Henry's law. Assumes a linear dependence of adsorbed amount with pressure.
\[n(p) = K_H p\]
Notes
The simplest method of describing adsorption on a
surface is Henry’s law. It assumes only interactions
with the adsorbate surface and is described by a
linear dependence of adsorbed amount with
increasing pressure.
It is derived from the Gibbs isotherm, by substituting
a two dimensional analogue to the ideal gas law.
From a physical standpoint, Henry's law is unrealistic as
adsorption sites
will saturate at higher pressures. However, the constant kH,
or Henry’s constant, can be thought of as a measure of the strength
of the interaction of the probe gas with the surface. At very
low concentrations of gas there is a
thermodynamic requirement for the applicability of Henry's law.
Therefore, most models reduce to the Henry equation
as \(\lim_{p \to 0} n(p)\).
Usually, Henry's law is unrealistic because the adsorption sites
will saturate at higher pressures.
Only use if your data is linear.
The Langmuir theory [1], proposed at the start of the 20th century, states that
adsorption takes place on specific sites on a surface, until
all sites are occupied.
It was originally derived from a kinetic model of gas adsorption and
is based on several assumptions.
All sites are equivalent and have the same chance of being occupied
Each adsorbate molecule can occupy one adsorption site
There are no interactions between adsorbed molecules
The rates of adsorption and desorption are proportional to the number of
sites currently free and currently occupied, respectively
Adsorption is complete when all sites are filled.
Using these assumptions we can define rates for both adsorption and
desorption. The adsorption rate \(r_a\)
will be proportional to the number of sites available on
the surface, as well as the number of molecules in the gas,
which is given by pressure.
The desorption rate \(r_d\), on the other hand, will
be proportional to the number of occupied sites and the energy
of adsorption. It is also useful to define
\(\theta = n_{ads}/n_{ads}^m\) as the fractional
surface coverage, the number of sites occupied divided by the total
sites. At equilibrium, the rate of adsorption and the rate of
desorption are equal, therefore the two equations can be combined.
The equation can then be arranged to obtain an expression for the
loading called the Langmuir model. Mathematically:
At equilibrium, the rate of adsorption and the rate of
desorption are equal, therefore the two equations can be combined.
\[k_a p (1 - \theta) = k_d \theta \exp{\Big(-\frac{E_{ads}}{R_gT}\Big)}\]
Rearranging to get an expression for the loading, the Langmuir equation becomes:
\[n(p) = n_m \frac{K p}{1 + K p}\]
Here, \(n_m\) is the moles adsorbed at the completion of the
monolayer, and therefore the maximum possible loading.
The Langmuir constant is the product of the individual desorption
and adsorption constants \(k_a\) and \(k_d\) and exponentially
related to the energy of adsorption
\(\exp{(-\frac{E}{RT})}\).
An extension to the Langmuir model is to consider the experimental isotherm to be
the sum of several Langmuir-type isotherms with different monolayer capacities and
affinities [2]. The assumption is that the adsorbent presents several distinct
types of homogeneous adsorption sites, and that separate Langmuir equations
should be applied to each. This is particularly applicable in cases where the
structure of the adsorbent suggests that different types of sites are present,
such as in crystalline materials of variable chemistry like zeolites and MOFs.
The resulting isotherm equation is:
\[n(p) = \sum_i n_{m_i} \frac{K_i p}{1+K_i p}\]
In practice, up to three adsorption sites are considered.
This model is the dual-site model (\(i=2\))
An extension to the Langmuir model is to consider the experimental isotherm
to be the sum of several Langmuir-type isotherms with different monolayer
capacities and affinities [3]. The assumption is that the adsorbent
material presents several distinct types of homogeneous adsorption sites,
and that separate Langmuir equations should be applied to each. This is
particularly applicable in cases where the structure of the adsorbent
suggests that different types of sites are present, such as in crystalline
materials of variable chemistry like zeolites and MOFs. The resulting
isotherm equation is:
\[n(p) = \sum_i n_{m_i}\frac{K_i p}{1+K_i p}\]
In practice, up to three adsorption sites are considered.
