Name: catalyst action in reaction rates
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 2 min 50 s
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.5.1

Catalysis

El estudio de la cinética y los mecanismos de reacción ayuda a los investigadores a optimizar la velocidad de una reacción. Un aumento en la temperatura o concentración acelerará la velocidad, pero también puede conducir a la descomposición o productos secundarios cuando se aumenta demasiado. Alternativamente, se puede agregar un producto químico a la mezcla de reacción que acelera la velocidad de reacción sin ser alterado o consumido permanentemente.Estas sustancias se denominan catalizadores y afectan la constante de velocidad cambiando la energía de activación. Recuerde que cuanto mayor sea la energía de activación, más lenta será la velocidad de reacción. Por lo tanto, muchas reacciones químicas, como la descomposición del peróxido de hidrógeno acuoso, progresan lentamente.La adición de un catalizador reduce la energía de activación al proporcionar un mecanismo de reacción alternativo sin afectar los estados de energía de los reactivos y productos. Hay dos tipos de catalizadores:homogéneos y heterogéneos. Existe un catalizador homogéneo en la misma fase que los reactivos.Por ejemplo, se agrega bromuro de sodio al peróxido de hidrógeno acuoso para acelerar su descomposición en oxígeno gaseoso y agua. Primero, los iones de bromuro reaccionan con el peróxido de hidrógeno en un medio ácido para formar una solución naranja de bromo acuoso y agua. A continuación, el bromo acuoso y el peróxido de hidrógeno reaccionan y liberan iones de bromuro indicados por una solución incolora.Como es característico de un catalizador, los iones de bromuro aceleran la reacción, pero permanecen sin ser consumidos y no aparecen en la ecuación neta balanceada. Existe un catalizador heterogéneo en un estado físico diferente en comparación con los reactivos. La catálisis heterogénea se caracteriza por cuatro pasos subyacentes:adsorción, difusión, reacción y desorción.Por ejemplo, la reacción de hidrogenación de eteno gaseoso insaturado a etano se acelera mediante paladio finamente disperso sobre carbón. Aquí, el catalizador existe en su estado sólido, mientras que los reactivos están en sus formas gaseosas. Durante esta catálisis heterogénea, las moléculas de eteno e hidrógeno se adsorben en la superficie del catalizador.El enlace hidrógeno-hidrógeno se rompe permitiendo que los átomos de hidrógeno se difundan en la superficie del catalizador. Cuando los átomos de hidrógeno en difusión encuentran moléculas de eteno adsorbidas, reaccionan para formar etano saturado. Posteriormente, los productos se desorban y se alejan de la superficie metálica, dejando atrás el catalizador intacto.

