What are the steps involved in the Langmuir-Hinshelwood mechanism?

The Langmuir-Hinshelwood mechanism involves three main steps: (1) adsorption of reactants onto the catalyst surface, (2) reaction between adsorbed species, and (3) desorption of products from the catalyst surface.

How does the Langmuir-Hinshelwood mechanism differ from the Eley-Rideal mechanism?

The Langmuir-Hinshelwood mechanism involves the reaction of two adsorbed reactants on a catalyst's surface, while the Eley-Rideal mechanism involves a reaction between one adsorbed reactant and one reactant directly from the gas phase.

What assumptions are made in the Langmuir-Hinshelwood mechanism?

The Langmuir-Hinshelwood mechanism assumes that adsorption of reactants occurs on a uniform catalyst surface, surface adsorption is in equilibrium, the surface reaction is the rate-determining step, and adsorbed species do not interact. Additionally, it assumes that only a monolayer of adsorbates covers the surface and that the desorption step is rapid.

What types of reactions typically follow the Langmuir-Hinshelwood mechanism?

Heterogeneous catalytic reactions, particularly surface reactions such as hydrogenations, oxidations, and ammonia synthesis, typically follow the Langmuir-Hinshelwood mechanism. This involves the adsorption of reactants on a catalyst surface, the surface reaction between adsorbed species, and subsequent desorption of the products.

What factors influence the rate of reaction in the Langmuir-Hinshelwood mechanism?

The rate of reaction in the Langmuir-Hinshelwood mechanism is influenced by the surface coverage of reactants, adsorption and desorption constants, temperature, and the catalytic surface's activity. These factors affect how reactants adsorb onto, react on, and desorb from the catalytic surface.

What is the primary focus of the Langmuir-Hinshelwood mechanism?

Examining phase changes in pure substances during heating.

What does the Langmuir-Hinshelwood mechanism describe?

Interactions of ions in a homogeneous solution.

What is the Langmuir-Hinshelwood mechanism primarily used for?

Reactions with gaseous reactants on solid catalysts.

What are the stages involved in the Langmuir-Hinshelwood mechanism?

Adsorption, surface reaction, desorption.

In the Langmuir-Hinshelwood mechanism, what does the rate equation involve?

\text{Rate} = \frac{k}{\Delta H} + \theta_T.

Langmuir-Hinshelwood mechanism: Rate Law, Surface Reaction

Langmuir-Hinshelwood mechanism

The Langmuir-Hinshelwood mechanism describes a catalytic reaction process where two reactant molecules adsorb onto a catalyst's surface before undergoing a reaction to form a product. This reaction pathway emphasizes that both reactants must be present on the catalyst surface simultaneously, differentiating it from other mechanisms such as the Eley-Rideal mechanism. Understanding this mechanism is crucial for optimizing industrial catalytic processes, such as in the production of ammonia and hydrocarbon cracking.

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Langmuir-Hinshelwood Mechanism Definition

The Langmuir-Hinshelwood mechanism is a significant concept in the study of heterogeneous catalysis. It explains how two reactants adsorb on a catalyst surface and react to form products.

This mechanism is often used to describe reactions occurring on solid surfaces, especially when both reactants are gases. Understanding this mechanism helps predict reaction rates and can optimize industrial processes that depend on surface reactions.

The Langmuir-Hinshelwood mechanism refers to a kinetic model in which two different molecules adsorb onto a catalyst surface, react to form a product, and then desorb from the surface.

Key Components of the Langmuir-Hinshelwood Mechanism

The Langmuir-Hinshelwood mechanism involves several stages, which can be broadly categorized as follows:

Adsorption: Both reactant molecules (let's call them A and B) adsorb onto the catalyst surface. This may involve simple physisorption or chemisorption, depending on the nature of the reactant and surface.
Surface Reaction: Once both reactants are adsorbed, they migrate on the surface and can react with each other to form the product molecule (denoted as P). The reaction is typically governed by surface diffusion and concentration of the reactants.
Desorption: The product molecule desorbs from the surface to release it back to the reaction environment.

The overall rate-determining step can vary depending on the conditions, such as temperature and pressure, and properties of the catalyst and reactants.

A classic example is the reaction between hydrogen (H₂) and oxygen (O₂) on a platinum surface to form water (H₂O). In this case, both H₂ and O₂ adsorb onto the platinum, react to form H₂O, and the water vapor then desorbs from the surface:

Step 1: \text{H}_2 \text{(g)} + 2* \rightarrow 2 \text{H*}
Step 2: \text{O}_2 \text{(g)} + 2* \rightarrow 2 \text{O*}
Step 3: \text{2H*} + \text{O*} \rightarrow \text{H}_2\text{O(g)} + 3*

You might encounter variations of this mechanism in literature, such as the Eley-Rideal mechanism, which assumes that one reactant is adsorbed while the other is in the gas phase.

