Brunauer–Emmett–Teller (BET) theory aims to explain the physical adsorption of gas molecules on a solid surface and serves as the basis for an important analysis technique for the measurement of the specific surface area of materials. The observations are very often referred to as physical adsorption or physisorption. In 1938, Stephen Brunauer, Paul Hugh Emmett, and Edward Teller presented their theory in the Journal of the American Chemical Society.^[1] BET theory applies to systems of multilayer adsorption that usually utilizes a probing gas (called the adsorbate) that does not react chemically with the adsorptive (the material upon which the gas attaches to) to quantify specific surface area. Nitrogen is the most commonly employed gaseous adsorbate for probing surface(s). For this reason, standard BET analysis is most often conducted at the boiling temperature of N₂ (77 K). Other probing adsorbates are also utilized, albeit less often, allowing the measurement of surface area at different temperatures and measurement scales. These include argon, carbon dioxide, and water. Specific surface area is a scale-dependent property, with no single true value of specific surface area definable, and thus quantities of specific surface area determined through BET theory may depend on the adsorbate molecule utilized and its adsorption cross section.^[2]

Concept

BET model of multilayer adsorption, that is, a random distribution of sites covered by one, two, three, etc., adsorbate molecules.

The concept of the theory is an extension of the Langmuir theory, which is a theory for monolayer molecular adsorption, to multilayer adsorption with the following hypotheses:

1. gas molecules physically adsorb on a solid in layers infinitely;
2. gas molecules only interact with adjacent layers; and
3. the Langmuir theory can be applied to each layer.
4. the enthalpy of adsorption for the first layer is constant and greater than the second (and higher).
5. the enthalpy of adsorption for the second (and higher) layers is the same as the enthalpy of liquefaction.

The resulting BET equation is

${\displaystyle \theta ={\frac {cp}{(1-p/p_{o}){\bigl (}p_{o}+p(c-1){\bigr )}}}}$

where c is referred to as the BET C-constant, ${\displaystyle p_{o}}$is the vapor pressure of the adsorptive bulk liquid phase which would be at the temperature of the adsorbate and θ is the surface coverage, defined as:

${\displaystyle \theta =n_{ads}/n_{m}}$.

Here ${\displaystyle n_{ads}}$is the amount of adsorbate and ${\displaystyle n_{m}}$ is called the monolayer equivalent. The ${\displaystyle n_{m}}$ is the entire amount that would be present as a monolayer (which is theoretically impossible for physical adsorption) would cover the surface with exactly one layer of adsorbate. The above equation is usually rearranged to yield the following equation for the ease of analysis:

${\displaystyle {\frac {{p}/{p_{0}}}{v\left[1-\left({p}/{p_{0}}\right)\right]}}={\frac {c-1}{v_{\mathrm {m} }c}}\left({\frac {p}{p_{0}}}\right)+{\frac {1}{v_{m}c}},\qquad (1)}$

where ${\displaystyle p}$ and ${\displaystyle p_{0}}$ are the equilibrium and the saturation pressure of adsorbates at the temperature of adsorption, respectively; ${\displaystyle v}$ is the adsorbed gas quantity (for example, in volume units) while ${\displaystyle v_{\mathrm {m} }}$ is the monolayer adsorbed gas quantity. ${\displaystyle c}$ is the BET constant,

${\displaystyle c=\exp \left({\frac {E_{1}-E_{\mathrm {L} }}{RT}}\right),\qquad (2)}$

where ${\displaystyle E_{1}}$ is the heat of adsorption for the first layer, and ${\displaystyle E_{\mathrm {L} }}$ is that for the second and higher layers and is equal to the heat of liquefaction or heat of vaporization.

BET plot

Equation (1) is an adsorption isotherm and can be plotted as a straight line with ${\displaystyle 1/{v[({p_{0}}/{p})-1]}}$ on the y-axis and ${\displaystyle \varphi ={p}/{p_{0}}}$ on the x-axis according to experimental results. This plot is called a BET plot. The linear relationship of this equation is maintained only in the range of ${\displaystyle 0.05<{p}/{p_{0}}<0.35}$. The value of the slope ${\displaystyle A}$ and the y-intercept ${\displaystyle I}$ of the line are used to calculate the monolayer adsorbed gas quantity ${\displaystyle v_{\mathrm {m} }}$ and the BET constant ${\displaystyle c}$. The following equations can be used:

${\displaystyle v_{m}={\frac {1}{A+I}}\qquad (3)}$

${\displaystyle c=1+{\frac {A}{I}}.\qquad (4)}$

The BET method is widely used in materials science for the calculation of surface areas of solids by physical adsorption of gas molecules. The total surface area ${\displaystyle S_{\mathrm {total} }}$ and the specific surface area ${\displaystyle S_{\mathrm {BET} }}$ are given by

${\displaystyle S_{\mathrm {total} }={\frac {\left(v_{\mathrm {m} }Ns\right)}{V}},\qquad (5)}$

${\displaystyle S_{\mathrm {BET} }={\frac {S_{\mathrm {total} }}{a}},\qquad (6)}$

where ${\displaystyle v_{\mathrm {m} }}$ is in units of volume which are also the units of the monolayer volume of the adsorbate gas, ${\displaystyle N}$ is the Avogadro number, ${\displaystyle s}$ the adsorption cross section of the adsorbate,^[3] ${\displaystyle V}$ the molar volume of the adsorbate gas, and ${\displaystyle a}$ the mass of the solid sample or adsorbent.