catálisis

La presencia de un catalizador afecta la velocidad de una reacción química. Un catalizador es una sustancia que puede aumentar la velocidad de la reacción sin consumirse durante el proceso. Una comprensión básica del papel de los catalizadores durante las reacciones químicas puede entenderse a partir del concepto de los mecanismos de reacción y los diagramas de energía.
 <img alt="Image1" src="/files/ftp_upload/11383/11383_Image_1.png" style="text-align: center; height: 350px;" />
 La imagen ilustrada representa los diagramas de reacción de un proceso químico endotérmico que progresa en ausencia (curva roja) y en presencia (curva azul) de un catalizador.
 Ambas curvas representan la misma reacción general – comienzan y terminan en las mismas energías. (En este caso, los productos tienen más energía que los reactivos. Por lo tanto, la reacción es endotérmica). Sin embargo, sus mecanismos de reacción son diferentes. La reacción no catalizada procede a través de un mecanismo de un solo paso (con sólo un estado de transición observado). En cambio, la reacción catalizada sigue un mecanismo de dos pasos (se observan dos estados de transición) con una energía de activación notablemente inferior. Esta diferencia en las rutas de la reacción ilustra el papel del catalizador en proporcionar un mecanismo de reacción alternativo con menor energía de activación, acelerando así las reacciones.
 El mecanismo de reacción catalizado no necesita involucrar un mayor número de pasos elementales que el mecanismo no catalizado. Sin embargo, debe proporcionar una ruta de reacción alternativa cuyo paso determinante de la velocidad sea más rápido (con una Ea o energía de activación más baja).
 Una reacción catalítica puede clasificarse como homogénea o heterogénea, basándose en los estados físicos en que existen los catalizadores y los reactivos durante el proceso catalítico.
 Catálisis homogénea
 En la catálisis homogénea, el catalizador está presente en la misma fase que los reactivos: Sólido, líquido o gas. Durante el proceso, el catalizador interactúa con el reactivo para formar una sustancia intermedia, que luego se descompone o reacciona con otro reactivo en uno o más pasos para regenerar el catalizador original y formar el producto final.
 Un ejemplo de catálisis homogénea es el proceso químico que implica la descomposición del ozono que se produce en la atmósfera superior de la Tierra. El ozono es una molécula relativamente inestable que se descompone para producir oxígeno diatómico. Esta reacción de descomposición es coherente con el siguiente mecanismo de dos pasos:
 <img alt="Eq1" src="/files/ftp_upload/11383/11383_Equation_1.png" style="text-align: center; height: 75px;" />
 Muchas sustancias pueden catalizar la descomposición del ozono. Por ejemplo, se cree que la descomposición del ozono catalizada por óxido nítrico se produce a través del siguiente mecanismo de tres pasos:
 <img alt="Eq2" src="/files/ftp_upload/11383/11383_Equation_2.png" style="text-align: center; height: 115px;" />
 Sin embargo, la reacción general es la misma tanto para el mecanismo de dos pasos no catalizado como para el mecanismo de tres pasos catalizado por NO:
 <img alt="Eq3" src="/files/ftp_upload/11383/11383_Equation_3.png" style="text-align: center; height: 50px;" />
 En la reacción catalizada, observe que NO es un reactivo en el primer paso del mecanismo y un producto en el último paso. Este es otro rasgo característico de un catalizador: Aunque participa en la reacción química, no es consumido por la reacción. Además, en esta catálisis homogénea, tanto el reactivo como el catalizador se encuentran en fase gaseosa.
 Catálisis heterogénea
 En la catálisis heterogénea, el catalizador está presente en una fase diferente (generalmente un sólido) a la de los reactivos. Tales catalizadores funcionan generalmente proporcionando una superficie activa sobre la cual puede ocurrir una reacción. Las reacciones en fase gaseosa y líquida catalizadas por catalizadores heterogéneos ocurren en la superficie del catalizador en lugar de dentro de la fase gaseosa o líquida.
 La catálisis heterogénea suele implicar los siguientes procesos:
 <ol>
 <li>Adsorción del reactivo o reactivos en la superficie del catalizador</li>
 <li>Activación de los reactivos adsorbidos</li>
 <li>La reacción de los reactivos adsorbidos</li>
 <li>Desorción del producto o productos en la superficie del catalizador</li>
 </ol>
 <img alt="Image2" src="/files/ftp_upload/11383/11383_Image_2.png" style="text-align: center; height: 250px;" />
 La imagen ilustrada representa el mecanismo de reacción que involucra la catálisis heterogénea del eteno y del gas hidrógeno en una superficie sólida de níquel, formando gas etano (C2H4 + H2 ⟶ C2H6):
 (A) El hidrógeno se adsorbe en la superficie del níquel. Durante el proceso, los enlaces hidrógeno-hidrógeno se rompen para formar enlaces níquel-hidrógeno. 
 (b) El eteno también se adsorbe en la superficie del níquel rompiendo el enlace pi carbono-carbono y formando enlaces níquel-carbono. 
 (c) Los átomos de hidrógeno difunden a través de la superficie y forman nuevos enlaces carbono-hidrógeno cuando colisionan para formar etano (C2H6). 
 (D) Moléculas de metano se desorben de la superficie del níquel.
 La catálisis heterogénea se utiliza para la fabricación industrial de productos químicos como el amoníaco, el ácido nítrico, el ácido sulfúrico y el metanol. Los catalizadores heterogéneos también se utilizan en los convertidores catalíticos que se encuentran en la mayoría de los automóviles alimentados con gasolina.
 Este texto está adaptado de<a href="https://openstax.org/books/chemistry-2e/pages/12-7-catalysis"> Openstax, Chemistry 2e, Sección 12,7: Catálisis</a>.

