7.3 KiB
| title | chunk | source | category | tags | date_saved | instance |
|---|---|---|---|---|---|---|
| Adsorption | 1/6 | https://en.wikipedia.org/wiki/Adsorption | reference | science, encyclopedia | 2026-05-05T10:45:47.677105+00:00 | kb-cron |
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.
Like surface tension, adsorption is a consequence of surface energy. In a bulk material, all the bonding requirements (be they ionic, covalent, or metallic) of the constituent atoms of the material are fulfilled by other atoms in the material. However, atoms on the surface of the adsorbent are not wholly surrounded by other adsorbent atoms and therefore can attract adsorbates. The exact nature of the bonding depends on the details of the species involved, but the adsorption process is generally classified as physisorption (characteristic of weak van der Waals forces) or chemisorption (characteristic of covalent bonding). It may also occur due to electrostatic attraction. The nature of the adsorption can affect the structure of the adsorbed species. For example, polymer physisorption from solution can result in squashed structures on a surface. Adsorption is present in many natural, physical, biological, and chemical systems and is widely used in industrial applications such as heterogeneous catalysts, activated charcoal, capturing and using waste heat to provide cold water for air conditioning and other process requirements (adsorption chillers), synthetic resins, increasing storage capacity of carbide-derived carbons and water purification. Adsorption, ion exchange, and chromatography are sorption processes in which certain adsorbates are selectively transferred from the fluid phase to the surface of insoluble, rigid particles suspended in a vessel or packed in a column. Pharmaceutical industry applications, which use adsorption as a means to prolong neurological exposure to specific drugs or parts thereof, are lesser known. The word "adsorption" was coined in 1881 by German physicist Heinrich Kayser (1853–1940).
== Isotherms == The adsorption of gases and solutes is usually described through isotherms, that is, the amount of adsorbate on the adsorbent as a function of its pressure (if gas) or concentration (for liquid phase solutes) at constant temperature. The quantity adsorbed is nearly always normalized by the mass of the adsorbent to allow comparison of different materials. A number of different isotherm models have been developed.
=== Freundlich ===
The first mathematical fit to an isotherm was published by Freundlich and Kuster (1906) and is a purely empirical formula for gaseous adsorbates:
x
m
=
k
P
1
/
n
,
{\displaystyle {\frac {x}{m}}=kP^{1/n},}
where
x
{\displaystyle x}
is the mass of adsorbate adsorbed,
m
{\displaystyle m}
is the mass of the adsorbent,
P
{\displaystyle P}
is the pressure of adsorbate (this can be changed to concentration if investigating solution rather than gas), and
k
{\displaystyle k}
and
n
{\displaystyle n}
are empirical constants for each adsorbent–adsorbate pair at a given temperature. The function is not adequate at very high pressure because in reality
x
/
m
{\displaystyle x/m}
has an asymptotic maximum as pressure increases without bound. As the temperature increases, the constants
k
{\displaystyle k}
and
n
{\displaystyle n}
change to reflect the empirical observation that the quantity adsorbed rises more slowly and higher pressures are required to saturate the surface.
=== Langmuir ===
Irving Langmuir was the first to derive a scientifically based adsorption isotherm in 1918. The model applies to gases adsorbed on solid surfaces. It is a semi-empirical isotherm with a kinetic basis and was derived based on statistical thermodynamics. It is the most common isotherm equation to use due to its simplicity and its ability to fit a variety of adsorption data. It is based on four assumptions:
All of the adsorption sites are equivalent, and each site can only accommodate one molecule. The surface is energetically homogeneous, and adsorbed molecules do not interact. There are no phase transitions. At the maximum adsorption, only a monolayer is formed. Adsorption only occurs on localized sites on the surface, not with other adsorbates. These four assumptions are seldom all true: there are always imperfections on the surface, adsorbed molecules are not necessarily inert, and the mechanism is clearly not the same for the first molecules to adsorb to a surface as for the last. The fourth condition is the most troublesome, as frequently more molecules will adsorb to the monolayer; this problem is addressed by the BET isotherm for relatively flat (non-microporous) surfaces. The Langmuir isotherm is nonetheless the first choice for most models of adsorption and has many applications in surface kinetics (usually called Langmuir–Hinshelwood kinetics) and thermodynamics. Langmuir suggested that adsorption takes place through this mechanism:
A
g
+
S
⇌
A
S
{\displaystyle A_{\text{g}}+S\rightleftharpoons AS}
, where A is a gas molecule, and S is an adsorption site. The direct and inverse rate constants are k and k−1. If we define surface coverage,
θ
{\displaystyle \theta }
, as the fraction of the adsorption sites occupied, in the equilibrium we have:
K
=
k
k
−
1
=
θ
(
1
−
θ
)
P
,
{\displaystyle K={\frac {k}{k_{-1}}}={\frac {\theta }{(1-\theta )P}},}
or
θ
=
K
P
1
+
K
P
,
{\displaystyle \theta ={\frac {KP}{1+KP}},}