur Konzentration des Reaktanten ist, ist eine Reaktion erster Ordnung. Die Reaktantenordnung für eine Reaktion erster Ordnung ist eins, und gemäß dem Geschwindigkeitsgesetz wird die Konzentration des Reaktanten auf die erste Potenz erhöht.
Da der Wert einer beliebigen Zahl, die hoch eins wird, gleich bleibt, hängt die Reaktionsgeschwindigkeit einer Reaktion erster Ordnung direkt von der Reaktantenkonzentration ab. Mit abnehmender Reaktantenkonzentration nimmt die Reaktionsgeschwindigkeit linear proportional ab.
Eine unimolekulare chemische Reaktion, bei der die Reaktionsgeschwindigkeit vom Quadrat der Konzentration des Reaktanten abhängt, ist eine Reaktion zweiter Ordnung. Die Reaktantenordnung ist zwei, und die Reaktantenkonzentration wird auf die zweite Potenz erhöht.
Dementsprechend hängt die Reaktionsgeschwindigkeit in einer Reaktion zweiter Ordnung direkt vom Quadrat der Reaktantenkonzentration ab. Wenn die Reaktantenkonzentration abnimmt, nimmt die Reaktionsgeschwindigkeit exponentiell quadratisch ab.

konzentrations- und geschwindigkeitsgesetz

Die Geschwindigkeit einer Reaktion wird durch die Konzentrationen der Reaktanten beeinflusst. Geschwindigkeitsgesetze (differentielle Geschwindigkeitsgesetze) oder Geschwindigkeitsgleichungen sind mathematische Ausdrücke, die den Zusammenhang zwischen der Geschwindigkeit einer chemischen Reaktion und der Konzentration ihrer Reaktanten beschreiben. Beispielsweise kann in einer generischen Reaktion aA + bB ⟶ Produkte, bei der a und b stöchiometrische Koeffizienten sind, das Geschwindigkeitsgesetz wie folgt geschrieben werden:  <img alt="Eq1" src="/files/ftp_upload/11375/11375_Equation_1.png" style="height: 50px;"> [A] und [B] stellen die molaren Konzentrationen der Reaktanten dar, und k ist die Geschwindigkeitskonstante, die für eine bestimmte Reaktion bei einer bestimmten Temperatur spezifisch ist. Die Exponenten m und n sind die Reaktionsordnungen und sind typischerweise positive ganze Zahlen, obwohl sie Brüche, negativ oder Null sein können. Die Geschwindigkeitskonstante k und die Reaktionsordnungen m und n werden experimentell bestimmt, indem beobachtet wird, wie sich die Geschwindigkeit einer Reaktion ändert, wenn sich die Konzentrationen der Reaktanten ändern. Die Geschwindigkeitskonstante k ist unabhängig von den Reaktantenkonzentrationen, variiert jedoch mit der Temperatur. Die Reaktionsordnungen in einem Geschwindigkeitsgesetz beschreiben die mathematische Abhängigkeit der Geschwindigkeit von den Reaktantenkonzentrationen. Unter Bezugnahme auf das generische Geschwindigkeitsgesetz (Rate = k[A]m[B]n) ist die Reaktion m-ter Ordnung in Bezug auf A und n-ter Ordnung in Bezug auf B. Wenn beispielsweise m = 1 und n = 2, ist die Die Reaktion ist in A erster Ordnung und in B zweiter Ordnung. Die Gesamtreaktionsordnung ist einfach die Summe der Ordnungen für jeden Reaktanten. Für das hier beispielhafte Geschwindigkeitsgesetz ist die Reaktion insgesamt dritter Ordnung (1 + 2 = 3). Ein üblicher experimenteller Ansatz zur Bestimmung von Geschwindigkeitsgesetzen ist die Methode der Anfangsgeschwindigkeiten. Bei dieser Methode werden Reaktionsgeschwindigkeiten für mehrere experimentelle Versuche gemessen, die mit unterschiedlichen anfänglichen Reaktantenkonzentrationen durchgeführt werden. Der Vergleich der gemessenen Geschwindigkeiten dieser Versuche ermöglicht die Bestimmung der Reaktionsordnungen und anschließend der Geschwindigkeitskonstanten, die zusammen zur Formulierung eines Geschwindigkeitsgesetzes verwendet werden. Geschwindigkeitsgesetze können für einige Reaktanten gebrochene Ordnungen aufweisen, und manchmal werden negative Reaktionsordnungen beobachtet, wenn eine Erhöhung der Konzentration eines Reaktanten zu einer Abnahme der Reaktionsgeschwindigkeit führt. Es ist wichtig zu beachten, dass Geschwindigkeitsgesetze nur durch Experimente bestimmt werden und nicht zuverlässig durch die Reaktionsstöchiometrie vorhergesagt werden können. Die Reaktionsreihenfolge bestimmt den Zusammenhang zwischen der Reaktionsgeschwindigkeit und der Konzentration der Reaktanten oder Produkte. • Bei einer Reaktion nullter Ordnung hat die Konzentration der Reaktanten keinen Einfluss auf die Reaktionsgeschwindigkeit, die durchgehend konstant bleibt. • Bei einer Reaktion erster Ordnung ist die Reaktionsgeschwindigkeit direkt und linear proportional zur Änderung der Reaktantenkonzentration. Mit abnehmender Reaktantenkonzentration nimmt auch die Reaktionsgeschwindigkeit proportional ab. • Bei Reaktionen zweiter oder höherer Ordnung ist die Reaktionsgeschwindigkeit proportional zum Exponentialwert der Reaktanten. Daher nimmt die Reaktionsgeschwindigkeit mit fortschreitender Reaktion und abnehmender Konzentration der Reaktanten exponentiell ab. Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/12-3-rate-laws#57033">Openstax, Chemistry 2e, Section 12.3: Rate Laws</a>

