Adsorption
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Physical adsorption involves weak van der Waals forces between adsorbate and adsorbent molecules, resulting in a reversible and multimolecular adsorption layer. Chemical adsorption forms stronger chemical bonds in an irreversible and unimolecular layer. Physical adsorption heat is small around 5 kcal/mol while chemical adsorption heat is much larger from 20-100 kcal/mol. Physical adsorption increases with lower temperature and higher pressure while chemical adsorption is less dependent on these factors.
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Adsorption
Surface chemistry deals with phenomena that occur at interfaces between phases. Adsorption is a key phenomenon where molecules accumulate at surfaces rather than in the bulk. Some materials like charcoal and silica gel act as good adsorbents due to their large surface areas. Adsorption involves molecules of gases, liquids, or dissolved substances concentrating on the surface of an adsorbent rather than in its bulk.
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This document discusses different types of adsorption including physical, chemical, and exchange adsorption. It provides details on physical adsorption such as the forces involved and its exothermic and reversible nature. Chemical adsorption forms strong bonds and is usually irreversible. Exchange adsorption involves charged sites on the adsorbent surface. Common adsorbents like activated carbon, silica gel, and zeolites are also described. Adsorption isotherms models including Langmuir and Freundlich are summarized which relate the amount of adsorbate removed to its concentration at equilibrium.
Adsorption isotherm
- Adsorption occurs when a gas or liquid accumulates on the surface of a solid, forming a film. It differs from absorption which involves diffusion into the bulk.
- The Langmuir adsorption model describes monolayer adsorption on uniform sites but makes assumptions that do not always apply. The BET model extends it to account for multilayer adsorption.
- The Temkin isotherm accounts for indirect interactions between adsorbed molecules which affect heat of adsorption and coverage at high pressures.
Adsorption
Adsorption is the process where matter accumulates at the interface between two phases, such as a gas transferring to the surface of a liquid. This occurs due to higher surface energy at interfaces compared to interior molecules. Adsorption equilibria can be modeled using isotherms such as Langmuir, Freundlich, and BET, which relate the amount adsorbed to concentration in solution. Factors like adsorbate properties, pH, temperature, and presence of other solutes influence adsorption extent and isotherm shape.
Freundlich adsorption isotherm
The Freundlich adsorption isotherm model describes the relationship between the amount of gas adsorbed on an adsorbent and the gas pressure at equilibrium. It states that the extent of adsorption (amount of gas adsorbed per unit mass of adsorbent) increases with increasing pressure but is not directly proportional to pressure. The Freundlich equation is x/m = KP1/n, where x is the amount of adsorbate, m is the mass of adsorbent, P is the pressure, K is a constant, and 1/n is between 0 and 1. A plot of log(x/m) versus log(P) yields a straight line with slope
Adsorption
Adsorption is the process where a gas or liquid accumulates on the surface of a solid or liquid, forming a film. It occurs due to surface energy - atoms on the surface experience a bond deficiency. There are two types: physisorption, where adsorbate adheres via weak van der Waals forces; and chemisorption, where chemical bonds form. Factors influencing adsorption include surface area, gas nature, temperature, and pressure. Adsorption has applications in vacuum production, gas masks, catalysis, and water purification.
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This document summarizes key concepts about adsorption. It discusses adsorption at liquid-gas, liquid-liquid, and solid-gas interfaces. It differentiates between physical adsorption and chemisorption, and describes common adsorption isotherms like Langmuir, Freundlich, Temkin, and BET isotherms. It also discusses measuring gas adsorption through volumetric and gravimetric methods. Finally, it covers adsorption from solutions and compares apparent adsorption isotherms to composite isotherms for solute adsorption from binary liquid mixtures.
Surface chemistry ppt CLASS 12 CBSE CHAPTER 5
- Adsorption is the accumulation of molecular species at the surface of a solid or liquid rather than in the bulk. The substance that accumulates is called the adsorbate and the surface it accumulates on is the adsorbent.
- Examples of adsorption include gases accumulating on charcoal surfaces, dye molecules accumulating on charcoal when added to solutions, and aqueous sugar solutions becoming colorless when passed over beds of charcoal.