Derivation

The BET theory can be derived similarly to the Langmuir theory, but by considering multilayered gas molecule adsorption, where it is not required for a layer to be completed before an upper layer formation starts. Furthermore, the authors made five assumptions:^[4]

1. Adsorptions occur only on well-defined sites of the sample surface (one per molecule)
2. The only molecular interaction considered is the following one: a molecule can act as a single adsorption site for a molecule of the upper layer.
3. The uppermost molecule layer is in equilibrium with the gas phase, i.e. similar molecule adsorption and desorption rates.
4. The desorption is a kinetically limited process, i.e. a heat of adsorption must be provided:
   • these phenomena are homogeneous, i.e. same heat of adsorption for a given molecule layer.
   • it is E₁ for the first layer, i.e. the heat of adsorption at the solid sample surface
   • the other layers are assumed similar and can be represented as condensed species, i.e. liquid state. Hence, the heat of adsorption is E_L is equal to the heat of liquefaction.
5. At the saturation pressure, the molecule layer number tends to infinity (i.e. equivalent to the sample being surrounded by a liquid phase)

Consider a given amount of solid sample in a controlled atmosphere. Let θ_i be the fractional coverage of the sample surface covered by a number i of successive molecule layers. Let us assume that the adsorption rate R_ads,i-1 for molecules on a layer (i-1) (i.e. formation of a layer i) is proportional to both its fractional surface θ_i-1 and to the pressure P, and that the desorption rate R_des,i on a layer i is also proportional to its fractional surface θ_i:

${\displaystyle R_{\mathrm {ads} ,i-1}=k_{i}P\Theta _{i-1}}$

${\displaystyle R_{\mathrm {des} ,i}=k_{-i}\Theta _{i},}$

where k_i and k_−i are the kinetic constants (depending on the temperature) for the adsorption on the layer (i−1) and desorption on layer i, respectively. For the adsorptions, these constants are assumed similar whatever the surface. Assuming an Arrhenius law for desorption, the related constants can be expressed as

${\displaystyle k_{i}=\exp(-E_{i}/RT),}$

where E_i is the heat of adsorption, equal to E₁ at the sample surface and to E_L otherwise.

Consider some substance A. The adsorption of A onto an available surface site ${\displaystyle (*)_{0}}$ produces a new site ${\displaystyle (*)_{1}}$ on the first layer. In summary,

${\displaystyle {\ce {A(g) +}}}$ ${\displaystyle (*)_{0}}$ ${\displaystyle {\ce {<=>}}}$ ${\displaystyle (*)_{1}}$

Extending this to higher order layers one obtains

${\displaystyle {\ce {A(g) +}}}$ ${\displaystyle (*)_{1}}$ ${\displaystyle {\ce {<=>}}}$ ${\displaystyle (*)_{2}}$

and similarly

${\displaystyle {\ce {A(g) +}}}$ ${\displaystyle (*)}$_{${\displaystyle n-1}$} ${\displaystyle {\ce {<=>}}}$ ${\displaystyle (*)_{n}}$

Denoting the activity of the number of available sites of the ${\displaystyle n}$th layer with ${\displaystyle \theta _{n}}$ and the partial pressure of A with ${\displaystyle P}$, the last equilibrium can be written

${\displaystyle K_{n}={\frac {\theta _{n}}{P\theta _{n-1}}}}$

It follows that the coverage of the first layer can be written

${\displaystyle \theta _{1}=K_{1}P\theta _{0}}$

and that the coverage of the second layer can be written

${\displaystyle \theta _{2}=K_{2}P\theta _{1}=K_{2}PK_{1}P\theta _{0}}$

Realising that the adsorption of A onto the second layer is equivalent to adsorption of A onto its own liquid phase,^[5] the rate constant for ${\displaystyle n>1}$ should be the same, which results in the recursion

${\displaystyle \theta _{n}=(K_{\ell }P)^{n-1}PK_{1}\theta _{0}}$

In order to simplify some infinite summations, let ${\displaystyle x=K_{\ell }P}$ and let ${\displaystyle y=K_{1}P}$. Then the ${\displaystyle n}$th layer coverage can written

${\displaystyle \theta _{n}=c\theta _{0}x^{n},\quad n>0}$

if ${\displaystyle c=y/x}$. The coverage of any layer is defined as the relative number of available sites. An alternative definition, which leads to a set of coverage's that are numerically to those resulting from the original way of defining surface coverage, is that ${\displaystyle \theta _{n}}$ denotes the relative number of sites covered by only ${\displaystyle n}$ adsorbents.^[5] Doing so it is easy to see that the total volume of adsorbed molecules can be written as the sum