Konzentrations- und Geschwindigkeitsgesetz

Die Geschwindigkeit einer Reaktion wird durch die Konzentrationen der Reaktanten beeinflusst. Geschwindigkeitsgesetze (Differentialgeschwindigkeitsgesetze) oder Geschwindigkeitsgleichungen sind mathematische Ausdrücke ...

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reaction order from concentration

Reaction order from concentration shows how reactant amounts affect reaction rate. Rate laws, also called differential rate laws or rate equations, are mathematical expressions that connect reaction rate with the concentrations of reactants. For a generic reaction a A + b B → products, the rate law can be written using the reactant concentrations [A] and [B] and a rate constant k.

In a rate law, k is the rate constant for one specific reaction at one specific temperature. The exponents m and n are the reaction orders. They are usually positive integers, but they can also be fractions, negative numbers, or zero. The values of k, m, and n are found experimentally by measuring how the rate changes when reactant concentrations change.

The rate constant does not depend on the reactant concentrations, but it can change with temperature. The reaction orders show the mathematical link between concentration and rate. In the expression rate = k [A]m [B]n, the reaction is m order with respect to A and n order with respect to B. For example, if m = 1 and n = 2, the reaction is first order in A and second order in B.

The overall reaction order is the sum of the orders for each reactant. In the example above, the reaction is third order overall because 1 + 2 = 3. A common way to find a rate law is the method of initial rates. In this method, reaction rates are measured in several trials that start with different initial reactant concentrations. Comparing those rates makes it possible to find the reaction orders and then the rate constant.

Rate laws can also include fractional orders. In some cases, a reactant may have a negative order. That means increasing its concentration can lower the reaction rate. Rate laws are determined by experiment only, and they cannot be reliably predicted from reaction stoichiometry. The reaction order also describes how the rate changes as reactant or product concentration changes.

A zero-order reaction has a rate that does not change with reactant concentration. The rate stays constant throughout the reaction. In a first-order reaction, the rate is directly proportional to the change in reactant concentration. As the reactant concentration drops, the rate drops by the same proportion. In second-order or higher-order reactions, the rate depends on the reactants raised to an exponent. As the reaction continues and reactant concentration decreases, the rate falls exponentially.

Reaction Order from Concentration

reaction rate

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...