- There are two main types of adsorption - physical adsorption (physisorption) due to weak van der Waals forces, and chemical adsorption (chemisorption) due to chemical bonding between adsorbate and adsorbent.
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Adsorption
Surface chemistry deals with phenomena that occur at interfaces between phases. Adsorption is a key phenomenon where molecules accumulate at surfaces rather than in the bulk. Some materials like charcoal and silica gel act as good adsorbents due to their large surface areas. Adsorption involves molecules of gases, liquids, or dissolved substances concentrating on the surface of an adsorbent rather than in its bulk.
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This document discusses different types of adsorption including physical, chemical, and exchange adsorption. It provides details on physical adsorption such as the forces involved and its exothermic and reversible nature. Chemical adsorption forms strong bonds and is usually irreversible. Exchange adsorption involves charged sites on the adsorbent surface. Common adsorbents like activated carbon, silica gel, and zeolites are also described. Adsorption isotherms models including Langmuir and Freundlich are summarized which relate the amount of adsorbate removed to its concentration at equilibrium.
Adsorption isotherm
- Adsorption occurs when a gas or liquid accumulates on the surface of a solid, forming a film. It differs from absorption which involves diffusion into the bulk.
- The Langmuir adsorption model describes monolayer adsorption on uniform sites but makes assumptions that do not always apply. The BET model extends it to account for multilayer adsorption.
- The Temkin isotherm accounts for indirect interactions between adsorbed molecules which affect heat of adsorption and coverage at high pressures.
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Adsorption is the process where matter accumulates at the interface between two phases, such as a gas transferring to the surface of a liquid. This occurs due to higher surface energy at interfaces compared to interior molecules. Adsorption equilibria can be modeled using isotherms such as Langmuir, Freundlich, and BET, which relate the amount adsorbed to concentration in solution. Factors like adsorbate properties, pH, temperature, and presence of other solutes influence adsorption extent and isotherm shape.
Freundlich adsorption isotherm
The Freundlich adsorption isotherm model describes the relationship between the amount of gas adsorbed on an adsorbent and the gas pressure at equilibrium. It states that the extent of adsorption (amount of gas adsorbed per unit mass of adsorbent) increases with increasing pressure but is not directly proportional to pressure. The Freundlich equation is x/m = KP1/n, where x is the amount of adsorbate, m is the mass of adsorbent, P is the pressure, K is a constant, and 1/n is between 0 and 1. A plot of log(x/m) versus log(P) yields a straight line with slope
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Adsorption is the process where a gas or liquid accumulates on the surface of a solid or liquid, forming a film. It occurs due to surface energy - atoms on the surface experience a bond deficiency. There are two types: physisorption, where adsorbate adheres via weak van der Waals forces; and chemisorption, where chemical bonds form. Factors influencing adsorption include surface area, gas nature, temperature, and pressure. Adsorption has applications in vacuum production, gas masks, catalysis, and water purification.
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This document summarizes key concepts about adsorption. It discusses adsorption at liquid-gas, liquid-liquid, and solid-gas interfaces. It differentiates between physical adsorption and chemisorption, and describes common adsorption isotherms like Langmuir, Freundlich, Temkin, and BET isotherms. It also discusses measuring gas adsorption through volumetric and gravimetric methods. Finally, it covers adsorption from solutions and compares apparent adsorption isotherms to composite isotherms for solute adsorption from binary liquid mixtures.
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- Adsorption is the accumulation of molecular species at the surface of a solid or liquid rather than in the bulk. The substance that accumulates is called the adsorbate and the surface it accumulates on is the adsorbent.
- Examples of adsorption include gases accumulating on charcoal surfaces, dye molecules accumulating on charcoal when added to solutions, and aqueous sugar solutions becoming colorless when passed over beds of charcoal.
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1. Adsorption is the accumulation of atoms, molecules, or ions on the surface of an adsorbent material. It is a surface phenomenon where adsorbate adheres to the surface of an adsorbent.
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1. Surface chemistry deals with phenomena that occur at interfaces between different phases such as solid-gas or solid-liquid.