Catálisis

La presencia de un catalizador afecta la velocidad de una reacción química. Un catalizador es una sustancia que puede aumentar la velocidad de reacción sin ser consumido ...

Education

Educación

JoVE Core

Química

Chemical Kinetics

Cinética Química

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

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 activation energy, or Ea. The lower rate-determining barrier is what makes the reaction faster.

Catalytic reactions are often grouped as homogeneous or heterogeneous. In homogeneous catalysis, the catalyst and reactants are in the same phase, which may be solid, liquid, or gas. The catalyst reacts with the reactant to form an intermediate, and that intermediate then breaks down or reacts again to form the product and regenerate the catalyst.

A good example of homogeneous catalysis is ozone decomposition in the upper atmosphere. Ozone breaks down to form diatomic oxygen, and nitric oxide can catalyze that process through a three-step mechanism. In this reaction, NO appears as a reactant in the first step and a product in the last step, which shows that it participates in the reaction but is not used up. Here, both the reactant and the catalyst are gases.

In heterogeneous catalysis, the catalyst is in a different phase from the reactants, usually a solid. These reactions happen on the catalyst surface. They typically include adsorption of reactants, activation on the surface, reaction of the adsorbed molecules, and desorption of the products.

The nickel-catalyzed reaction of ethene and hydrogen to form ethane shows this surface process. Hydrogen first adsorbs on nickel, and the H-H bond breaks to form nickel-hydrogen bonds. Ethene also adsorbs as its carbon-carbon pi bond breaks and nickel-carbon bonds form. Hydrogen atoms then move across the surface and make new carbon-hydrogen bonds, and the ethane product desorbs from the nickel surface.

Heterogeneous catalysts are important in industry. They help make ammonia, nitric acid, sulfuric acid, and methanol. They are also used in catalytic converters in most gasoline-powered cars.

Catalyst Action in Reaction Rates

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...

measuring reaction rates

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

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...

temperature dependence on reaction rate

Collision Theory and Reaction Speed

Collision theory explains why reaction speed depends on how particles collide. Atoms, molecules, or ions must come close together before they can react. The theory says the reaction rate depends on the collision rate, the orientation of the colliding species, and whether the collision has enough energy for bonds to change. A gas-phase reaction between carbon monoxide and oxygen shows why orientation matters. The molecules can collide in more than one way. If the oxygen side of carbon monoxide...

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...

reaction mechanisms

Elementary Steps in Reaction Mechanisms

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

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

Explore how catalysts speed up reactions by lowering activation energy, with clear examples of homogeneous and heterogeneous catalysis for high school chemistry.

Catalyst Action in Reaction Rates | JoVE K12

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Pennsylvania State Academic Standards

Physical Science

Chemical Reactions

3.2.9-12.D

3.2.9-12.E

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

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New York State Science Learning Standards

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Catalysts in Chemical Reactions

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The Pauli Exclusion Principle

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The Energies of Atomic Orbitals

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The Aufbau Principle and Hund's Rule

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PS.Chm.1.3

Periodic Classification of the Elements

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The Periodic Table

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Atomic Mass

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Molar Mass

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Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

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Atomic Radii and Effective Nuclear Charge

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Ionic Radii

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Ionization Energy

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Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



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Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

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Lewis Symbols and the Octet Rule

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Resonance

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Formal Charges

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Exceptions to the Octet Rule

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	...

Bond Energies and Bond Lengths

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Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

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Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Catalyst Action in Reaction Rates

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