Analyzing the kinetics of the Langmuir-Hinshelwood mechanism leads us to a set of rate equations:

The rate of surface reaction can often be represented as: \text{Rate} = k \frac{\theta_A \theta_B}{1 + K_A P_A + K_B P_B}, where \(k\) is the rate constant, \(\theta_A\) and \(\theta_B\) are the surface coverages of reactants A and B, and \(K_A\) and \(K_B\) are the adsorption equilibrium constants for the reactants.
This equation simplifies when one of the reactants is present in excess, allowing for simplified analysis and understanding of specific systems.
Surface coverage is critical and can be expressed as \(\theta_i = \frac{K_i P_i}{1 + \text{sum of all adsorption terms}} \).

Exploring these equations provides insights into how changes in pressure or temperature can shift equilibrium and affect reaction rates, offering ways to optimize the process for industrial applications.

Langmuir-Hinshelwood Mechanism Fundamentals

The Langmuir-Hinshelwood mechanism is pivotal in understanding heterogeneous catalysis, particularly when gas-phase reactants interact on the surface of a solid catalyst. As you venture into the world of chemical reactions on surfaces, this mechanism provides critical insights.

Understanding Surface Adsorption

At the heart of the Langmuir-Hinshelwood mechanism lies the process of adsorption. This is where the reactants adhere to the catalyst's surface, which can be quite complex depending on whether the adsorption is through weak Van der Waals forces (physisorption) or stronger chemical bonding (chemisorption). The adsorbed molecules then experience movements on the surface, which facilitates the reactions required to form products. The effectiveness of these surface reactions is key for industrial applications.

Surface Reactions And Desorption

After adsorption, the adsorbed molecules undergo surface reactions. These are influenced by factors like surface coverage and temperature. The reaction typically proceeds via the following steps:

Molecules A and B adsorb onto specific sites on the catalyst.
These molecules then migrate and react to form an intermediate or directly the product, depending on the reaction pathway.
Finally, the product desorbs from the catalyst, making room for new reactant molecules.

This cycle perpetuates the catalytic process, with desorption crucial since it regenerates the catalyst's active sites for further reactions.

An instructive example is the synthesis of ammonia (NH₃) from nitrogen (N₂) and hydrogen (H₂) on an iron catalyst, a typical Langmuir-Hinshelwood scenario:

Step 1:	N₂ (g) + 2* → 2N*
Step 2:	3H₂ (g) + 3* → 6H*
Step 3:	2N* + 6H* → 2NH₃ (g) + 8*

The reactants adsorb, react, and then the ammonia molecules desorb, freeing the surface.

The balance between adsorption and desorption rates often dictates the overall reaction rate in these catalytic processes.

For a deeper analysis, consider the reaction rate (\text{r}) under this mechanism, expressed mathematically as:

\(r = k \frac{\theta_A \theta_B}{1 + K_A P_A + K_B P_B}\)

Where:

\(k\) is the rate constant.
\(\theta_A\) and \(\theta_B\) are the fractional surface coverages of reactants A and B.
\(K_A\) and \(K_B\) are their respective adsorption equilibrium constants.

This equation elucidates how the presence of either reactant and their partial pressures influence the overall rate, emphasizing the significance of surface dynamics in catalysis.

Langmuir-Hinshelwood Mechanism in Heterogeneous Catalysis

In the realm of heterogeneous catalysis, the Langmuir-Hinshelwood mechanism plays a crucial role. It provides insights into how chemical reactions occur on the surface of catalysts, particularly when the reactants are in the gas phase and interact on solid catalysts.

This understanding is essential for optimizing industrial processes and improving catalyst efficiency, making it a fundamental topic in chemical engineering and catalytic studies.

The Langmuir-Hinshelwood mechanism is a kinetic model describing how two adsorbed molecules on a catalyst surface interact to form a product that desorbs, making the surface available for more reactions.

Mechanism Steps In Detail

The Langmuir-Hinshelwood mechanism consists of several distinct steps:

Adsorption: Reactants A and B adhere to the catalyst surface. This could involve physisorption, where physical forces play a role, or chemisorption, where chemical bonds are formed.
Surface Reaction: Once adsorbed, the reactants migrate on the surface, meeting other reactants to facilitate a chemical reaction.
Desorption: The newly formed product, P, detaches from the surface, freeing up space for new reactant molecules to adsorb.