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This document provides an overview of solid state and surface chemistry, specifically focusing on adsorption. It defines key terms like adsorption, desorption, chemisorption and physisorption. There are two main types of adsorption - physical and chemical. Physical adsorption involves weak van der Waals bonding, while chemical adsorption has stronger chemical bonding. Adsorption can be modeled using isotherms, with the Langmuir isotherm describing monolayer adsorption and the BET isotherm describing multilayer adsorption. Surface coverage is plotted against gas pressure at constant temperature to obtain adsorption isotherms, which can provide information about adsorption equilibrium and surface properties.
681_Fin surfacechemistrEREREREERy ppt.pptx
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Adsorption
Adsorption refers to the binding of molecules or particles to a surface. It is a surface phenomenon where the concentration of a substance is higher at the interface between two phases compared to the bulk phases. Common adsorbents used industrially include activated carbon, silica gel, and alumina due to their large surface areas. Adsorption plays an important role in processes like gas masks, ammonia production, and removing colors from solutions by using adsorbents like charcoal and bone black.
Adsorption
Adsorption refers to the binding of molecules or particles to a surface. It occurs when there is a higher concentration of substances at an interface compared to the bulk phase. Common adsorbents used industrially include activated carbon, silica gel, and alumina due to their large surface areas. Adsorption can be physical or chemical in nature. Physical adsorption involves weak van der Waals forces while chemical adsorption forms chemical bonds. Adsorption finds applications in gas masks, ammonia production, and removing colors from solutions.
Surface Chem.pptx
Surface chemistry involves absorption and adsorption. Absorption occurs when particles accumulate uniformly throughout a bulk solid, while adsorption occurs when particles accumulate only on the surface. Adsorption involves the formation of new interactions as molecules bind to a surface. It is a spontaneous process characterized by negative enthalpy and entropy. The factors that affect adsorption include surface area, temperature, pressure, and the nature of the gas. Adsorption can be physical (physisorption) or chemical (chemisorption) in nature. Applications of adsorption include producing high vacuums, controlling humidity, removing color from solutions, and enabling heterogeneous catalysis.
Adsorption
This document discusses adsorption equilibrium and factors that influence adsorption. It defines adsorption as the accumulation of molecules on a surface, compared to absorption which is dissolution within a phase. The main factors that influence adsorption are surface area, nature of the gas, heats of adsorption, reversibility, temperature, pressure, and thickness of the adsorbed layer. Common adsorption models like Langmuir and Freundlich isotherms are also summarized.
Adsorption pharmaceutical analysis
This document discusses adsorption equilibrium and factors that influence adsorption. It defines adsorption as the accumulation of molecules on a surface, compared to absorption which is dissolution within a phase. The main factors that influence adsorption are surface area, nature of the gas, heats of adsorption, reversibility, temperature, pressure, and thickness of the adsorbed layer. Common adsorption models like Langmuir and Freundlich isotherms are also summarized.
Physisorption chemisorption and work function change induced by adsorbates
This document discusses different types of adsorption - physisorption and chemisorption - and how they differ. Physisorption involves weak van der Waals forces between adsorbate and adsorbent molecules, while chemisorption involves chemical bond formation. It also discusses isotherm models like the Langmuir and Freundlich isotherms that describe the relationship between amount of gas adsorbed and pressure or concentration. Finally, it mentions that adsorption can change the work function of materials by altering charge distribution and dipole formation at the surface.
Chemistry chapter 1
This document provides an introduction to chemistry, including:
1. Definitions of key terms like matter, elements, compounds, properties and changes in matter.
2. The major branches of chemistry like organic, inorganic, physical and analytical chemistry.
3. An overview of the periodic table, including periodic trends and classifications of elements as metals, nonmetals, metalloids and noble gases.
chapter 5
This document discusses surface chemistry and adsorption. It begins by defining surface chemistry as phenomena that occur at interfaces between different phases, such as solid-gas interfaces. It then defines adsorption as the accumulation of molecules at surfaces rather than in the bulk of a solid or liquid. Adsorption occurs due to unbalanced attractive forces at surfaces. There are two main types of adsorption: physical adsorption due to weak van der Waals forces, and chemical adsorption where chemical bonds form between adsorbate and adsorbent molecules. The mechanism and factors affecting adsorption are also explained.