This model is the triple-site model (\(i=3\)).
\[n(p) = n_m \frac{C p}{(1 - N p)(1 - N p + C p)}\]
Notes
Like the Langmuir model, the BET model [4]
assumes that adsorption is kinetically driven and takes place on
adsorption sites at the material surface. However, each adsorbed
molecule becomes, in itself, a secondary adsorption site, such
that incremental layers are formed. The conditions imagined by
the BET model are:
The adsorption sites are equivalent, and therefore the surface is heterogeneous
There are no lateral interactions between adsorbed molecules
The adsorption occurs in layers, with adsorbed molecules acting as
adsorption sites for new molecules
The adsorption energy of a molecule on the second and higher layers equals
the condensation energy of the adsorbent \(E_L\).
A particular surface percentage \(\theta_x\) is occupied with x layers.
For each layer at equilibrium, the adsorption and desorption rates must be
equal. We can then apply the Langmuir theory for each layer. It is assumed
that the adsorption energy of a molecule on the second and higher layers is
just the condensation energy of the adsorbent \(E_{i>1} = E_L\).
\[ \begin{align}\begin{aligned}k_{a_1} p \theta_0 &= k_{d_1} \theta_1 \exp{(-\frac{E_1}{R_gT})}\\k_{a_2} p \theta_1 &= k_{d_2} \theta_2 \exp{(-\frac{E_L}{R_gT})}\\...\\k_{a_i} p \theta_{i-1} &= k_{d_i} \theta_i \exp{-\frac{E_L}{R_gT}}\end{aligned}\end{align} \]
Since we are assuming that all layers beside the first have the same properties,
we can define \(g= \frac{k_{d_2}}{k_{a_2}} = \frac{k_{d_3}}{k_{a_3}} = ...\).
The coverages \(\theta\) can now be expressed in terms of \(\theta_0\).
\[ \begin{align}\begin{aligned}\theta_1 &= y \theta_0 \quad where \quad y = \frac{k_{a_1}}{k_{d_1}} p \exp{(-\frac{E_1}{R_gT})}\\\theta_2 &= x \theta_1 \quad where \quad x = \frac{p}{g} \exp{(-\frac{E_L}{R_gT})}\\\theta_3 &= x \theta_2 = x^2 \theta_1\\...\\\theta_i &= x^{i-1} \theta_1 = y x^{i-1} \theta_0\end{aligned}\end{align} \]
A constant C may be defined such that
\[ \begin{align}\begin{aligned}C = \frac{y}{x} = \frac{k_{a_1}}{k_{d_1}} g \exp{(\frac{E_1 - E_L}{R_gT})}\\\theta_i = C x^i \theta_0\end{aligned}\end{align} \]
For all the layers, the equations can be summed:
\[\frac{n}{n_m} = \sum_{i=1}^{\infty} i \theta^i = C \sum_{i=1}^{\infty} i x^i \theta_0\]
\[n(p) = \frac{n}{n_m} = n_m\frac{C p}{(1-N p)(1-N p+ C p)}\]
The BET constant C is exponentially proportional to the
difference between the surface adsorption energy and the
intermolecular attraction, and can be seen to influence the knee
a BET-type isotherm has at low pressure, before statistical
monolayer formation.
\[n(p) = n_m \frac{C K p}{(1 - K p)(1 - K p + C K p)}\]
Notes
An extension of the BET model which introduces a constant
K, accounting for a different enthalpy of adsorption of
the adsorbed phase when compared to liquefaction enthalpy of
the bulk phase.
It is often used to fit adsorption and desorption isotherms of
water in the food industry. [5]
Warning: this model is not physically consistent as it
does not converge to a maximum plateau.
Notes
The Freundlich [6] isotherm model is an empirical attempt to
modify Henry's law in order to account for adsorption site
saturation by using a decreasing slope with increased loading.
It should be noted that the model never converges to a
"maximum", and therefore is not strictly physically consistent.
However, it is often good for fitting experimental data before
complete saturation.
There are two parameters which define the model:
A surface interaction constant K denoting the interaction with the
material surface.
An exponential term m accounting for the decrease in available
adsorption sites at higher loading.