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Tracking Reaction Kinetics with Light and Pressure

Reaction kinetics can be tracked with polarimetry, spectrometry, and pressure measurements. These methods let scientists follow a reaction without disturbing the sample. They also help determine how reactant or product concentrations change over time. Polarimetry is used for optically active substances. These substances rotate the plane of polarized light, which is called optical rotation. The effect comes from molecular structure. Normal monochromatic light is unpolarized, but after it passes...

concentration and rate law

Reaction order from concentration shows how reactant amounts affect reaction rate. Rate laws, also called differential rate laws or rate equations, are mathematical expressions that connect reaction rate with the concentrations of reactants. For a generic reaction a A + b B → products, the rate law can be written using the reactant concentrations [A] and [B] and a rate constant k. In a rate law, k is the rate constant for one specific reaction at one specific temperature. The exponents m and n...

determining order of reaction

Finding Rate Law from Initial Rates

Rate laws connect the speed of a chemical reaction to the concentration of its reactants. The rate constant, k, and the reaction orders are not taken from the chemical equation. They are found experimentally by watching how the rate changes when the reactant concentrations change. One common way to do this is the method of initial rates. In this method, several trials are run with different starting concentrations. The measured rates are then compared to determine the reaction orders and,...

the integrated rate law: the dependence of concentration on time

the-integrated-rate-law-the-dependence-of-concentration-on-time

Reading Reaction Progress with Integrated Laws

Integrated rate laws connect reaction concentration to time. They help show how much reactant or product is present after a certain period. They can also help estimate how long a reaction must run to reach a given extent. A common use is finding how long radioactive material must be stored before its radioactivity drops to a safe level. These equations come from the differential rate law after it is integrated with respect to time. For a first-order reaction, where rate = k[A], the integrated...

half-life of a reaction

Reaction Half-Life in Kinetics

Reaction half-life is the time needed for half of a reactant to be consumed. After each half-life, half of the remaining reactant is used up. A hydrogen peroxide decomposition example shows this pattern clearly. The concentration drops from 1.000 M to 0.500 M in the first 6.00 hours, then to 0.250 M in the next 6.00 hours, and then to 0.125 M in the third period. Each later 6.00-hour interval removes half of what is left. For first-order reactions, the half-life does not depend on the reactant...

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arrhenius plots

Determining Activation Energy from Temperature

The Arrhenius equation links activation energy and the rate constant, k, for chemical reactions. It is written as k = Ae−Ea/RT. In this equation, R is the ideal gas constant with a value of 8.314 J/mol·K, T is the temperature on the kelvin scale, Ea is the activation energy in J/mole, e is the constant 2.7183, and A is the frequency factor. The frequency factor depends on collision frequency and the orientation of reacting molecules. Experimental kinetic data can be used to find the activation...

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Chemical reactions can happen in steps, and a balanced equation does not show the full path at the molecular level. A reaction mechanism, also called a reaction path, gives the step-by-step process that explains how reactants become products. The decomposition of ozone is one example of a reaction that can be described by a sequence of steps. Each step in a mechanism is an elementary reaction. These elementary reactions happen in order, and when they are added together, they give the balanced...

rate-determining steps

Reaction Bottlenecks in Chemical Kinetics

Reaction bottlenecks help explain rate-determining steps in multistep reaction mechanisms. In a mechanism with several elementary steps, one step is often much slower than the others. That slowest step is called the rate-limiting step, or rate-determining step. A reaction cannot move faster than its slowest step, so this step controls the overall reaction rate. The idea is like traffic on a four-lane freeway with one lane closed. Cars can only move as fast as the bottleneck allows. In the same...

catalysis

Catalyst Action in Reaction Rates

Catalysts change the rate of a chemical reaction by giving it a faster path. A catalyst increases reaction rate without being consumed during the process. Its effect is often explained with reaction mechanisms and energy diagrams. For an endothermic reaction, the reactants and products start and end at the same energies in both cases. The uncatalyzed path is a one-step mechanism with one transition state. The catalyzed path follows a different mechanism with two transition states and a lower...

enzymes

Enzyme Action and Inhibition

Enzymes are biological catalysts that speed up many reactions in living organisms. They help control cellular metabolism by lowering the activation energy needed for biochemical reactions. When activation energy drops, reaction rates can increase. Enzyme problems can also lead to serious disease. A genetic abnormality that causes G6PD, or glucose-6-phosphate dehydrogenase, deficiency can disrupt the pathway that supplies NADPH to cells. In red blood cells, this can reduce glutathione and...

key terms and concepts

Learn how concentration affects reaction rate, how rate laws are written, and how initial rates reveal reaction order, the rate constant, and overall order.

Reaction Order from Concentration | JoVE K12

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IPC.7.D

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IPC.7.E

Science concepts. The student knows that relationships exist between the structure and properties of matter. The student is expected to:

Reaction Order from Concentration

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