The equilibrium and rates of these steps are crucial for determining the overall reaction rate on a catalyst surface.

An example is the catalytic oxidation of carbon monoxide (CO) with oxygen (O₂) on a platinum surface:

Step 1:	CO (g) + * → CO*
Step 2:	O₂ (g) + 2* → 2O*
Step 3:	CO* + O* → CO₂ (g) + 2*

The CO and O₂ adsorb onto the platinum, react to form carbon dioxide (CO₂), and then desorb from the surface.

The Langmuir-Hinshelwood mechanism is typically considered when both reactants are present in comparable concentrations on the catalyst surface.

Examining the kinetics within this mechanism involves detailed expressions for adsorption-desorption equilibrium and reaction rates:

The Langmuir-Hinshelwood rate equation is described as:

\(r = k \frac{\theta_A \theta_B}{1 + K_A P_A + K_B P_B + K_P P_P}\)

Where:

\(r\) is the rate of reaction.
\(k\) is the intrinsic rate constant for the surface reaction.
\(\theta_A\) and \(\theta_B\) represent the surface coverages of A and B.
\(K_A\), \(K_B\), and \(K_P\) are equilibrium constants for adsorption of A, B, and the product P, respectively.
\(P_A\), \(P_B\), and \(P_P\) indicate the partial pressures of A, B, and P.

This equation highlights the dependencies on adsorbate coverage, providing insights into how conditions like pressure and surface characteristics impact reaction rates.

Langmuir-Hinshelwood Mechanism Derivation

In chemical kinetics, understanding the derivation of the Langmuir-Hinshelwood mechanism involves a sequence of carefully defined steps that explain how reactants interact on a catalyst surface. This model is particularly useful for reactions involving gaseous reactants and solid catalysts, offering insights into reaction dynamics.

Langmuir-Hinshelwood Mechanism Rate Law

The rate law for the Langmuir-Hinshelwood mechanism captures the core principles of adsorption, surface reaction, and desorption. This is expressed through a distinct mathematical formula:

The rate of reaction \( r \) can be described by:

\(r = k \frac{K_A P_A K_B P_B}{(1 + K_A P_A + K_B P_B)^2}\)

Where:

\( k \) is the intrinsic rate constant for the surface reaction.
\( K_A \) and \( K_B \) are adsorption equilibrium constants for reactants A and B, respectively.
\( P_A \) and \( P_B \) are partial pressures of A and B.

This formula reflects the complexities of reactions on surfaces, where multiple variables interact to influence the rate.

An example of using this rate law is in studying the decomposition of ammonia (NH₃) on a platinum surface:

Step 1:	NH₃ (g) + * → NH₃*
Step 2:	NH₃* → N* + 3H*
Step 3:	N* + H* → NH₃*

This scenario shows how surface coverage and reaction kinetics are integral to understanding the catalytic process.

Delving deeper into the kinetics, the Langmuir-Hinshelwood mechanism can be understood through multiple assumptions:

Both A and B must be chemisorbed on the surface before reacting.
The surface reaction is often the rate-determining step, as opposed to diffusion or adsorption.

For further verification of the theoretical model against experimental data, detailed analysis of variables such as temperature and pressure is crucial. Moreover, the interaction parameter \( K \) provides insights into changes in adsorption behavior under varying conditions.

Langmuir-Hinshelwood mechanism - Key takeaways

Langmuir-Hinshelwood Mechanism Definition: A kinetic model in heterogeneous catalysis where two reactants adsorb onto a catalyst surface, react to form a product, and desorb.
Heterogeneous Catalysis: Langmuir-Hinshelwood mechanism is crucial for understanding reactions on solid catalysts with gas-phase reactants.
Key Stages: The mechanism involves adsorption of reactants, surface reaction, and desorption of products.
Rate Law: Given by `Rate = k (θ_A θ_B) / (1 + K_A P_A + K_B P_B)`, where θ and K are surface coverage and equilibrium constants.
Surface Reaction: Governed by surface diffusion and concentration, and can be the rate-determining step.
Applications: Optimizes industrial processes like ammonia synthesis and CO oxidation, providing insights into catalyst efficiency.

Langmuir-Hinshelwood mechanism

StudySmarter Editorial Team

Langmuir-Hinshelwood Mechanism Definition

Key Components of the Langmuir-Hinshelwood Mechanism