${\displaystyle V_{\text{ads}}=V_{\text{m}}\sum _{n=1}^{\infty }n\theta _{n}=V_{\text{m}}c\theta _{0}x\sum _{n=1}^{\infty }nx^{n-1}}$

where ${\displaystyle V_{\text{m}}}$ is the molecular volume. Employing the fact that this sum is the first derivative of a geometric sum, the volume becomes

${\displaystyle V_{\text{ads}}=V_{\text{m}}c\theta _{0}{\frac {x}{(1-x)^{2}}},\quad |x|<1}$

Since the total coverage of a mono-layer must be unity, the full mono-layer coverage must be

${\displaystyle 1=\sum _{n=1}^{\infty }\theta _{n}}$

In order to properly make the substitution for ${\displaystyle \theta _{n}}$, the restriction ${\displaystyle n>1}$ forces us to take the zeroth contribution outside the summation, resulting in

${\displaystyle \sum _{n=1}^{\infty }\theta _{n}=\theta _{0}+c\theta _{0}x\sum _{n=0}^{\infty }x^{n}=\theta _{0}+c\theta _{0}{\frac {x}{1-x}},\quad |x|<1}$

Lastly, defining the excess coverage as ${\displaystyle V_{\text{excess}}=V_{\text{ads}}/V_{\text{m}}}$, the excess volume relative to the volume of an adsorbed mono-layer becomes

${\displaystyle V_{\text{excess}}={\frac {\sum _{n=0}^{\infty }n\theta _{n}}{1}}={\frac {\sum _{n=0}^{\infty }n\theta _{n}}{\sum _{n=0}^{\infty }\theta _{n}}}={\frac {cx}{(1-x)(1+(c-1)x)}}}$

where the last equality was obtained by making use of the series expansions presented above. The constant ${\displaystyle c}$ must be interpreted as the relative binding affinity the substance A has towards a surface, relative to its own liquid. If ${\displaystyle c>1}$ then the initial part of the isotherm will be reminiscent of the Langmuir isotherm which reaches a plateau at full mono-layer coverage, whereas ${\displaystyle c<1}$ means the mono-layer will have a slow build-up. Another thing to note is that in order for the geometric substitutions to hold, ${\displaystyle x<1}$. The isotherm above exhibits a singularity at ${\displaystyle x^{\ast }=1}$. Since ${\displaystyle x=K_{\ell }P}$ one can write ${\displaystyle x^{\ast }=K_{\ell }P^{\ast }}$, implying that ${\displaystyle K_{\ell }=1/P^{\ast }}$. This means that ${\displaystyle x=P/P^{\ast }}$ must be true, ultimately resulting in ${\displaystyle x\in [0,1)}$.

Finding the linear BET range

It is still not clear on how to find the linear range of the BET plot for microporous materials in a way that reduces any subjectivity in the assessment of the monolayer capacity. A crowd-sourced study involving 61 research groups has shown that reproducibility of BET area determination from identical isotherms is, in some cases, problematic.^[6] Rouquerol et al.^[7] suggested a procedure that is based on two criteria:

• C must be positive implying that any negative intercept on the BET plot indicates that one is outside the valid range of the BET equation.
• Application of the BET equation must be limited to the range where the term V(1-P/P₀) continuously increases with P/P₀.

These corrections are an attempt to salvage the BET theory, which is restricted to type II isotherms. Even while using this type, use of the data itself is restricted to 0.05 to 0.35 of ${\displaystyle P/P_{0}}$, routinely discarding 70% of the data. This restriction must be modified depending upon conditions.

Limitations of BET

Terrell L. Hill described BET as a theory that is "... extremely useful as a qualitative guide; but it is not quantitatively correct".^[8] Although BET adsorption isotherm is still extensively used for different applications and is used for specific surface area determinations of powders whose calculation is not sensitive to the simplifications of the BET theory.^[8] Both Hackerman's^[9] and Sing's group^[10] have highlighted the limitations of the BET method.^[11] Hackerman et al. noted the potential for 10% uncertainty in the method's values,^[9] with Sing's group attributed the significant variation in reported values of molecular area to the BET method's possible inaccurate assessment of monolayer capacity.^[11] In subsequent studies using the BET interpretation of nitrogen and water vapor adsorption isotherms, the reported area occupied by an adsorbed water molecule on fully hydroxylated silica ranged from 0.25 to 0.44 nm².^[11] Other issues with the BET include the fact that in certain cases, BET leads to anomalies such as reaching an infinite amount adsorbed at ${\displaystyle P/P_{0}}$ reaching unity,^[12] and in some cases, the constant C (surface binding energy) can be determined to be negative.^[13]

Applications

See also

• Adsorption
• Capillary condensation
• Langmuir adsorption model
• Mercury intrusion porosimetry
• Physisorption
• Surface tension

References