The model can also be derived from a more physical basis,
using the potential theory of Polanyi, essentially resulting in
a Dubinin-Astakov model where the exponential is equal to 1.
The pressure passed should be in a relative basis.
Notes
The Dubinin-Radushkevich isotherm model [7] extends the potential theory of
Polanyi, which asserts that molecules near a surface are subjected to a
potential field. The adsorbate at the surface is in a liquid state and its
local pressure is conversely equal to the vapour pressure at the adsorption
temperature. The Polanyi theory attempts to relate the surface coverage with
the Gibbs free energy of adsorption,
\(\Delta G^{ads} = - R T \ln p/p_0\) and the total coverage
\(\theta\).
There are two parameters which define the model:
The total amount adsorbed (n_t), analogous to the monolayer capacity in
the Langmuir model.
A potential energy term e.
It describes adsorption in a single uniform type of pores. To note
that the model does not reduce to Henry's law at low pressure
and is therefore not strictly physical.
The pressure passed should be in a relative basis.
Notes
The Dubinin-Astakov isotherm model [8] extends the
Dubinin-Radushkevich model, itself based on the potential theory
of Polanyi, which asserts that molecules
near a surface are subjected to a potential field.
The adsorbate at the surface is in a liquid state and
its local pressure is conversely equal to the vapour pressure
at the adsorption temperature. The Polanyi theory attempts to
relate the surface coverage with the Gibbs free energy of adsorption,
\(\Delta G^{ads} = - R T \ln p/p_0\) and the total coverage
\(\theta\).
There are three parameters which define the model:
The total amount adsorbed (n_t), analogous to the monolayer capacity in
the Langmuir model.
A potential energy term e.
A power term, m, which can vary between 1 and 3. The DA model becomes
the DR model when m=2.
It describes adsorption in a single uniform type of pores. To note
that the model does not reduce to Henry's law at low pressure
and is therefore not strictly physical.
The quadratic adsorption isotherm exhibits an inflection point; the loading
is convex at low pressures but changes concavity as it saturates, yielding
an S-shape. The S-shape can be explained by adsorbate-adsorbate attractive
forces; the initial convexity is due to a cooperative
effect of adsorbate-adsorbate attractions aiding in the recruitment of
additional adsorbate molecules [9].
The parameter \(K_a\) can be interpreted as the Langmuir constant; the
strength of the adsorbate-adsorbate attractive forces is embedded in
\(K_b\). It is often useful in systems where the energy of guest-guest
interactions is actually higher than the energy of adsorption, such as when
adsorbing water on a hydrophobic surface.
\[n(p) = n_m \frac{K p}{1 + K p} + n_m \theta (\frac{K p}{1 + K p})^2 (\frac{K p}{1 + K p} -1)\]
Notes
The Temkin adsorption isotherm [10], like the Langmuir model, considers
a surface with n_m identical adsorption sites, but takes into account adsorbate-
adsorbate interactions by assuming that the enthalpy of adsorption is a linear
function of the coverage. The Temkin isotherm is derived [11] using a
mean-field argument and used an asymptotic approximation
to obtain an explicit equation for the loading.
Here, \(n_m\) and K have the same physical meaning as in the Langmuir model.
The additional parameter \(\theta\) describes the strength of the adsorbate-adsorbate
interactions (\(\theta < 0\) for attractions).
The Toth model is an empirical modification to the Langmuir equation.
The parameter \(t\) is a measure of the system heterogeneity.
Thanks to this additional parameter, the Toth equation can accurately describe a
large number of adsorbent/adsorbate systems and is such as
hydrocarbons, carbon oxides, hydrogen sulphide and alcohols on
activated carbons and zeolites.
\[n(p) = K p \Big[1 + \Big(\frac{K p}{(a (1 + b p)}\Big)^c\Big]^{-1/c}\]
Notes
When modelling adsorption in micropores, a requirement was highlighted by
Jensen and Seaton in 1996 [12], that at sufficiently high pressures the
adsorption isotherm should not reach a horizontal plateau corresponding
to saturation but that this asymptote should continue to rise due to
the compression of the adsorbate in the pores. They came up with a
semi-empirical equation to describe this phenomenon based on a function
that interpolates between two asymptotes: the Henry’s law asymptote
at low pressure and an asymptote reflecting the compressibility of the
adsorbate at high pressure.