Surface chemistry
The document discusses surface chemistry and catalysis. It defines key terms like adsorption, absorption, interface and provides differences between adsorption and absorption. It describes different types of adsorption like physical and chemical adsorption. Factors affecting adsorption like nature of adsorbent and adsorbate, surface area, temperature, pressure are explained. Different models of adsorption isotherms including Freundlich and Langmuir isotherms are introduced.
Adsorption is the adhesion of atoms, ions or molecules from a gas, liquid or ...
Adsorption is the adhesion of atoms, ions or molecules from a gas, liquid or dissolved solid to a surface. This process creates a film of the adsorbate on the surface of the adsorbent. This process differs from absorption, in which a fluid (the absorbate) is dissolved by or permeates a liquid or solid (the absorbent). While adsorption does often precede absorption, which involves the transfer of the absorbate into the volume of the absorbent material, alternatively, adsorption is distinctly a surface phenomenon, wherein the adsorbate does not penetrate through the material surface and into the bulk of the adsorbent. The term sorption encompasses both adsorption and absorption, and desorption is the reverse of sorption.
Chemistry Chapter 1
This document provides an introduction to chemistry, including:
1. Definitions of key terms like elements, compounds, physical and chemical properties and changes.
2. An overview of the major branches of chemistry like organic, inorganic, physical and analytical chemistry.
3. Descriptions of the periodic table, including groups like alkali metals and halogens, and periodic trends.
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1st Lecture on Adsorption and Colloids | Chemistry Part II | 11th Std
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Adsorption
- 1. Introduction of adsorption. Properties of physical & chemical adsorption.
- 2. Adsorption The phenomenon of concentration of molecules of a gas or liquid at a solid surface is called adsorption. The substance that deposits at the surface is called adsorbate and the solid on whose surface the deposition occurs is called the adsorbent.
- 3. Types of adsorption The adsorption of a gas into a solid surface is mainly two types: 1. Physical adsorption: This is due to the gas molecules being held to the solid surface by van der waal’s attraction forces. It is also referred to as van der waal’s adsorption. For example, Adsorption of hydrogen or oxygen on charcoal is physical adsorption
- 4. Types of adsorption 2. Chemical adsorption: In this kind of adsorption, the gas molecules or atoms are held to the solid surface by chemical bonds. These bonds may be covalent or ionic in nature. For example, hydrogen is chemisorbed in nickel. Hydrogen molecules is first adsorbed by van der waal’s forces and then dissociates. The hydrogen atoms are thus chemisorbed in nickel.
- 6. Mechanism of Adsorption Atoms or molecules of a solid surface behave like the surface molecules of a liquid. These are not surrounded by atoms or molecules of their kind. Therefore, they have unbalanced or residual attractive forces on the surface which can hold adsorbate particles.
- 7. Mechanism of Adsorption The adsorbed atoms or molecules can be held on the surface of a metal such as platinum (Pt) by physical van der Waal’s force or chemical forces due to residual valence bonds. Thus the adsorption of hydrogen on platinum may take place in two ways (molecularly or atomically as shown above).
- 8. Properties of physical & chemical adsorption 1. Adsorption and Surface area: Physical adsorption caused by intermolecular van der Waal’s forces. Chemical adsorption caused by chemical bond formation. 2. Nature of Gas: Physical adsorption depends on nature of gas. Easily liquefiable gases are adsorbed readily. Chemical adsorption much more specific than physical adsorption. 3. Heats of Adsorption: Physical adsorption heat of adsorption is small (about 5 kcal mol–1). Chemical adsorption heat of adsorption is large (20–100 kcal mol–1).
- 9. Properties of physical & chemical adsorption 4. Reversible character: Physical adsorption is reversible. Chemical adsorption is irreversible. 5. Effect of temperature: Physical adsorption occurs rapidly at low temperature; decreases with increasing temperature. Chemical adsorption increases with increase of temperature.
- 10. Properties of physical & chemical adsorption 6. Effect of pressure: Physical adsorption increase of pressure increases adsorption; decrease of pressure causes desorption. Chemical adsorption change of pressure has no such effects. 7. Thickness of Adsorbed layer of gas: Physical adsorption is multimolecular layers on adsorbent surface. Chemical adsorption is unimolecular layer.
- 11. Thank You