Here \(K\) is the Henry constant, \(b\) is the compressibility of the
adsorbed phase and \(c\) an empirical constant.
The equation can be used to model both absolute and excess adsorption as
the pore volume can be incorporated into the definition of \(b\),
although this can lead to negative adsorption slopes for the
compressibility asymptote. This equation has been found to provide a
better fit for experimental data from microporous solids than the Langmuir
or Toth equation, in particular for adsorbent/adsorbate systems with
high Henry’s constants where the amount adsorbed increases rapidly at
relatively low pressures and then slows down dramatically.
It has been applied with success to describe the behaviour of standard as
well as supercritical isotherms. The factors are usually empirical,
although some relationship with physical can be determined:
the first constant is related to the Henry constant at zero loading, while
the second constant is a measure of the interaction strength with the surface.
\[K_1 = -\ln{K_{H,0}}\]
In practice, besides the first constant, only 2-3 factors are used.
As a part of the Vacancy Solution Theory (VST) family of models, it is based on concept
of a “vacancy” species, denoted v, and assumes that the system consists of a
mixture of these vacancies and the adsorbate [13].
The VST model is defined as follows:
A vacancy is an imaginary entity defined as a vacuum space which acts as
the solvent in both the gas and adsorbed phases.
The properties of the adsorbed phase are defined as excess properties in
relation to a dividing surface.
The entire system including the material are in thermal equilibrium
however only the gas and adsorbed phases are in thermodynamic equilibrium.
The equilibrium of the system is maintained by the spreading pressure
which arises from a potential field at the surface
It is possible to derive expressions for the vacancy chemical potential in both
the adsorbed phase and the gas phase, which when equated give the following equation
of state for the adsorbed phase:
\[\pi = - \frac{R_g T}{\sigma_v} \ln{y_v x_v}\]
where \(y_v\) is the activity coefficient and \(x_v\) is the mole fraction of
the vacancy in the adsorbed phase.
This can then be introduced into the Gibbs equation to give a general isotherm equation
for the Vacancy Solution Theory where \(K_H\) is the Henry’s constant and
\(f(\theta)\) is a function that describes the non-ideality of the system based
on activity coefficients:
The general VST equation requires an expression for the activity coefficients.
The Wilson equation can be used, which expresses the activity coefficient in terms
of the mole fractions of the two species (adsorbate and vacancy) and two constants
\(\Lambda_{1v}\) and \(\Lambda_{1v}\). The equation becomes:
Flory-Huggins Vacancy Solution Theory isotherm model.
Notes
As a part of the Vacancy Solution Theory (VST) family of models, it is based on concept
of a “vacancy” species, denoted v, and assumes that the system consists of a
mixture of these vacancies and the adsorbate [14].
The VST model is defined as follows:
A vacancy is an imaginary entity defined as a vacuum space which acts as
the solvent in both the gas and adsorbed phases.
The properties of the adsorbed phase are defined as excess properties in
relation to a dividing surface.
The entire system including the adsorbent are in thermal equilibrium
however only the gas and adsorbed phases are in thermodynamic equilibrium.
The equilibrium of the system is maintained by the spreading pressure
which arises from a potential field at the surface
It is possible to derive expressions for the vacancy chemical potential in both
the adsorbed phase and the gas phase, which when equated give the following equation
of state for the adsorbed phase:
\[\pi = - \frac{R_g T}{\sigma_v} \ln{y_v x_v}\]
where \(y_v\) is the activity coefficient and \(x_v\) is the mole fraction of
the vacancy in the adsorbed phase.
This can then be introduced into the Gibbs equation to give a general isotherm equation
for the Vacancy Solution Theory where \(K_H\) is the Henry’s constant and
\(f(\theta)\) is a function that describes the non-ideality of the system based
on activity coefficients:
The general VST equation requires an expression for the activity coefficients.
Cochran [15] developed a simpler, three
parameter equation based on the Flory – Huggins equation for the activity coefficient.
The equation then becomes: