**1. Introduction**

162 Thermodynamics – Interaction Studies – Solids, Liquids and Gases

Polzin, K. L.; J. M. Toole; J. R. Ledwell & R. W. Schmitt (1997). Spatial Variability of

Sandström, J. W. (1908). Dynamische Versuche mit Meerwasser, *Annalen der Hydrographie* 

Sandström, J. W. (1916). Meteorologische Studien im Schwedischen Hochgebirge, *Göteborgs Kungl. Vetenskaps- och Vitterhetssamhälles Handlingar*, Vol. 17, pp. 1–48 Sawada, Y. (1981). A Thermodynamic Variational Principle in Nonlinear Non-equilibrium

Shimokawa, S., & H. Ozawa (2001). On the Thermodynamics of the Oceanic General

Shimokawa, S., & H. Ozawa (2002). On the Thermodynamics of the Oceanic General

Shimokawa, S. (2002). Thermodynamics of the Oceanic General Circulation: Entropy Increase Rate of a Fluid System (PhD thesis), The University of Tokyo, Tokyo Shimokawa, S., & H. Ozawa (2007). Thermodynamics of Irreversible Transitions in the

Toggweiler, J. R. (1994). The Ocean's Overturning Circulation, *Physics Today*, Vol. 47, pp. 45-

Yamagata, T. (1996). The Ocean Determining Decadal and Centurial Climate Variability (in

Wunsch, C. (1998). The Work Done by the Wind on the Oceanic General Circulation, *J. Phys.* 

Wunsch, C., & R. Ferrari (2004). Vertical Mixing, Energy, and the General Circulation of the

Circulation: Entropy Increase Rate of an Open Dissipative System and its

Circulation: Irreversible Transition to a State with Higher Rate of Entropy

Oceanic General Circulation, *Geophys. Res. Lett.,* Vol. 34, L12606,

Japanese), In *Kikou Hendouron (Climate Variability)*, A. Sumi (Ed.), 69-101, Iwanami

Turbulent Mixing in the Abyssal Ocean, *Science*, Vol. 276, pp. 93–96

*und Maritimen Meteorologie*, Vol. 36, pp. 6–23

Surroundings, *Tellus*, Vol. A53, pp. 266–277

doi:10.1029/2007GL030208

Shoten, ISBN 4-00-010731-3, Tokyo

*Oceanogr.,* Vol. 28, pp. 2332–2340

Whitfield, J. (2005). Order Out of Chaos, *Nature*, Vol. 436, pp. 905–907

Oceans, *Ann. Rev. Fluid Mech.,* Vol. 36, pp. 281–314

50

Phenomena, *Prog. Theor. Phys.,* Vol. 66, pp. 68–76

Production, *Q. J. R. Meteorol. Soc.,* Vol. 128, pp. 2115–2128

For decades the man has had to face one of the major problems resulting from technological development and global population growth, environmental pollution, which has impacted on the different systems of life. The impacts of technological progress attained by man, have necessitated the establishment of international rules and regulations that set limits and establish a balance between development and the effects caused by the same (**Rodríguez 2003, Callister 2007, Rodriguez-Reinoso, 2007**). For this reason, we have launched various alternative solutions to environmental problems, including the synthesis and use of porous materials from organic waste or waste products with high carbon content, has been successful mainly in catalysis, adsorption and gas separation.

Activated carbon is a material that consists of microcrystals elementary hexagonal planes which are not well targeted, but displaced relative to each other and overlapping each other, so they have a high percentage of highly disordered structure. In fact there are hexagonal folding sheets with spaces of varying size (usually less than 2 nm) which make up the porosity of the material (**Marsh & Rodriguez-Reinoso, 2006**). These characteristics confer an exceptionally high surface area and good absorbent properties can be exploited in different areas. The production of activated carbon is linked to the purification of products and environmental protection. To the extent that the demands of purity of products require more sophisticated processes and emissions standards become more stringent, the activated carbon evolves, the production of the classic styles granular and powder have been joined by other like fibers, fabrics, monoliths among others (**Blanco et al., 2000**). Forms of activated carbon that are known and marketed, recent studies have shown that the monoliths exhibit characteristics that differentiate them from conventional ways, including the following highlights: allow the passage of gases with a very drop small, have a high geometric surface per unit weight / volume, the gas flow is very uniform, with easy handling, resistance to friction, reduce the constraints generated by phenomena of internal diffusion and mass transfer, these properties the have become used as support materials or adsorbents that favor direct adsorption process in the gas phase (**Nakagawa et al., 2007**).

Thermodynamic of the Interactions Between

In which, *<sup>a</sup>*

system will:

In which:

*a U n*

Gas-Solid and Solid-Liquid on Carbonaceous Materials 165

Adsorption is a simple and attractive method for removing contaminants in aqueous phase, due to its high efficiency and easy handling. Given that the adsorption phenomenon is clearly exothermic, it is possible to characterize all the interactions inherent in the process of adsorption. For this purpose we describe the phenomenon of adsorption in terms of energy: If the interaction is solid-gas, may be the differential molar enthalpy of adsorption from the molar internal energy of the adsorbed phase and energy Ua adsorbate molar Ug, then, the

*<sup>a</sup> <sup>a</sup> <sup>g</sup> <sup>a</sup>*

*<sup>U</sup> UU U*

This change in molar internal energy of the system is the integral molar energy of adsorption, ΔUa, which depends on interactions adsorbate-adsorbate and adsorbate-

When an infinitesimal amount of moles of adsorbate, dna, is transferred to the solid surface from the gas phase at constant volume, the change in internal energy of the

> , *<sup>a</sup> <sup>a</sup>*

Where Ha and Hg are the molar enthalpies of the adsorbate adsorbed state and gas phase.

 , *<sup>a</sup> <sup>a</sup>*

With the theoretical basis described above, it is possible to know then the extent of heat evolved in the adsorption process, known as heat of adsorption and is defined as a

*<sup>H</sup> <sup>H</sup> n*

thermodynamic function, which can be used to characterize the surface of a solid .

*a T P*

*<sup>U</sup> <sup>U</sup> n*

*a T A*

adsorbent. Ua is the average molar internal energy, for all the adsorbed molecules.

Where *Ua* = is the differential molar energy of adsorption, and is defined as:

= is the molar energy change of the system, caused by the transfer of n moles

(1)

*UUU a a <sup>g</sup>* (2)

*HHH a a <sup>g</sup>* (4)

*<sup>g</sup> HHH a a* (5)

(3)

(6)

change in internal energy as a result of adsorption can be represented as:

*a*

*n*

of adsorbate from the gas phase to the adsorbed state.

Similar to what was expressed for energy,

Likewise, the differential molar adsorption enthalpy is:

There are two ways of expressing the heat of adsorption:

In addition to their interesting adsorptive properties, during the process of obtaining activated carbons it is possible to modify and / or design their properties through a treatment of pre-or post-synthesis in order to obtain materials. These materials can be intended for more specific uses taking into consideration that the adsorption capacity of activated carbon depends on its textural characteristics and also on its surface chemistry (**Dias** *et al***. 2007, Petit et al. 2010**). The surface chemistry of activated carbon is determined by the presence of atoms different from carbon atoms in graphene layers also known as heteroatoms, the most common are: oxygen, hydrogen and nitrogen. These heteroatoms produce a wide variety of surface groups, these groups can be acidic such as: carboxylic, lactone, anhydride and phenolic, while the basic character is attributed to groups such as quinones, pyrones besides of the delocalized π electrons in graphene layers or with a neutral character like carbonyl and ether (**Montes-Moran** *et al***. 2004,Rivera-Utrilla & Sanchez-Polo. 2003**); surface groups determine parameters such as acidity and total basicity, surface charge and hydrophobicity, this will depend mainly on the type and concentration of groups on the surface of activated carbon.

Surface chemistry of activated carbon can be modified mainly by oxidation treatments and controlled thermal treatments that promote the formation and / or selective removal of different groups, as reported by Figueiredo and Pereira 2010. The role of surface chemistry in adsorption of gases, metal ions and organic molecules, is mainly due to specific interactions between surface groups and the different species.

In general, any organic material with relatively high carbon content is capable of being transformed into activated carbon. The activated carbon produced by manufacturing can come from wood and forest residues or other biomass (peat, lignite and other coals) as well as various polymers and natural or synthetic fibers. The factors that must be taken into account when choosing a suitable precursor are good availability and low cost, low mineral content and the resulting carbon possesses good mechanical properties and adsorption capacity. Wood waste, coconut shells, nuts, seeds and fruits along with some coals and petroleum coke are the most commonly used precursors (**Giraldo et al. 2008**). The complexity of the structure of activated carbon, can be characterized textural, chemical and energy by using different techniques among which include: physical adsorption of gases or vapors, scanning electron microscopy (SEM), electron microscopy transmission (TEM), infrared spectroscopy (FT-IR), X-ray diffraction, temperature programmed desorption (TPD), mercury porosimetry, immersion calorimetry and adsorption rates of methylene blue adsorption, density, size, moisture , ash, abrasion resistance and other parameters applicable to the specifications of coal (**Marsh & Rodriguez-Reinoso, 2006**).

The most common use is given to activated carbon adsorption processes of pollutants in liquid and gas phase. Adsorption is a process by which atoms, ions or molecules are trapped or retained on the surface of a material, which is different from absorption, which involves volume. This process involves an adsorbent, which in this case is activated carbon and adsorbate, which is the contaminant retained

The adsorption is exothermic, which can be classified as chemical or physical, depending on the magnitude of the interactions established between the retained material and the adsorbent surface. The amount of material that accumulates depends on the dynamic equilibrium is reached between the rate at which the material is adsorbed to the surface and the speed at which it evaporates or releases, in turn, they usually depend importantly on temperature.

In addition to their interesting adsorptive properties, during the process of obtaining activated carbons it is possible to modify and / or design their properties through a treatment of pre-or post-synthesis in order to obtain materials. These materials can be intended for more specific uses taking into consideration that the adsorption capacity of activated carbon depends on its textural characteristics and also on its surface chemistry (**Dias** *et al***. 2007, Petit et al. 2010**). The surface chemistry of activated carbon is determined by the presence of atoms different from carbon atoms in graphene layers also known as heteroatoms, the most common are: oxygen, hydrogen and nitrogen. These heteroatoms produce a wide variety of surface groups, these groups can be acidic such as: carboxylic, lactone, anhydride and phenolic, while the basic character is attributed to groups such as quinones, pyrones besides of the delocalized π electrons in graphene layers or with a neutral character like carbonyl and ether (**Montes-Moran** *et al***. 2004,Rivera-Utrilla & Sanchez-Polo. 2003**); surface groups determine parameters such as acidity and total basicity, surface charge and hydrophobicity, this will depend mainly on the type and concentration of groups on

Surface chemistry of activated carbon can be modified mainly by oxidation treatments and controlled thermal treatments that promote the formation and / or selective removal of different groups, as reported by Figueiredo and Pereira 2010. The role of surface chemistry in adsorption of gases, metal ions and organic molecules, is mainly due to specific

In general, any organic material with relatively high carbon content is capable of being transformed into activated carbon. The activated carbon produced by manufacturing can come from wood and forest residues or other biomass (peat, lignite and other coals) as well as various polymers and natural or synthetic fibers. The factors that must be taken into account when choosing a suitable precursor are good availability and low cost, low mineral content and the resulting carbon possesses good mechanical properties and adsorption capacity. Wood waste, coconut shells, nuts, seeds and fruits along with some coals and petroleum coke are the most commonly used precursors (**Giraldo et al. 2008**). The complexity of the structure of activated carbon, can be characterized textural, chemical and energy by using different techniques among which include: physical adsorption of gases or vapors, scanning electron microscopy (SEM), electron microscopy transmission (TEM), infrared spectroscopy (FT-IR), X-ray diffraction, temperature programmed desorption (TPD), mercury porosimetry, immersion calorimetry and adsorption rates of methylene blue adsorption, density, size, moisture , ash, abrasion resistance and other parameters applicable

The most common use is given to activated carbon adsorption processes of pollutants in liquid and gas phase. Adsorption is a process by which atoms, ions or molecules are trapped or retained on the surface of a material, which is different from absorption, which involves volume. This process involves an adsorbent, which in this case is activated carbon and

The adsorption is exothermic, which can be classified as chemical or physical, depending on the magnitude of the interactions established between the retained material and the adsorbent surface. The amount of material that accumulates depends on the dynamic equilibrium is reached between the rate at which the material is adsorbed to the surface and the speed at which it evaporates or releases, in turn, they usually depend importantly on

interactions between surface groups and the different species.

to the specifications of coal (**Marsh & Rodriguez-Reinoso, 2006**).

adsorbate, which is the contaminant retained

temperature.

the surface of activated carbon.

Adsorption is a simple and attractive method for removing contaminants in aqueous phase, due to its high efficiency and easy handling. Given that the adsorption phenomenon is clearly exothermic, it is possible to characterize all the interactions inherent in the process of adsorption. For this purpose we describe the phenomenon of adsorption in terms of energy: If the interaction is solid-gas, may be the differential molar enthalpy of adsorption from the molar internal energy of the adsorbed phase and energy Ua adsorbate molar Ug, then, the change in internal energy as a result of adsorption can be represented as:

$$\frac{\Delta \mathcal{U}\_a}{m\_a} = \overline{\mathcal{U}\_a} - \overline{\mathcal{U}}\_{\mathcal{S}} = \Delta \overline{\mathcal{U}}\_a \tag{1}$$

In which, *<sup>a</sup> a U n* = is the molar energy change of the system, caused by the transfer of n moles

of adsorbate from the gas phase to the adsorbed state.

This change in molar internal energy of the system is the integral molar energy of adsorption, ΔUa, which depends on interactions adsorbate-adsorbate and adsorbateadsorbent. Ua is the average molar internal energy, for all the adsorbed molecules.

When an infinitesimal amount of moles of adsorbate, dna, is transferred to the solid surface from the gas phase at constant volume, the change in internal energy of the system will:

$$
\overline{\Delta \mathcal{U}\_a} = \overline{\mathcal{U}\_a} - \overline{\mathcal{U}\_g} \tag{2}
$$

Where *Ua* = is the differential molar energy of adsorption, and is defined as:

$$\overline{\mathcal{U}\mathcal{U}\_a} = \left(\frac{\partial \mathcal{U}\mathcal{U}\_a}{\partial \mathfrak{n}\_a}\right)\_{T,A} \tag{3}$$

Similar to what was expressed for energy,

$$
\Delta H\_a = H\_a - H\_g \tag{4}
$$

Where Ha and Hg are the molar enthalpies of the adsorbate adsorbed state and gas phase. Likewise, the differential molar adsorption enthalpy is:

$$
\Delta \overline{H\_a} = \overline{H\_a} - \overline{H}\_{\mathcal{S}} \tag{5}
$$

In which:

$$
\overline{H\_a} = \left(\frac{\partial H\_a}{\partial \mathfrak{n}\_a}\right)\_{T,P} \tag{6}
$$

With the theoretical basis described above, it is possible to know then the extent of heat evolved in the adsorption process, known as heat of adsorption and is defined as a thermodynamic function, which can be used to characterize the surface of a solid . There are two ways of expressing the heat of adsorption:

Thermodynamic of the Interactions Between

Thus, equation (10) can be written as:

**Piraján & Giraldo 2007**).

adsorbent surface as follows

where hi is specific enthalpy in J/m2. As the external surface is defined as:

So, the external surface may be known as:

Gas-Solid and Solid-Liquid on Carbonaceous Materials 167

1 1 1 1 2 2

0

*T E HE d <sup>d</sup>* (10)

*E T <sup>H</sup>* (13)

 

1 1 ln ln

0 0

*para p*

*para p*

 

Which is valid for the micropores filling, in activated carbons at temperature T (**Moreno-**

For a coal with a micropore volume Wo and an adsorbate with a molar volume Vm, Stoeckli and colleagues established a relationship between the enthalpy of different types of activated carbons in various body fluids and the parameters obtained by adsorption of vapors of these liquids on the same solid. In the equation of Stoeckli and Krahenbüehl

2

Where β is the adsorbate affinity coefficient, E0 is the characteristic free energy of adsorption of vapor of reference, W0 is the total volume of micropores of the solid, is the coefficient of

The immersion in a nonpolar solvent, which is known molecular dimensions, and generate a thermal effect only by filling the micropores of the solid, relates the thermal effect of the

exp

*<sup>i</sup> <sup>i</sup> ext i i*

*<sup>H</sup> <sup>H</sup> <sup>S</sup>*

.

*E W*

*V*

*m*

 

*<sup>o</sup> <sup>i</sup>*

*<sup>o</sup> <sup>o</sup> <sup>i</sup>*

<sup>222</sup> ( 1) 1 1

<sup>1</sup> ln ( 1) *p*

*dx p*

 

2

1 3 :

> : 2 2

 (1 )

(1 )

*T*

(14)

*H H hS* exp. *i i ext*. (15)

*h h* (16)

2 *i o*

*x*

*p*

(**Moreno-Piraján & Giraldo 2007, Stoekli & Kraehenbuehl 1989**):

*H*

thermal expansion at temperature T, and Vm is the volume molar.

Which corresponds to the immersion enthalpy Hi , en J/g.

The solution for the integrals of this type, is a function gamma ( (x) )

1

0

(11)

(12)

*Integral heat of adsorption*, amount of heat, Q, released when one gram of solid adsorbent adsorbs x grams. Its units are Joules / gram of adsorbent.

*Differential heat of adsorption*, ΔH, amount of heat generated when x moles of adsorbate adsorbed. Its units are Joules / mole of adsorbate.

The differential heat of adsorption is also known as isosteric heat of adsorption and can be determined by using calorimetry or by adsorption isotherms, measured at two or more temperatures. (**Bansal et al. 1988, Moreno-Piraján & Giraldo, 2007**).

On the other hand, it is necessary to know the pore structure of the solid. Thus, for microporous solids without external surface (**Kraus 1955**), ΔHi immersion enthalpy is related to the isosteric heat of adsorption qisost by the expression:

$$-\Delta H\_i(T) = \int\_0^1 q^{i\text{osst.}}(T; \Theta) d\Theta - \Delta H\_{vap.}(T) \tag{7}$$

Where:

#### = degree of volume filling W/Wo

The negative sign is because qisost convention is positive, while Hi is negative. Dubinin **(Moreno-Piraján & Giraldo 2007, Dubinin 1975)** define of net Heat of adsorption (qnet ) as:

$$q^{net} = q^{\text{isost.}} - \Delta H\_{cap}$$

0

when ΔHvap is vaporization enthalpy.

For the general case of n, the above equation becomes:

$$q^{net} = E\_0 \left[ \left( \ln \frac{n\_a^o}{n\_a} \right)^{\frac{1}{n}} + \left( \frac{\alpha T}{n} \right) \left( \ln \frac{n\_a^o}{n\_a} \right)^{\left( \frac{1}{n} \right) - 1} \right] \tag{8}$$

.

Donde,

 = Thermal expansion coefficient of adsorbate na = Amount adsorbed at relative pressure P/Po na = Amount adsorbed ar relative pressure P/Po Eo= Characteristic energy for vapor adsorption

= Micropore filling degree

For activated carbons with n=2

$$q^{net} = \beta E\_o \text{I} \left[ \ln \frac{1}{\Theta} \right]^{\frac{1}{2}} + \left( \frac{aT}{2} \right) \left( \ln \frac{1}{\Theta} \right)^{-\left( \frac{1}{2} \right)} \text{I} \tag{9}$$

$$-\Delta H\_i = \int q^{net} d\Theta$$

By replacing in equation (9):

*Integral heat of adsorption*, amount of heat, Q, released when one gram of solid adsorbent

*Differential heat of adsorption*, ΔH, amount of heat generated when x moles of adsorbate

The differential heat of adsorption is also known as isosteric heat of adsorption and can be determined by using calorimetry or by adsorption isotherms, measured at two or more

On the other hand, it is necessary to know the pore structure of the solid. Thus, for microporous solids without external surface (**Kraus 1955**), ΔHi immersion enthalpy is

> 1

> > 0

The negative sign is because qisost convention is positive, while Hi is negative.

.

= degree of volume filling W/Wo

Dubinin **(Moreno-Piraján & Giraldo 2007, Dubinin 1975)** define of net Heat of adsorption

.

 

 

> 1

0 *net H qd <sup>i</sup>*

1 1 1 1 2 2 [ ln ln ] <sup>2</sup>

*<sup>T</sup> q E* (9)

*o*

*net*

*n nn*

*a a*

<sup>0</sup> ln ln *o o n n net a a*

*n n <sup>T</sup> q E*

*net isost vap qq H*

.

1 1 <sup>1</sup>

 

(8)

.

() (; ) () *isost HT q T d H T <sup>i</sup> vap* (7)

adsorbs x grams. Its units are Joules / gram of adsorbent.

temperatures. (**Bansal et al. 1988, Moreno-Piraján & Giraldo, 2007**).

related to the isosteric heat of adsorption qisost by the expression:

adsorbed. Its units are Joules / mole of adsorbate.

Where:

(qnet ) as:

Donde,

when ΔHvap is vaporization enthalpy.

 = Micropore filling degree For activated carbons with n=2

By replacing in equation (9):

For the general case of n, the above equation becomes:

 = Thermal expansion coefficient of adsorbate na = Amount adsorbed at relative pressure P/Po na = Amount adsorbed ar relative pressure P/Po Eo= Characteristic energy for vapor adsorption

$$-\Delta H\_i = \beta E\_o \int\_0^1 \left(\ln \frac{1}{\Theta}\right)^{\frac{1}{2}} d\Theta + \frac{\alpha T \beta E\_0}{2} \int\_0^1 \left(\ln \frac{1}{\Theta}\right)^{-\frac{1}{2}} d\Theta \tag{10}$$

The solution for the integrals of this type, is a function gamma ( (x) )

$$\int\_0^1 \ln\left(\frac{1}{\varkappa}\right)^p d\mathbf{x} = \Gamma(p+1) \tag{11}$$

$$\Gamma(p+1) = \begin{cases} para \, p = \frac{1}{2} : \Gamma\left(\frac{3}{2}\right) = \frac{\sqrt{\pi}}{2} \\\\ para \, p = -\frac{1}{2} : \Gamma\left(\frac{1}{2}\right) = \sqrt{\pi} \end{cases} \tag{12}$$

Thus, equation (10) can be written as:

$$
\Delta H\_i = -\frac{\beta \mathcal{E}\_o \sqrt{\pi} (1 + aT)}{2} \tag{13}
$$

Which is valid for the micropores filling, in activated carbons at temperature T (**Moreno-Piraján & Giraldo 2007**).

For a coal with a micropore volume Wo and an adsorbate with a molar volume Vm, Stoeckli and colleagues established a relationship between the enthalpy of different types of activated carbons in various body fluids and the parameters obtained by adsorption of vapors of these liquids on the same solid. In the equation of Stoeckli and Krahenbüehl (**Moreno-Piraján & Giraldo 2007, Stoekli & Kraehenbuehl 1989**):

$$
\Delta H\_i = -\frac{\beta \sum\_o \mathcal{V} \mathcal{V}\_o \mathcal{N} \pi (1 + aT)}{2V\_m} \tag{14}
$$

Which corresponds to the immersion enthalpy Hi , en J/g.

Where β is the adsorbate affinity coefficient, E0 is the characteristic free energy of adsorption of vapor of reference, W0 is the total volume of micropores of the solid, is the coefficient of thermal expansion at temperature T, and Vm is the volume molar.

The immersion in a nonpolar solvent, which is known molecular dimensions, and generate a thermal effect only by filling the micropores of the solid, relates the thermal effect of the adsorbent surface as follows

$$
\Delta H\_{\text{exp.}} = \Delta H\_i + h\_i S\_{\text{ext.}} \tag{15}
$$

where hi is specific enthalpy in J/m2. As the external surface is defined as:

$$S\_{ext.} = \frac{\Delta H\_{i \text{exp}}}{h\_i} - \frac{\Delta H\_i}{h\_i} \tag{16}$$

So, the external surface may be known as:

Thermodynamic of the Interactions Between

the current (I) and heating time (t).

transfer of heat.

solid-liquid system.

(**Rouquerol et al. 1999**).

solid-liquid interaction.

Gas-Solid and Solid-Liquid on Carbonaceous Materials 169

supplied can be calculated if one knows the potential (Eh) through the heating resistor (Rh),

Thermometric system for measuring thermal effect, which consists of different types of sensors, which can be proportional to the temperature or property connected with the

According to the system you want to measure, you must use a specific calorimetric system.

For many years, immersion microcalorimetry has been a useful technique for the characterization of powders and porous solids like activated carbons and oxides (Hemminger & Höhne 1984). Technique involves immersing a known quantity of a solid in a specific liquid, and measure the heat generated due to wet the solid, liquid immersion. In the absence of complex effects such as filling of micropores, is usually taken as a first approximation, the energy due to the immersion of a solid degassed ΔimUo, which is

in which the energy of immersion per unit area, Δimui,o is characteristic of the nature of

When ΔimU, is known for a given solid-liquid system, the adsorbent surface (A) can be evaluated. When the surface of the sample of adsorbent is less than 1 m2, generates heat due to immersion, which is easily measured by colorimetric procedures and therefore the immersion microcalorimetry can be used to evaluate the specific surface of adsorbent

Immersion calorimetry is a useful technique to assess the total area and size distribution of micropores of a microporous carbon (**Denoyel et al.1993**), assuming that the energy of the dip is proportional to the area available for liquid immersion to any size and shape of the pores. In addition, it is assumed, from the point of view of energy per unit external surface area of solid has the same behavior (**Rouquerol et al. 1999, Hemminger & Höhne 1984**). The Figure 1 shows the immersion calorimetric heat conduction unit. To experimentally measure the immersion heat, the adsorbent is immersed in the liquid which is to determine the interaction. You can use a microcalorimeter heat conduction, which is expected to be reached thermal equilibrium between all components of the calorimetric system: the cell containing the immersion liquid, the vial containing the solid under study, a heating pad for perform system calibration, temperature sensors should be arranged around the cell containing the immersion fluid and the surroundings. To achieve this, the entire system must be completely insulated from temperature fluctuations. Once thermal equilibrium is reached, it is the breaking of the ampoule to allow liquid to come into contact and the adsorbent, it ends with an electrical calibration. Throughout the experiment, recorded the potential generated by the sensors, should have the thermal effect sensor thermocouples or thermopiles and evaluates the area under the curve of the signal generated in response to

Below is a brief description of immersion calorimetry and sorption

*Immersion calorimetry, measurement of solid-liquid interactions.* 

proportional to the solid surface, A, according to Equation 21:

*W Eh I t elect* (20)

, *im* . *im o i <sup>o</sup> U Au* (21)

$$S\_{\text{ext.}} = A\_{\text{TOTAL}} - A\_{\text{MICROPOP.}} \tag{17}$$

For a solid contribution also presents the mesopores and macropores, the total area is expressed as:

$$A\_{\text{TOTAL}} = A\_{\text{MICROP.}} + A\_{\text{MESOP.}} + A\_{\text{MACROP.}} + S\_{\text{abireta.}} \tag{18}$$

Where,

ATOTAL: Total area

AMICROP: Microporous area

AMESOP: Mesoporous area AMACROP: Macroporous area

SABIERTA: Open area non-poorus

When activated carbon presents neither external surface nor development of meso and macropores, the experimental enthalpy will:

$$
\Delta H\_{\text{exp}} = \Delta H\_i \tag{19}
$$

determinate by equation (15).

Until here, have been described the theoretical foundations of solid-gas interactions and solid-liquid, which can calculate the magnitude of the thermal effect generated and the type of interaction between the adsorbate and the adsorbent, which is proportional to the affinity between them, and allows for relationships that give an approximation of the surface area of adsorbent.

Now, referring to such calorimetric techniques, such as immersion calorimetry and adsorption for measuring the thermal effect of the interaction of a solid with a liquid or gas, which leads to determine the thermodynamic variables in different interfaces: solid-liquid, solid-gas and liquid-liquid, which provide valuable information about the behavior of the solid. Such is the importance of these techniques, which in recent years, several studies are focused on the design, construction and development of immersion calorimeters adsorption.

#### *Calorimetric technique*

Calorimetry is a technique used to measure a large number of processes that generate heat in their development, and which can determine the enthalpy changes DH and combination with other techniques to obtain the free energy change ΔG and entropy changes ΔS. Furthermore, this technique has been used to study physical and chemical events that occur on the surface of a solid. (**Moreno 1996**).

However, there is a team that is capable of performing all the above measures at a time, so different equipment should be used according to the type of study that you want to perform and the amount of heat generated in the system. For this reason, there are combustion calorimeters, adsorption and immersion, which basically consist of:

Calorimetric cell, which should be designed with a capacity that is associated with the type of sensors require the calorimeter and additionally must have regard to the material of construction depending on the system to be studied. In this cell are often attached a heating sample holder.

Electrical calibration system, which consists of an electrical circuit which provides power to the calorimeter to determine the constant of the system under study. Electrical work

For a solid contribution also presents the mesopores and macropores, the total area is

When activated carbon presents neither external surface nor development of meso and

Until here, have been described the theoretical foundations of solid-gas interactions and solid-liquid, which can calculate the magnitude of the thermal effect generated and the type of interaction between the adsorbate and the adsorbent, which is proportional to the affinity between them, and allows for relationships that give an approximation of the surface area of

Now, referring to such calorimetric techniques, such as immersion calorimetry and adsorption for measuring the thermal effect of the interaction of a solid with a liquid or gas, which leads to determine the thermodynamic variables in different interfaces: solid-liquid, solid-gas and liquid-liquid, which provide valuable information about the behavior of the solid. Such is the importance of these techniques, which in recent years, several studies are focused on the design, construction and development of immersion calorimeters adsorption.

Calorimetry is a technique used to measure a large number of processes that generate heat in their development, and which can determine the enthalpy changes DH and combination with other techniques to obtain the free energy change ΔG and entropy changes ΔS. Furthermore, this technique has been used to study physical and chemical events that occur

However, there is a team that is capable of performing all the above measures at a time, so different equipment should be used according to the type of study that you want to perform and the amount of heat generated in the system. For this reason, there are combustion

Calorimetric cell, which should be designed with a capacity that is associated with the type of sensors require the calorimeter and additionally must have regard to the material of construction depending on the system to be studied. In this cell are often attached a heating

Electrical calibration system, which consists of an electrical circuit which provides power to the calorimeter to determine the constant of the system under study. Electrical work

calorimeters, adsorption and immersion, which basically consist of:

expressed as:

ATOTAL: Total area

AMICROP: Microporous area AMESOP: Mesoporous area AMACROP: Macroporous area SABIERTA: Open area non-poorus

determinate by equation (15).

macropores, the experimental enthalpy will:

Where,

adsorbent.

*Calorimetric technique* 

sample holder.

on the surface of a solid. (**Moreno 1996**).

*SA A ext TOTAL MICROPO* . . (17)

*H H* exp *<sup>i</sup>* (19)

*AA A A S TOTAL MICROP MESOP MACROP abierta* . . .. (18)

supplied can be calculated if one knows the potential (Eh) through the heating resistor (Rh), the current (I) and heating time (t).

$$\mathcal{W}\_{\text{left}} = \text{Ely} \ast I \ast \text{t} \tag{20}$$

Thermometric system for measuring thermal effect, which consists of different types of sensors, which can be proportional to the temperature or property connected with the transfer of heat.

According to the system you want to measure, you must use a specific calorimetric system. Below is a brief description of immersion calorimetry and sorption

*Immersion calorimetry, measurement of solid-liquid interactions.* 

For many years, immersion microcalorimetry has been a useful technique for the characterization of powders and porous solids like activated carbons and oxides (Hemminger & Höhne 1984). Technique involves immersing a known quantity of a solid in a specific liquid, and measure the heat generated due to wet the solid, liquid immersion.

In the absence of complex effects such as filling of micropores, is usually taken as a first approximation, the energy due to the immersion of a solid degassed ΔimUo, which is proportional to the solid surface, A, according to Equation 21:

$$
\Delta\_{\rm in} \mathcal{U}^{\boldsymbol{o}} = A.\Delta\_{\rm in} \boldsymbol{u}^{\boldsymbol{i},\boldsymbol{o}} \tag{21}
$$

in which the energy of immersion per unit area, Δimui,o is characteristic of the nature of solid-liquid system.

When ΔimU, is known for a given solid-liquid system, the adsorbent surface (A) can be evaluated. When the surface of the sample of adsorbent is less than 1 m2, generates heat due to immersion, which is easily measured by colorimetric procedures and therefore the immersion microcalorimetry can be used to evaluate the specific surface of adsorbent (**Rouquerol et al. 1999**).

Immersion calorimetry is a useful technique to assess the total area and size distribution of micropores of a microporous carbon (**Denoyel et al.1993**), assuming that the energy of the dip is proportional to the area available for liquid immersion to any size and shape of the pores. In addition, it is assumed, from the point of view of energy per unit external surface area of solid has the same behavior (**Rouquerol et al. 1999, Hemminger & Höhne 1984**).

The Figure 1 shows the immersion calorimetric heat conduction unit. To experimentally measure the immersion heat, the adsorbent is immersed in the liquid which is to determine the interaction. You can use a microcalorimeter heat conduction, which is expected to be reached thermal equilibrium between all components of the calorimetric system: the cell containing the immersion liquid, the vial containing the solid under study, a heating pad for perform system calibration, temperature sensors should be arranged around the cell containing the immersion fluid and the surroundings. To achieve this, the entire system must be completely insulated from temperature fluctuations. Once thermal equilibrium is reached, it is the breaking of the ampoule to allow liquid to come into contact and the adsorbent, it ends with an electrical calibration. Throughout the experiment, recorded the potential generated by the sensors, should have the thermal effect sensor thermocouples or thermopiles and evaluates the area under the curve of the signal generated in response to solid-liquid interaction.

Thermodynamic of the Interactions Between

Gas-Solid and Solid-Liquid on Carbonaceous Materials 171

Figure 2 shows a typical thermogram obtained for the immersion of an activated carbon pellet ore (CAP), in benzene. It can be seen in the range of 0 to 500 seconds, the baseline obtained, which illustrates the heat balance and low noise level in the calorimetric signal. Table 1 shows the values of surface properties obtained by immersion calorimetry, for this

> **Wo** cm3/g

The sample CAPRED is a modification of CAP, obtained by heating the same until 1373 K, under nitrogen, for 3h. CAPN65 sample is a sample obtained by modification of CAP through the impregnation of CAP with 65% HNO3 and heating it to 473 K, for 2 hours. As shown in Table 1, the modification with HNO3 and 65% did not produce a significant change in the surface properties of the sample. This behavior is attributed to the low temperature at which it made the change, which did not affect the porous structure of the solid. The modification to 1373K nitrogen affected the pore structure of the solid, reducing the volume of micropores and consequently, the surface area there of in Figure 3 shows the

**SBET** m2/g

same sample, two samples obtained by the modification of the CAP.

kJ/mol

CAP 7.47 0.43 1248 CAPRED 6.48 0.38 1089 CAPN65 7.47 0.43 1253 Table 1. Surface properties obtained for three activated carbons by gas adsorption

Fig. 3. Nitrogen adsorption isotherms at 77 K, for the three carbons under study

The isotherm can be observed further that the sample has CAPRED mesoporosity development, so it appears the hysteresis loop in it. CAP and CAPN65 isotherms are

Sample **Eo**

isotherms of nitrogen at 77 K for these three samples.

Fig. 1. Calorimeter immersion scheme Tian type. (1)Sensors System; (2) Sample cell; (3) Sample; (4) Heat Sink; (5) Heat resistance for calibration; (6) Insulation jacket; (7) Output of resistance to power supply; (8) Output of sensors system to interface multimeter.

Fig. 2. Thermogram obtained for the immersion of an activated carbon pellet ore (CAP), in benzene

Fig. 1. Calorimeter immersion scheme Tian type. (1)Sensors System; (2) Sample cell; (3) Sample; (4) Heat Sink; (5) Heat resistance for calibration; (6) Insulation jacket; (7) Output of

Fig. 2. Thermogram obtained for the immersion of an activated carbon pellet ore (CAP), in

benzene

resistance to power supply; (8) Output of sensors system to interface multimeter.

Figure 2 shows a typical thermogram obtained for the immersion of an activated carbon pellet ore (CAP), in benzene. It can be seen in the range of 0 to 500 seconds, the baseline obtained, which illustrates the heat balance and low noise level in the calorimetric signal. Table 1 shows the values of surface properties obtained by immersion calorimetry, for this same sample, two samples obtained by the modification of the CAP.


Table 1. Surface properties obtained for three activated carbons by gas adsorption

The sample CAPRED is a modification of CAP, obtained by heating the same until 1373 K, under nitrogen, for 3h. CAPN65 sample is a sample obtained by modification of CAP through the impregnation of CAP with 65% HNO3 and heating it to 473 K, for 2 hours.

As shown in Table 1, the modification with HNO3 and 65% did not produce a significant change in the surface properties of the sample. This behavior is attributed to the low temperature at which it made the change, which did not affect the porous structure of the solid. The modification to 1373K nitrogen affected the pore structure of the solid, reducing the volume of micropores and consequently, the surface area there of in Figure 3 shows the isotherms of nitrogen at 77 K for these three samples.

Fig. 3. Nitrogen adsorption isotherms at 77 K, for the three carbons under study

The isotherm can be observed further that the sample has CAPRED mesoporosity development, so it appears the hysteresis loop in it. CAP and CAPN65 isotherms are

Thermodynamic of the Interactions Between

Gas-Solid and Solid-Liquid on Carbonaceous Materials 173

From these results we can see good correlation between the results obtained by the two methods compared, which shows a correlation coefficient of 0.9836, confirming that immersion calorimetry is a characterization parameter for solid-liquid interactions. You could make a more exhaustive with probe molecules of different sizes to benzene, since the

There are several reasons to determine the heat of adsorption to characterize the surface energy of materials (**Rouquerol et al. 1999**), provide basic data for development of new theories of equilibrium and kinetics of adsorption (**Zimmermann & Keller 2003**), design and plants improve separation processes by adsorption and desorption, PSA, VSA, TSA and

Adsorption calorimetry in combination with other physical or chemical properties to describe the properties of a solid surface (**Garcia-Cuello et al. 2009, Llewellyn & Maurin** 

To experimentally measure the heat of adsorption, calorimetric unit is used as shown in

Fig. 5. Adsorption calorimeter scheme. (1) Adsorbate, (2) precision valves, (3) needle valve, (4) Volume calibration, (5) pressure transducer 1 to 1000mbar, (6) pressure transducer 10-4 to 1 mbar , (7) measuring cell, (8) reference cell, (9) Calorimeter adsorption (10) thermopile sensors in 3D layout type, (11) thermostat, (12) Rotary Vacuum Pump, (13) Pump ultra high

pore size distribution can affect the calorimetric data (**Molina-Sabio et al. 2008**).

*Adsorption calorimetry, measurement of solid-gas interactions.* 

**2005, Garcia-Cuello et al. 2008, Moreno & Giraldo 2005**).

their combinations (**Ruthven 1984, Yang 1997**).

Figure 5.

vacuum

virtually identical, confirming that the modification with 65% HNO3 shows no effect on the texture of activated carbon.

Table 2 shows the surface properties obtained by immersion calorimetry for these three samples


Table 2. Surface properties obtained for three activated carbons by immersion calorimetry in benzene

The results for ΔHinm, from equation (14). and ΔHexp are the experimental results. The external surface area Sext , of micropores AMICROP, and the total area Atotal, were obtained from the equations (16), (17) and (18) respectively.

Table 3 shows the parameters used for calculations of surface properties obtained by immersion calorimetry into benzene.


Table 3. Physical characteristics of benzene.

Figure 4 shows a relationship between the areas obtained by gas adsorption and that obtained by immersion calorimetry.

Fig. 4. Relationship between the total area obtained by adsorption calorimetry and nitrogen adsorption.

virtually identical, confirming that the modification with 65% HNO3 shows no effect on the

Table 2 shows the surface properties obtained by immersion calorimetry for these three

Table 2. Surface properties obtained for three activated carbons by immersion calorimetry in

The results for ΔHinm, from equation (14). and ΔHexp are the experimental results. The external surface area Sext , of micropores AMICROP, and the total area Atotal, were obtained

Table 3 shows the parameters used for calculations of surface properties obtained by

**α Β Vm**  1,24E-03 1 88,9

Figure 4 shows a relationship between the areas obtained by gas adsorption and that

Fig. 4. Relationship between the total area obtained by adsorption calorimetry and nitrogen

CAP 37 -44 -48 1219 1256 CAPRED 55 -33 -39 1065 1120 CAPN65 64 -34 -41 1219 1283

**ΔHexp J/g** 

**AMICROP m2/g** 

**Atotal m2/g** 

**ΔHimm J/g** 

texture of activated carbon.

**m2/g** 

immersion calorimetry into benzene.

obtained by immersion calorimetry.

Table 3. Physical characteristics of benzene.

from the equations (16), (17) and (18) respectively.

**Sample Sext**

samples

benzene

adsorption.

From these results we can see good correlation between the results obtained by the two methods compared, which shows a correlation coefficient of 0.9836, confirming that immersion calorimetry is a characterization parameter for solid-liquid interactions. You could make a more exhaustive with probe molecules of different sizes to benzene, since the pore size distribution can affect the calorimetric data (**Molina-Sabio et al. 2008**).

## *Adsorption calorimetry, measurement of solid-gas interactions.*

There are several reasons to determine the heat of adsorption to characterize the surface energy of materials (**Rouquerol et al. 1999**), provide basic data for development of new theories of equilibrium and kinetics of adsorption (**Zimmermann & Keller 2003**), design and plants improve separation processes by adsorption and desorption, PSA, VSA, TSA and their combinations (**Ruthven 1984, Yang 1997**).

Adsorption calorimetry in combination with other physical or chemical properties to describe the properties of a solid surface (**Garcia-Cuello et al. 2009, Llewellyn & Maurin 2005, Garcia-Cuello et al. 2008, Moreno & Giraldo 2005**).

To experimentally measure the heat of adsorption, calorimetric unit is used as shown in Figure 5.

Fig. 5. Adsorption calorimeter scheme. (1) Adsorbate, (2) precision valves, (3) needle valve, (4) Volume calibration, (5) pressure transducer 1 to 1000mbar, (6) pressure transducer 10-4 to 1 mbar , (7) measuring cell, (8) reference cell, (9) Calorimeter adsorption (10) thermopile sensors in 3D layout type, (11) thermostat, (12) Rotary Vacuum Pump, (13) Pump ultra high vacuum

Thermodynamic of the Interactions Between

OH

N O O

**0**

Fig. 7. Adsorption isotherm of DNP on bone char

**4**

**8**

**q**

**e (mg/g)**

**12**

**16**

Fig. 6. Species of DNP in aqueous solution.

ability of adsorbent to adsorb a particular molecule.

Gas-Solid and Solid-Liquid on Carbonaceous Materials 175

The chemical properties of the adsorbent depends the surface concentration of acid and basic sites, but these are in pH function of solution because the charge on the surface depends of this property. In this study was used 2,4-Dinitrophenol (DNP) a organic compounds commonly used for tincture manufacturing, wood preservatives, explosives, substances for insects control and other chemical products **(Su-Hsia & Ruey-Shin, 2009, Tae Young et al., 2001)** that in

pKa=4.09

The adsorption isotherm represents the thermodynamic equilibrium between the adsorbed solute and the solute in solution, the obtained equilibrium data which are used to assess the

Figure 7 shows the influence of concentration on the adsorption of DNP on CHB, where the mass of solute adsorbed onto the adsorbent continues to increase when raising the

**0 10 20 30 40 50 60**

**Ce (mg/L)**

concentration of solute in equilibrium and is not asymptotic at high concentrations.

N

O

3OH <sup>+</sup> +

O

O-

N O O

aqueous solution can be found as ionic or nonionic species Figure 6.

O

+ 2OH

N

O

The heats of adsorption measured at a temperature of liquefaction of the adsorbate, in the case of nitrogen at 77 K and 273 K. CO2 For this, use a thermostat bath at that temperature. Make contact with the solid adsorbate successive small doses. This allows measure the evolution of the interaction energy compared to coverage. Before start the calorimetric measurements. To start the measurements in the microcalorimeter, initially must be empty throughout the adsorption system, including the solid sample under study, using a vacuum system that achieves at least 10-3 Torr. When the system reaches the expected vacuum level, are the respective gas injection, waiting time for a balance between system components and are simultaneously recorded volumes of gas adsorbed and the heat evolved at each injection. Developed to sense heat, temperature sensors are used thermopile type, with appropriate sensitivity to detect heat from 10 to 100 J / g. Pressure readings are made using a pressure sensor with adequate sensitivity and precision must be known in the injection volume. The differential molar adsorption energy can be obtained by equation (3), and evaluating the area under the curve obtained in the experiment, which is the signal generated by the thermopile due to solid-gas interaction which is proportional to the adsorption energy (**Garcia-Cuello et al. 2008, Garcia-Cuello et al. 2009**).

#### *Preparation, characterization, modification and use of carbonaceous Materials*

Preparation, characterization, modification and use of carbonaceous materials like activated carbon in different presentation such as: granulate, powder, pelettes, char, monoliths, among other, it has been object investigation during many years. Next are presented some results of investigations developed in the by the authors about these porous solids and their employment in the adsorption of pollutants in liquid and gas phase.

#### *Bone char in the adsorption of derivates phenolics*

The bovine bone char (BBC) have received attention by industry of treatment waste water; due to its advantages in front of others adsorbents between these are found: low cost and adsorbent versatility for wide variety pollutants **(Deyder et al., 2005)**. The BBC was prepared in the following way: The bones were cleaned from meat and fat and cut by saw to pieces of approximate size 4-10 cm. Subsequently, bones were washed with tap water for several times. The bones were then transferred to the oven for drying at 353 K. After 24 h, the dried bones were crushed and milled into different particle sizes in the range of 2-3 mm. These particles are burned in an inert atmosphere. This process was carried out in a tubular fixed bed reactor from room temperature to 1073 K for 2 h at a heating rate of 3 K min–1 and a flow of N2 80 cm3 min–1.

The adsorption from solution depends on the chemical and physical characteristics of the solid as surface area, porosity and surface chemistry, see Table 4. The study about this process has shown dependence with the solution characteristics as pH, ionic strength and temperature **(Moreno-Castilla & López-Ramos M.V., 2007)**. These factors have influence in the adsorption mechanism and in consequence, the magnitude in that the system – (solidliquid) - liberates heat.


Table 4. Physical and chemical characteristics of the BBC

The heats of adsorption measured at a temperature of liquefaction of the adsorbate, in the case of nitrogen at 77 K and 273 K. CO2 For this, use a thermostat bath at that temperature. Make contact with the solid adsorbate successive small doses. This allows measure the evolution of the interaction energy compared to coverage. Before start the calorimetric measurements. To start the measurements in the microcalorimeter, initially must be empty throughout the adsorption system, including the solid sample under study, using a vacuum system that achieves at least 10-3 Torr. When the system reaches the expected vacuum level, are the respective gas injection, waiting time for a balance between system components and are simultaneously recorded volumes of gas adsorbed and the heat evolved at each injection. Developed to sense heat, temperature sensors are used thermopile type, with appropriate sensitivity to detect heat from 10 to 100 J / g. Pressure readings are made using a pressure sensor with adequate sensitivity and precision must be known in the injection volume. The differential molar adsorption energy can be obtained by equation (3), and evaluating the area under the curve obtained in the experiment, which is the signal generated by the thermopile due to solid-gas interaction which is proportional to the

Preparation, characterization, modification and use of carbonaceous materials like activated carbon in different presentation such as: granulate, powder, pelettes, char, monoliths, among other, it has been object investigation during many years. Next are presented some results of investigations developed in the by the authors about these porous solids and their

The bovine bone char (BBC) have received attention by industry of treatment waste water; due to its advantages in front of others adsorbents between these are found: low cost and adsorbent versatility for wide variety pollutants **(Deyder et al., 2005)**. The BBC was prepared in the following way: The bones were cleaned from meat and fat and cut by saw to pieces of approximate size 4-10 cm. Subsequently, bones were washed with tap water for several times. The bones were then transferred to the oven for drying at 353 K. After 24 h, the dried bones were crushed and milled into different particle sizes in the range of 2-3 mm. These particles are burned in an inert atmosphere. This process was carried out in a tubular fixed bed reactor from room temperature to 1073 K for 2 h at a heating rate of 3 K min–1 and

The adsorption from solution depends on the chemical and physical characteristics of the solid as surface area, porosity and surface chemistry, see Table 4. The study about this process has shown dependence with the solution characteristics as pH, ionic strength and temperature **(Moreno-Castilla & López-Ramos M.V., 2007)**. These factors have influence in the adsorption mechanism and in consequence, the magnitude in that the system – (solid-

> SBET (m2 /g) 157 Pore Volume (cm3/g) 0.14 Pore Size (nm) 3.0 Acid Sites (meq/g) 0.23 Basic Sites (meq /g) 0.42 PZC 8.5

adsorption energy (**Garcia-Cuello et al. 2008, Garcia-Cuello et al. 2009**). *Preparation, characterization, modification and use of carbonaceous Materials* 

employment in the adsorption of pollutants in liquid and gas phase.

*Bone char in the adsorption of derivates phenolics* 

Table 4. Physical and chemical characteristics of the BBC

a flow of N2 80 cm3 min–1.

liquid) - liberates heat.

The chemical properties of the adsorbent depends the surface concentration of acid and basic sites, but these are in pH function of solution because the charge on the surface depends of this property. In this study was used 2,4-Dinitrophenol (DNP) a organic compounds commonly used for tincture manufacturing, wood preservatives, explosives, substances for insects control and other chemical products **(Su-Hsia & Ruey-Shin, 2009, Tae Young et al., 2001)** that in aqueous solution can be found as ionic or nonionic species Figure 6.

Fig. 6. Species of DNP in aqueous solution.

The adsorption isotherm represents the thermodynamic equilibrium between the adsorbed solute and the solute in solution, the obtained equilibrium data which are used to assess the ability of adsorbent to adsorb a particular molecule.

Figure 7 shows the influence of concentration on the adsorption of DNP on CHB, where the mass of solute adsorbed onto the adsorbent continues to increase when raising the concentration of solute in equilibrium and is not asymptotic at high concentrations.

Fig. 7. Adsorption isotherm of DNP on bone char

Thermodynamic of the Interactions Between

**0**

Fig. 9. Adsorption isotherm Freundlich model

**1**

**2**

**Ln Ce**

**3**

**4**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 177

**0,0 0,5 1,0 1,5 2,0 2,5 3,0**

**Ln qe**

Isotherm Parameter

Langmuir qm = 61.96

Freundlich K

Table 6. Isotherm parameters for Langmuir and Freundlich models.

interactions between adsorbate and surface active sites.

Values

b = 0.068

= 0.7969

= 0.8907

R2

R2

Correlating the experimental data of adsorption of DNP on BBC with both models, Figure 8 and 9 shows the typical behavior of the Freundlich isotherm, which contrasts with the parameters and correlation coefficients, see Table 6. This model describes the surface of the adsorbent is energetically heterogeneous and includes the lateral interactions between adsorbate molecules. In this type of liquid-solid systems, it is important understand that when a model fits the experimental data does not support the adsorption mechanism occurs under the principles of the model. Although these data are adjusted by mathematical methods - statistics to calculate the parameters given, these methods do not consider the

Depending on the thermodynamic conditions of the system, heat is produced when a solid comes into contact with the solution; this intensity is determined by immersion enthalpy. It is set for a specific amount of a solid and measured by a technique known as immersion

F = 0.593 n = 0.798

 **DNP**

 **Freundlich**

In the literature on liquid phase adsorption has been reported different mathematical models to represent the adsorption isotherms, the most used are the Langmuir and Freundlich model. The first assumes: (i) uniform adsorption energies on the surface, (ii) no interaction between adsorbed molecules (III) adsorption occurs at specific sites. Meanwhile, the second (I) assumes that the adsorbent surface is energetically heterogeneous, (ii) that increasing the concentration of adsorbate, increases the amount adsorbed on the surface **(Oke et al., 2008, Moreno et al., 2010)**.

Isotherm Equation Lineal Form Graphic Langmuir <sup>1</sup> *m e <sup>e</sup> e q b C <sup>q</sup> b C* 1 11 1 *qe me m b q C q* 1 1 . *e e vs q C* Freundlich 1/*<sup>n</sup> efe q kC* <sup>1</sup> *Ln q Ln k Ln C <sup>e</sup> <sup>f</sup> <sup>e</sup> <sup>n</sup>* . *Ln e e q vs Ln C*

These models are represented mathematically as shown in table 5:

Table 5. Mathematics models of Langmuir and Freundlich.

where qe is the amount adsorbed at Ce (mg/L), concentration of DNP at equilibrium, b (L/mg), and q0 (mg/g) are the Langmuir constants related to the energy of adsorption and maximum capacity, respectively; kf (mg1-1/n l1/n g-1) and 1/n are the Freundlich constants related to the adsorption capacity and intensity, respectively; and qe (mg/g) is the mass of DNP adsorbed per mass of adsorbent.

Fig. 8. Adsorption isotherm Langmuir model

In the literature on liquid phase adsorption has been reported different mathematical models to represent the adsorption isotherms, the most used are the Langmuir and Freundlich model. The first assumes: (i) uniform adsorption energies on the surface, (ii) no interaction between adsorbed molecules (III) adsorption occurs at specific sites. Meanwhile, the second (I) assumes that the adsorbent surface is energetically heterogeneous, (ii) that increasing the concentration of adsorbate, increases the amount adsorbed on the surface

Isotherm Equation Lineal Form Graphic

where qe is the amount adsorbed at Ce (mg/L), concentration of DNP at equilibrium, b (L/mg), and q0 (mg/g) are the Langmuir constants related to the energy of adsorption and maximum capacity, respectively; kf (mg1-1/n l1/n g-1) and 1/n are the Freundlich constants related to the adsorption capacity and intensity, respectively; and qe (mg/g) is the mass of

**0,0 0,1 0,2 0,3 0,4 0,5 0,6 0,7**

**1/qe**

 1 11 1 *qe me m b q C q*

<sup>1</sup> *Ln q Ln k Ln C <sup>e</sup> <sup>f</sup> <sup>e</sup> <sup>n</sup>*

1 1 . *e e vs q C*

. *Ln e e q vs Ln C*

 **DNP**

**Langmuir**

**(Oke et al., 2008, Moreno et al., 2010)**.

Langmuir <sup>1</sup>

Freundlich 1/*<sup>n</sup>*

DNP adsorbed per mass of adsorbent.

**0,00**

Fig. 8. Adsorption isotherm Langmuir model

**0,04**

**0,08**

**1/Ce**

**0,12**

**0,16**

These models are represented mathematically as shown in table 5:

*e*

*efe q kC*

*m e <sup>e</sup>*

*q b C <sup>q</sup> b C*

Table 5. Mathematics models of Langmuir and Freundlich.

Fig. 9. Adsorption isotherm Freundlich model


Table 6. Isotherm parameters for Langmuir and Freundlich models.

Correlating the experimental data of adsorption of DNP on BBC with both models, Figure 8 and 9 shows the typical behavior of the Freundlich isotherm, which contrasts with the parameters and correlation coefficients, see Table 6. This model describes the surface of the adsorbent is energetically heterogeneous and includes the lateral interactions between adsorbate molecules. In this type of liquid-solid systems, it is important understand that when a model fits the experimental data does not support the adsorption mechanism occurs under the principles of the model. Although these data are adjusted by mathematical methods - statistics to calculate the parameters given, these methods do not consider the interactions between adsorbate and surface active sites.

Depending on the thermodynamic conditions of the system, heat is produced when a solid comes into contact with the solution; this intensity is determined by immersion enthalpy. It is set for a specific amount of a solid and measured by a technique known as immersion

Thermodynamic of the Interactions Between

equilibrium (Ce) to tfinal, by equation (22).

**0**

DNP is thermodynamically feasible.

*Granular activated carbon for adsorption of nickel* 

obtained for free energy.

**1**

**2**

**-HInm (J/g)**

**3**

**4**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 179

parameter is the fundamental criterion of spontaneity **(Smiciklas et al., 2008)**, and may be calculated considering the initial concentration (Co) and the concentration in the

**0 20 40 60 80 100**

Fig. 11. Enthalpies of immersion of BBC on DNP to different concentration.


**Concentration (mg/L)**

Where ∆G (kJ/mol) is differential free energy change; R is universal gas constant, and T (K) is absolute temperature. Reaction occurs spontaneously if G is a negative quantity. From the above equation, the differential change Gibbs free energy for the adsorption process of DNP on BBC to tfinal (293 K) is -113.0 kJ/mol, this negative value indicate that the adsorption of

In the specific case of the solution 30 mg/L which has a differential ∆Himm = -56.10 kJ/(g\*mol) and substituting the parameters known in equation (23) determine the differential entropy of the process is equivalent to 580 J/(mol K) this positive value suggests that the organization of the adsorbate in the solid-liquid interface and coincide with value

> <sup>|</sup> *tf imm ti*

*H G <sup>S</sup>*

The samples used for nickel removal were obtained from a commercial granular activated carbon made from coconut shell GAC, which was oxidized with GACoxN 6M nitric acid, two parts of this sample were treated one at 723 K and another 1023 K under nitrogen atmosphere, GACoxN723 and GACoxN1023, and a final sample obtained by heating the sample at 1173 K GAC, GAC1173, these samples were characterized by N2 physisorption at -

*<sup>C</sup> G RT Ln*

*tf <sup>o</sup> ti*

*e*

*C* (22)

*T* (23)

**Interaction Charred-Solution Interaction Charred-Adsorbate**

calorimetry **(Blanco et al., 2008)**. When make this type of measure, where contact between a solid and a solution is involved, there are different interactions that contribute to the total amount of heat produced. Among these are interactions between water and the groups on the solid's surface, the filling of pores and adsorption on the surface. Furthermore, there are also adsorption of and interactions with the solute; these depend on the characteristics of the solution **(Moreno-Piraján et al., 2007)**.

The values of the enthalpies of immersion were evaluated from the thermograms, where the heat generated by the process of adsorption is proportional to the area under the curve of the peak generated by the thermal effect. Figure 10 shows the typical thermograms for the immersion of BBC in DNP solutions of 10 and 30 mg/L.

Fig. 10. Thermograms of BBC immersion in a solution of DNP at concentrations of 10 and 30 mg/L at 298 K.

Figure 11 shows the (a) interactions between bone char and DNP in solutions at different concentrations and the (2) interactions with the adsorbate char was obtained subtracting the effect of char-water interactions.

As can be seen in the Figure 11, at low concentrations (10-30 mg/L) there was a greater interaction between the BBC and the adsorbate (DNP); however, as the concentration increased (50-100 mg/L) there was a decrease in enthalpy, i.e. weaker interactions between the adsorbent and the adsorbate.

When relating the enthalpies as a function of adsorbed amount of DNP can be seen that the enthalpy is directly proportional to the percent of retention, this behavior is due to the main morphological characteristic of the material is its heterogeneity, therefore the heat generated is different because that the adsorbate has occupied the most active sites than the immediately occupy.

The differential free energy of adsorption that occurs in the time interval, in which it is carry a calorimetry measure, is determined relating the kinetics of the process to this time interval. Where tinicial is the time in that started the immersion solid-liquid and tfinal is the time in that ended the calorimetric measurement. The free energy difference as a thermodynamic

calorimetry **(Blanco et al., 2008)**. When make this type of measure, where contact between a solid and a solution is involved, there are different interactions that contribute to the total amount of heat produced. Among these are interactions between water and the groups on the solid's surface, the filling of pores and adsorption on the surface. Furthermore, there are also adsorption of and interactions with the solute; these depend on the characteristics of the

The values of the enthalpies of immersion were evaluated from the thermograms, where the heat generated by the process of adsorption is proportional to the area under the curve of the peak generated by the thermal effect. Figure 10 shows the typical thermograms for the

Fig. 10. Thermograms of BBC immersion in a solution of DNP at concentrations of 10 and 30

Figure 11 shows the (a) interactions between bone char and DNP in solutions at different concentrations and the (2) interactions with the adsorbate char was obtained subtracting the

As can be seen in the Figure 11, at low concentrations (10-30 mg/L) there was a greater interaction between the BBC and the adsorbate (DNP); however, as the concentration increased (50-100 mg/L) there was a decrease in enthalpy, i.e. weaker interactions between

When relating the enthalpies as a function of adsorbed amount of DNP can be seen that the enthalpy is directly proportional to the percent of retention, this behavior is due to the main morphological characteristic of the material is its heterogeneity, therefore the heat generated is different because that the adsorbate has occupied the most active sites than the

The differential free energy of adsorption that occurs in the time interval, in which it is carry a calorimetry measure, is determined relating the kinetics of the process to this time interval. Where tinicial is the time in that started the immersion solid-liquid and tfinal is the time in that ended the calorimetric measurement. The free energy difference as a thermodynamic

solution **(Moreno-Piraján et al., 2007)**.

mg/L at 298 K.

effect of char-water interactions.

the adsorbent and the adsorbate.

immediately occupy.

immersion of BBC in DNP solutions of 10 and 30 mg/L.

parameter is the fundamental criterion of spontaneity **(Smiciklas et al., 2008)**, and may be calculated considering the initial concentration (Co) and the concentration in the equilibrium (Ce) to tfinal, by equation (22).

Fig. 11. Enthalpies of immersion of BBC on DNP to different concentration.

$$
\Delta \mathbf{G} \left| \stackrel{\text{ff}}{=} -RT \, \text{Ln} \; \left( \frac{\mathbf{C}\_o}{\mathbf{C}\_e} \right) \right. \tag{22}
$$

Where ∆G (kJ/mol) is differential free energy change; R is universal gas constant, and T (K) is absolute temperature. Reaction occurs spontaneously if G is a negative quantity. From the above equation, the differential change Gibbs free energy for the adsorption process of DNP on BBC to tfinal (293 K) is -113.0 kJ/mol, this negative value indicate that the adsorption of DNP is thermodynamically feasible.

In the specific case of the solution 30 mg/L which has a differential ∆Himm = -56.10 kJ/(g\*mol) and substituting the parameters known in equation (23) determine the differential entropy of the process is equivalent to 580 J/(mol K) this positive value suggests that the organization of the adsorbate in the solid-liquid interface and coincide with value obtained for free energy.

$$
\Delta S \left| \begin{matrix} \frac{\text{ff}}{\text{ff}} = \frac{\Delta H\_{immm} - \Delta G}{T} \end{matrix} \right. \tag{23}
$$

### *Granular activated carbon for adsorption of nickel*

The samples used for nickel removal were obtained from a commercial granular activated carbon made from coconut shell GAC, which was oxidized with GACoxN 6M nitric acid, two parts of this sample were treated one at 723 K and another 1023 K under nitrogen atmosphere, GACoxN723 and GACoxN1023, and a final sample obtained by heating the sample at 1173 K GAC, GAC1173, these samples were characterized by N2 physisorption at -

Thermodynamic of the Interactions Between

**Figueiredo & Pereira. 2010**)

with benzene that is smaller.

Gas-Solid and Solid-Liquid on Carbonaceous Materials 181

On the other hand, we evaluated the changes in surface chemistry of each sample, taking into consideration the important role of surface chemistry on the removal of dissolved metals in aqueous solutions. Table 7 shows the results of the amount of surface groups of each of the samples obtained through Boehm titration. It is observed that the content of acid groups increased by the oxidation treatment, favoring mainly the formation of carboxylic groups, such as reported in other studies (**Gao** *et al***. 2009**). Additionally heat treatment changed the number of groups according to their different thermal stabilities, so, in general it is considered that at low temperatures (about 700 K) and in an inert atmosphere carboxylic groups decompose; in the range of 1000 K lactone groups, carboxylic anhydrides, phenol and ether decomposition is favored; and in higher temperatures up to 1200 K quinone and pyrone groups decompose. On the other hand the values of zero point of charge are consistent with changes in surface chemistry of each sample according to the treatment applied. (**Chingombe** *et al.* **2005; Szymański** *et al***. 2002; Figueiredo** *et al.* **1999;** 

As for the characterization of samples obtained by immersion calorimetry, it is important to note that the enthalpies of immersion allow to evaluate the type of interactions that occur between the solid and the wetting liquid, considering that: if there are no specific interactions between the molecules of the wetting liquid and the solid surface, the immersion enthalpy corresponds to the accessible area of the molecule of the liquid, and if on the contrary, there are specific interactions as in the case of some samples immersed in water, the immersion enthalpy would indicate the hydrophobic or hydrophilic character of

Table 8 shows the results obtained by calculating the enthalpies of immersion in benzene, carbon tetrachloride and water. As for the results using molecules with bipolar moments equal to zero it was observed that: the enthalpies of immersion changed according to changes of surface area as shown in Figure 2 and for the oxidized sample, which has a lower surface area, the enthalpy of immersion is less than for the original sample and even for the heat-treated ones in according to what it was discussed in the analysis of nitrogen adsorption isotherms, the same trend was observed for the enthalpies of immersion in carbon tetrachloride, although values were lower in these enthalpies of immersion, this is basically due to the difference in the size of the molecules of each liquid, which for benzene is 0.37 nm and for carbon tetrachloride is 0.66 nm, in other words, the carbon tetrachloride molecule has diffusion restrictions, therefore the interactions involved correspond only to pores in which the molecule does not have this restrictions, this situation does not occur

the surface of the sample.( **Stoeckli et al. 2001; Szymański et al. 2002**)

**Sample ΔHImmC6H6**

**(J/g)** 

Table 8. Enthalpies of immersion in Benzene, Carbon Tetrachloride and water.

GAC -106.4 -49.65 -75.05 GACoxN -94.98 -66.59 -85.87 GACoxN723 -107.9 -53.32 -50.76 GACoxN1023 -128.8 -37.39 -57.01 GAC1173 -145.1 -32.39 -94.29

**ΔHImmH2O (J/g)** 

**ΔHImm CCl4 (J/g)** 



Table 7. Physical and chemical parameters of samples

Fig. 12. N2 adsorption isotherms at 77 K for different samples

The isotherms of nitrogen obtained for each sample are shown in Figure 1. These are classified as type I adsorption isotherms, where a knee at low relative pressures is evidenced, characteristic of microporous solids in accordance with data obtained after applying the Dubinin-Raduskevich equation. It is important to note that the oxidation process caused a decrease in surface area, this is explained by considering that the oxidation with nitric acid promotes the formation of surface oxygenated groups at the edges of the openings of the pores, these groups are mainly carboxylic and carbonyl (**Dias** *et al.* **2007; Daud & Houshamnd. 2010; Yin** *et al.* **2007)** besides producing the collapse of certain porous structures (**Radovic** *et al***. 2000; Yin** *et al***. 2007; Silvestre-Alvero** *et al.* **2009**), additionally, a surface area increase can be observed even in relation to the sample treated with a higher temperature. This is a result of selective removal of surface groups formed in the oxidation processes, which break down into carbon monoxide and carbon dioxide. In other words, with heat treatment more carbon atoms are lost promoting surface area increase in the solid.

196 ° C and their surface chemistry by Boehm and determining the point of zero charge, in addition, an immersion calorimetry was conducted in different liquids, such as benzene,

> **Lactonic μmol/g**

GAC 842 0.34 72.2 40.5 85.0 198 90.5 5.4 GACoxN 816 0.35 267 52.4 73.7 393 48.6 3.4 GACoxN723 903 0.32 95.3 60.2 112 268 103 7.9 GACoxN1023 935 0.37 2.36 10.2 47.9 60.5 266 8.2 GAC1173 876 0.35 0.00 11.5 34.9 46.4 278 8.9

The isotherms of nitrogen obtained for each sample are shown in Figure 1. These are classified as type I adsorption isotherms, where a knee at low relative pressures is evidenced, characteristic of microporous solids in accordance with data obtained after applying the Dubinin-Raduskevich equation. It is important to note that the oxidation process caused a decrease in surface area, this is explained by considering that the oxidation with nitric acid promotes the formation of surface oxygenated groups at the edges of the openings of the pores, these groups are mainly carboxylic and carbonyl (**Dias** *et al.* **2007; Daud & Houshamnd. 2010; Yin** *et al.* **2007)** besides producing the collapse of certain porous structures (**Radovic** *et al***. 2000; Yin** *et al***. 2007; Silvestre-Alvero** *et al.* **2009**), additionally, a surface area increase can be observed even in relation to the sample treated with a higher temperature. This is a result of selective removal of surface groups formed in the oxidation processes, which break down into carbon monoxide and carbon dioxide. In other words, with heat treatment more carbon atoms are lost promoting surface area increase in the solid.

**Phenolic μmol/g**

**Acidity Total μmol/g** 

**Basicity Total μmol/g** 

**pzc**

carbon tetrachloride and water.

**m2/g** 

**Vo cm3/g**

Table 7. Physical and chemical parameters of samples

Fig. 12. N2 adsorption isotherms at 77 K for different samples

**Carboxilic μmol/g** 

**Sample ÁreaBET**

On the other hand, we evaluated the changes in surface chemistry of each sample, taking into consideration the important role of surface chemistry on the removal of dissolved metals in aqueous solutions. Table 7 shows the results of the amount of surface groups of each of the samples obtained through Boehm titration. It is observed that the content of acid groups increased by the oxidation treatment, favoring mainly the formation of carboxylic groups, such as reported in other studies (**Gao** *et al***. 2009**). Additionally heat treatment changed the number of groups according to their different thermal stabilities, so, in general it is considered that at low temperatures (about 700 K) and in an inert atmosphere carboxylic groups decompose; in the range of 1000 K lactone groups, carboxylic anhydrides, phenol and ether decomposition is favored; and in higher temperatures up to 1200 K quinone and pyrone groups decompose. On the other hand the values of zero point of charge are consistent with changes in surface chemistry of each sample according to the treatment applied. (**Chingombe** *et al.* **2005; Szymański** *et al***. 2002; Figueiredo** *et al.* **1999; Figueiredo & Pereira. 2010**)

As for the characterization of samples obtained by immersion calorimetry, it is important to note that the enthalpies of immersion allow to evaluate the type of interactions that occur between the solid and the wetting liquid, considering that: if there are no specific interactions between the molecules of the wetting liquid and the solid surface, the immersion enthalpy corresponds to the accessible area of the molecule of the liquid, and if on the contrary, there are specific interactions as in the case of some samples immersed in water, the immersion enthalpy would indicate the hydrophobic or hydrophilic character of the surface of the sample.( **Stoeckli et al. 2001; Szymański et al. 2002**)

Table 8 shows the results obtained by calculating the enthalpies of immersion in benzene, carbon tetrachloride and water. As for the results using molecules with bipolar moments equal to zero it was observed that: the enthalpies of immersion changed according to changes of surface area as shown in Figure 2 and for the oxidized sample, which has a lower surface area, the enthalpy of immersion is less than for the original sample and even for the heat-treated ones in according to what it was discussed in the analysis of nitrogen adsorption isotherms, the same trend was observed for the enthalpies of immersion in carbon tetrachloride, although values were lower in these enthalpies of immersion, this is basically due to the difference in the size of the molecules of each liquid, which for benzene is 0.37 nm and for carbon tetrachloride is 0.66 nm, in other words, the carbon tetrachloride molecule has diffusion restrictions, therefore the interactions involved correspond only to pores in which the molecule does not have this restrictions, this situation does not occur with benzene that is smaller.


Table 8. Enthalpies of immersion in Benzene, Carbon Tetrachloride and water.

Thermodynamic of the Interactions Between

**0,0000**

of GAC1173 sample

**0,0000**

of GACoxN1173 sample

**0,0001**

**0,0002**

**E (mV)**

**0,0003**

**0,0004**

**0,0001**

**0,0002**

**0,0003**

**E (mV)**

**0,0004**

**0,0005**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 183

 **Benzene**

 **Water**

 **Carbon Tetrachloride**

**0 200 400 600 800 1000 1200**

Fig. 14. Thermogram of Immersion Calorimetry in Benzene, Carbon Tetrachloride and water

**Time (s)**

 **Benzene Water**

 **Carbon Tetrachloride**

**0 200 400 600 800 1000 1200 1400**

**Time (s)**

Fig. 15. Thermogram of Immersion Calorimetry in Benzene, Carbon Tetrachloride and water

Finally, the samples were used for the removal of nickel from aqueous solution, for this, 0.500 g of each sample were put in contact with 50ml of the nickel solution of concentrations from 100 to 500 mg /L, initial pH of the mixture was adjusted to 6, taking into account that in this pH is nickel is found as Ni (II). The experimental data obtained in the adsorption

process were adjusted to the Redlich-Peterson model and are shown in Figure 16.

Fig. 13. Enthalpies of immersion in Benzene, Carbon Tetrachloride and water in terms of BET area

On the other hand, the difference in the enthalpies of immersion in water of different samples indicates the change in surface chemistry (**Giraldo & Moreno-Piraján. 2008; López-Ramón** *et al.* **2000**), as a result of the different treatments that samples underwent, that is, the development or removal of surface groups on the surface of the solid, thus, a greater amount of oxygenated surface groups as in GACOx's case which leads to a bigger enthalpy of immersion, as a consequence of the interactions established between the polar molecule as is the water molecule and oxygen surface groups developed in the sample, which is consistent with the chemical characterization, these groups were mostly acid type, specifically carboxyl groups. It is also observed that in thermally treated samples decreased enthalpies of immersion in water due to the selective decomposition of the groups present on the surface and therefore a decrease in specific interactions with the water molecule. Additionally, it is possible to conclude that the interactions of water does not occur exclusively with surface groups of the different samples because the sample CAG1173 in which one would expect to have a minimum amount of oxygenated surface groups, also has an calorimetric effect attributed to interactions dispersive type and non- specific type. As for the hydrophobic character of the surface is found that this decrease with the oxidation process and gradually increases with the heat treatments, being higher in the sample treated at 1173 K. Figures 14 and 15 shows the typical thermograms, obtained in the immersion of a solid in the different liquids used. These two figures were chosen because you can see the difference in magnitude of the peaks corresponding to each liquid for to the most oxidized sample (GACoxN) and sample treated to highest temperature in an atmosphere inert (GAC1173).

Fig. 13. Enthalpies of immersion in Benzene, Carbon Tetrachloride and water in

On the other hand, the difference in the enthalpies of immersion in water of different samples indicates the change in surface chemistry (**Giraldo & Moreno-Piraján. 2008; López-Ramón** *et al.* **2000**), as a result of the different treatments that samples underwent, that is, the development or removal of surface groups on the surface of the solid, thus, a greater amount of oxygenated surface groups as in GACOx's case which leads to a bigger enthalpy of immersion, as a consequence of the interactions established between the polar molecule as is the water molecule and oxygen surface groups developed in the sample, which is consistent with the chemical characterization, these groups were mostly acid type, specifically carboxyl groups. It is also observed that in thermally treated samples decreased enthalpies of immersion in water due to the selective decomposition of the groups present on the surface and therefore a decrease in specific interactions with the water molecule. Additionally, it is possible to conclude that the interactions of water does not occur exclusively with surface groups of the different samples because the sample CAG1173 in which one would expect to have a minimum amount of oxygenated surface groups, also has an calorimetric effect attributed to interactions dispersive type and non- specific type. As for the hydrophobic character of the surface is found that this decrease with the oxidation process and gradually increases with the heat treatments, being higher in the sample treated at 1173 K. Figures 14 and 15 shows the typical thermograms, obtained in the immersion of a solid in the different liquids used. These two figures were chosen because you can see the difference in magnitude of the peaks corresponding to each liquid for to the most oxidized sample (GACoxN) and sample treated to highest temperature in an atmosphere inert

terms of BET area

(GAC1173).

Fig. 14. Thermogram of Immersion Calorimetry in Benzene, Carbon Tetrachloride and water of GAC1173 sample

Fig. 15. Thermogram of Immersion Calorimetry in Benzene, Carbon Tetrachloride and water of GACoxN1173 sample

Finally, the samples were used for the removal of nickel from aqueous solution, for this, 0.500 g of each sample were put in contact with 50ml of the nickel solution of concentrations from 100 to 500 mg /L, initial pH of the mixture was adjusted to 6, taking into account that in this pH is nickel is found as Ni (II). The experimental data obtained in the adsorption process were adjusted to the Redlich-Peterson model and are shown in Figure 16.

Thermodynamic of the Interactions Between

environment.

compiled in Table 9.

calorimetry

**2007**)

energy for the samples.

Samples SBET

multilayers. (**Martín-Martínez 1988**)

(m2/g)

Gas-Solid and Solid-Liquid on Carbonaceous Materials 185

processes. (**Nadem et al. 2001**) Another alternative that being studied at present is the production of activated carbon from this waste, there by creating a double benefit for the

A study was conducted about to granular activated carbon adsorbents prepared from tires. To this end, the tires were cut into pieces with a size of 10 mm thick, two samples were treated with phosphoric acid at 20 and 40% p/p (TCP20 and TCP40) and other samples were treated with potassium hydroxide to the same concentrations (TCK20 And TCK40), then underwent to a carbonization process in a horizontal furnace at 1123 K for 2 hours. In this way is prepare by physical activation with CO2, samples were subjected to a pyrolysis process with N2 at 923 K, and then activation with CO2 at two temperatures 1123 K and 1223 K (TCCO2-1123 and TCCO2-1223) during 2 hours. All samples were characterized by N2 adsorption at 77 K and immersion calorimetry in benzene. Some of the results obtain are

> Vo DR (cm3/g)

TCP20 71.17 0.018 13.59 5.670 TCP40 52.85 0.013 13.62 3.120 TCK20 149.2 0.068 19.95 35.55 TCK40 157.3 0.070 19.63 26.17 TCCO2-850 25.44 0.009 14.23 11.48 TCCO2-950 58.12 0.020 14.92 21.36

Table 9. Characteristics of the samples obtained by gas adsorption and immersion

Figure 17 shows the adsorption isotherms for three coals of the series prepared. the TCK40 sample presents a type I isotherm according to IUPAC classification, feature of microporous carbons, the samples and TCCO2-1223 and TCP20 have type II isotherms characteristic of mesoporous carbon, where adsorption occurs in open surface with the formation of

Immersion calorimetry as mentioned along this chapter, allow complement the characterization of porous materials. Figure 18 shows the thermograms obtained for the immersion of the samples in benzene, which is a liquid of wet to assess the area accessible to the molecule. It is observed that the highest enthalpies are obtained for samples prepared with sodium hydroxide which is consistent with the surface areas of these samples. By contrast the samples activated with phosphoric acid have low values compared with those activated with CO2, probably due to the presence of phosphorus compounds in activated carbon, which prevents the access of the benzene molecule. (**Marsh & Rodríguez-Reinoso.** 

From Dubinin Radushkevich equation was calculated pore volume and the characteristic

Eo (KJ/mol) -ΔHimm C6H6 (J/g)

Fig. 16. Adsorption isotherm of Nickel on different samples fit the Redlich-Peterson model.

The importance of the role of oxygenated groups on the activated carbon surface in the adsorption process of ions from aqueous solution has been highlighted by many authors (**Puziy** *et al***. 2002**). It is generally considered that the removal of an ion is mainly attributed to the interaction of surface groups and the ion, through various mechanisms, such as: formation of metal complexes like COOH-M and / or donor-acceptor reactions of electrons (**Petit et al. 2010; Moreno-Castilla** *et al.* **2010**), that is, by establishing specific interactions, therefore, these mechanisms are favored when the solid undergoes an oxidation process as in the case of the sample GACoxN, which has a higher adsorption capacity with respect to other ones, this capacity decreased in heat-treated samples after the process oxidation ratifying the importance of the presence of oxygenated surface groups, although it is important to note that the adsorption capacity of GAC1173 sample is lower, it is also suggested to contemplate within the mechanisms of adsorption interactions that are not only specific but also of the dispersive type, to a lesser extent but to complement the adsorption process.

#### *Activate carbon for the adsorption of phenol*

Among various industrial waste to generate contamination there are tires, this waste is a difficult material to degrade and handle due to its physicochemical composition, generating a problem of global nature. Therefore alternatives different have been proposed for reuse, among these are energy production through incineration, combustion, and pyrolysis

**GACox723 GAC1173 GACox1023**

**GAC GACox**

**0 100 200 300 400 500**

**0**

adsorption process.

*Activate carbon for the adsorption of phenol* 

**10**

**20**

**qe (mg/g)**

**30**

**40**

**Ce (mg/L)**

Fig. 16. Adsorption isotherm of Nickel on different samples fit the Redlich-Peterson model. The importance of the role of oxygenated groups on the activated carbon surface in the adsorption process of ions from aqueous solution has been highlighted by many authors (**Puziy** *et al***. 2002**). It is generally considered that the removal of an ion is mainly attributed to the interaction of surface groups and the ion, through various mechanisms, such as: formation of metal complexes like COOH-M and / or donor-acceptor reactions of electrons (**Petit et al. 2010; Moreno-Castilla** *et al.* **2010**), that is, by establishing specific interactions, therefore, these mechanisms are favored when the solid undergoes an oxidation process as in the case of the sample GACoxN, which has a higher adsorption capacity with respect to other ones, this capacity decreased in heat-treated samples after the process oxidation ratifying the importance of the presence of oxygenated surface groups, although it is important to note that the adsorption capacity of GAC1173 sample is lower, it is also suggested to contemplate within the mechanisms of adsorption interactions that are not only specific but also of the dispersive type, to a lesser extent but to complement the

Among various industrial waste to generate contamination there are tires, this waste is a difficult material to degrade and handle due to its physicochemical composition, generating a problem of global nature. Therefore alternatives different have been proposed for reuse, among these are energy production through incineration, combustion, and pyrolysis processes. (**Nadem et al. 2001**) Another alternative that being studied at present is the production of activated carbon from this waste, there by creating a double benefit for the environment.

A study was conducted about to granular activated carbon adsorbents prepared from tires. To this end, the tires were cut into pieces with a size of 10 mm thick, two samples were treated with phosphoric acid at 20 and 40% p/p (TCP20 and TCP40) and other samples were treated with potassium hydroxide to the same concentrations (TCK20 And TCK40), then underwent to a carbonization process in a horizontal furnace at 1123 K for 2 hours. In this way is prepare by physical activation with CO2, samples were subjected to a pyrolysis process with N2 at 923 K, and then activation with CO2 at two temperatures 1123 K and 1223 K (TCCO2-1123 and TCCO2-1223) during 2 hours. All samples were characterized by N2 adsorption at 77 K and immersion calorimetry in benzene. Some of the results obtain are compiled in Table 9.


Table 9. Characteristics of the samples obtained by gas adsorption and immersion calorimetry

Figure 17 shows the adsorption isotherms for three coals of the series prepared. the TCK40 sample presents a type I isotherm according to IUPAC classification, feature of microporous carbons, the samples and TCCO2-1223 and TCP20 have type II isotherms characteristic of mesoporous carbon, where adsorption occurs in open surface with the formation of multilayers. (**Martín-Martínez 1988**)

Immersion calorimetry as mentioned along this chapter, allow complement the characterization of porous materials. Figure 18 shows the thermograms obtained for the immersion of the samples in benzene, which is a liquid of wet to assess the area accessible to the molecule. It is observed that the highest enthalpies are obtained for samples prepared with sodium hydroxide which is consistent with the surface areas of these samples. By contrast the samples activated with phosphoric acid have low values compared with those activated with CO2, probably due to the presence of phosphorus compounds in activated carbon, which prevents the access of the benzene molecule. (**Marsh & Rodríguez-Reinoso. 2007**)

From Dubinin Radushkevich equation was calculated pore volume and the characteristic energy for the samples.

Thermodynamic of the Interactions Between

**0,5**

energy of adsorption given by the following equation:

77K and β is the affinity coefficient of nitrogen, 0.34.

with benzene **(Silvestre-Albero et al.2004).**

**1,0**

**1,5**

**2,0**

**Ln V**

1123.

**2,5**

**3,0**

**3,5**

**4,0**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 187

Figure 19 shows the graphs of DR for the samples TCK40 and TCK20 where you can see that a deviation from linearity near the saturation pressure, explaining that he has a multilayer adsorption and capillary condensation in mesopores **(Martín-Martínez 1988)** consistent with the isotherms of N2 obtained which present a mesoporosity of activated carbons.

**0 20 40 60 80 100**

Fig. 19. The graphs of DR for the samples. Organized as follows way TCP40-TCK20-TCCO2-

From of the constant D to be the slope of the graph permit to calculate the characteristic

 *<sup>o</sup> RT <sup>E</sup>*

ln ln ln *<sup>o</sup> <sup>o</sup> <sup>P</sup> V VD*

Where R is the gas constant, 80414J/mol, T is the critical temperature of liquide nitrogen,

Stoeckli and Krahenbüehl were the first to correlate the enthalpy of benzene with the microporous parameters, in this work is realized this correlation but for mesoporous carbons. Figure 20 relates the characteristic energy of the nitrogen molecule with the enthalpy of immersion of the benzene molecule. In the activated carbons with carbon dioxide and potassium hydroxide gives a higher characteristic energy to a higher enthalpy of immersion, unlike those activated with phosphoric acid, which has a decrease in enthalpy with increasing energy feature, this behavior shows proportionality existing between the enthalpy of benzene and energy characteristic of N2, despite being two different methods to perform. Samples with higher BET surface area have a higher enthalpy of immersion in benzene which is the expected behavior because it has a greater surface arranged to interact

2

*P* (24)

*D* (25)

**Ln (P/P0)**

 **TCP 40 TCK 20 TCCO2-1123 Linear Regression**

Fig. 17. Isotherms of N2 of the samples TCP20, TCK40 y TCCO2-1223

Fig. 18. Thermograms obtained for the samples.

$$\text{In } V = \ln V\_o - D \left( \ln \frac{P\_o}{P} \right)^2 \tag{24}$$

Where V is the volume adsorbed at certain pressures, P/Po is the partial pressure, Vo is the micropore volume and D is a constant. **Bansal et al. 1988** 

**0 500 1000 1500 2000**

 **TCK 20 TC CO2**

 **TCP 20 TCP 40** **-1223**

*P* (24)

**Time (s)**

ln ln ln *<sup>o</sup> <sup>o</sup> <sup>P</sup> V VD*

Where V is the volume adsorbed at certain pressures, P/Po is the partial pressure, Vo is the

2

Fig. 17. Isotherms of N2 of the samples TCP20, TCK40 y TCCO2-1223

**0,00000**

Fig. 18. Thermograms obtained for the samples.

micropore volume and D is a constant. **Bansal et al. 1988** 

**0,00001**

**0,00002**

**0,00003**

**0,00004**

**E (mV)**

**0,00005**

**0,00006**

**0,00007**

Figure 19 shows the graphs of DR for the samples TCK40 and TCK20 where you can see that a deviation from linearity near the saturation pressure, explaining that he has a multilayer adsorption and capillary condensation in mesopores **(Martín-Martínez 1988)** consistent with the isotherms of N2 obtained which present a mesoporosity of activated carbons.

Fig. 19. The graphs of DR for the samples. Organized as follows way TCP40-TCK20-TCCO2- 1123.

From of the constant D to be the slope of the graph permit to calculate the characteristic energy of adsorption given by the following equation:

$$\ln V = \ln V\_o - D \left( \ln \frac{P\_o}{P} \right)^2 \tag{24}$$

$$E\_o = \frac{RT}{\sqrt{D}\beta} \tag{25}$$

Where R is the gas constant, 80414J/mol, T is the critical temperature of liquide nitrogen, 77K and β is the affinity coefficient of nitrogen, 0.34.

Stoeckli and Krahenbüehl were the first to correlate the enthalpy of benzene with the microporous parameters, in this work is realized this correlation but for mesoporous carbons. Figure 20 relates the characteristic energy of the nitrogen molecule with the enthalpy of immersion of the benzene molecule. In the activated carbons with carbon dioxide and potassium hydroxide gives a higher characteristic energy to a higher enthalpy of immersion, unlike those activated with phosphoric acid, which has a decrease in enthalpy with increasing energy feature, this behavior shows proportionality existing between the enthalpy of benzene and energy characteristic of N2, despite being two different methods to perform. Samples with higher BET surface area have a higher enthalpy of immersion in benzene which is the expected behavior because it has a greater surface arranged to interact with benzene **(Silvestre-Albero et al.2004).**

Thermodynamic of the Interactions Between

**0**

**0**

and low adsorption capacity, with each precursor.

of samples CUD compared with the COD.

**1**

**2**

**n(mmol/g)**

**3**

**4**

 **COD32 COD48 CUD28 CUD48**

**5**

**10**

**n (mmol/g)**

**15**

**20**

**25**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 189

**0,0 0,2 0,4 0,6 0,8 1,0**

 **COD32 COD48 CUD28 CUD36**

**N2**

**CO2**

**P/Po**

**0,00 0,01 0,02 0,03**

**P/Po**

Fig. 21. Nitrogen adsorption isotherms at 77K and CO2 at 273K for the monoliths with high

Some of nitrogen and carbon dioxide isotherms obtained for disks are shown in Figure 22, is evidence the obtaining of microporous solids fact is justified by the form type I isotherms, these solids have a surface area between 975 and 1711 m2g-1 and no between 11.49 and 18.02 mmol, experimental results indicated that the monoliths prepared from African palm stone have higher adsorption capacity and therefore a larger surface area, further shows that the change in the concentration of H3PO4 produces a greater effect on the textural characteristics

Fig. 20. Relación entre la entalpía de inmersión y la energía característica del nitrógeno.

#### *Activated Carbon monoliths for CO2 adsorption*

Taking into account the interest they have taken the activated carbon monoliths in recent years, and its potential use in gas adsorption, is being developed in the research group work which seeks to make a contribution to knowledge of chemistry of solid adsorbents through the preparation, characterization and functionalization of carbon materials granular and monolithic type contribute to the study of the process of adsorption / gas capture a high environmental interest such as carbon dioxide. The CO2 adsorption, has been studied as a way to retain the gas and check for interactions and conditions that govern the process to be more efficient and better use, the problem with CO2 is not simple reason that alternatives are sought treatment with new materials, which will open avenues and possibilities according as knowledge of processes such as adsorption is broader.

As a preliminary approach to the preparation of carbonaceous materials of potential interest in the CO2 adsorption, has been carried out the preparation of activated carbon monoliths disk type take taking advantage of two materials source lignocellulosic s generated as waste in large quantities in Colombia; coconut shell (samples COD) and African palm stone (samples CUD), the endocarps of these precursors are impregnated with H3PO4 solutions at different concentrations for a period of 2 hours at 358K, then take a uniaxial press, where the shaping is done by pressing at 423 K, structures are then carbonized in a horizontal furnace at a linear heating rate of 1 Kmin-1 to a temperature of 723K remaining there 2 hours. Finally, the monoliths obtained are washed with hot distilled water until neutral pH to remove any traces of chemical agent used in the impregnation **(Rodriguez-Reinoso et al., 2004, Vargas et al., 2010)**.

Subsequently, textural, chemical and energy characterization of monoliths is performed to establish their behavior. The adsorption isotherms of N2 at 77K and CO2 at 273 K are determined, the experimental data fit the Langmuir model, and further immersion calorimetry in benzene are performed (0.37 nm) to establish energy correlations.

**4 8 12 16 20**

**Enthalpy (J/g)**

Fig. 20. Relación entre la entalpía de inmersión y la energía característica del nitrógeno.

Taking into account the interest they have taken the activated carbon monoliths in recent years, and its potential use in gas adsorption, is being developed in the research group work which seeks to make a contribution to knowledge of chemistry of solid adsorbents through the preparation, characterization and functionalization of carbon materials granular and monolithic type contribute to the study of the process of adsorption / gas capture a high environmental interest such as carbon dioxide. The CO2 adsorption, has been studied as a way to retain the gas and check for interactions and conditions that govern the process to be more efficient and better use, the problem with CO2 is not simple reason that alternatives are sought treatment with new materials, which will open avenues and possibilities according

As a preliminary approach to the preparation of carbonaceous materials of potential interest in the CO2 adsorption, has been carried out the preparation of activated carbon monoliths disk type take taking advantage of two materials source lignocellulosic s generated as waste in large quantities in Colombia; coconut shell (samples COD) and African palm stone (samples CUD), the endocarps of these precursors are impregnated with H3PO4 solutions at different concentrations for a period of 2 hours at 358K, then take a uniaxial press, where the shaping is done by pressing at 423 K, structures are then carbonized in a horizontal furnace at a linear heating rate of 1 Kmin-1 to a temperature of 723K remaining there 2 hours. Finally, the monoliths obtained are washed with hot distilled water until neutral pH to remove any traces of chemical agent used in the impregnation **(Rodriguez-Reinoso et al., 2004, Vargas** 

Subsequently, textural, chemical and energy characterization of monoliths is performed to establish their behavior. The adsorption isotherms of N2 at 77K and CO2 at 273 K are determined, the experimental data fit the Langmuir model, and further immersion

calorimetry in benzene are performed (0.37 nm) to establish energy correlations.

**12**

*Activated Carbon monoliths for CO2 adsorption* 

as knowledge of processes such as adsorption is broader.

**16**

**20**

**24**

**Eo (kJ/mol)**

**et al., 2010)**.

**28**

**32**

 **TCP TCK TC-CO2**

**36**

Fig. 21. Nitrogen adsorption isotherms at 77K and CO2 at 273K for the monoliths with high and low adsorption capacity, with each precursor.

Some of nitrogen and carbon dioxide isotherms obtained for disks are shown in Figure 22, is evidence the obtaining of microporous solids fact is justified by the form type I isotherms, these solids have a surface area between 975 and 1711 m2g-1 and no between 11.49 and 18.02 mmol, experimental results indicated that the monoliths prepared from African palm stone have higher adsorption capacity and therefore a larger surface area, further shows that the change in the concentration of H3PO4 produces a greater effect on the textural characteristics of samples CUD compared with the COD.

Thermodynamic of the Interactions Between

access to benzene and leads to a decrease in Eo.

the adsorbate is ratified with the increase of enthalpy value.

Fig. 22. Relationship between nm and no samples of each series.

generating a higher Eo.

**3**

**4**

**5**

**n**

**m**

**6**

**7**

**8**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 191

while benzene has a size of 0.37 nm for slit-shape pores and 0.56 nm for cylindrical restricts its accessibility and generates an increase in Eo. In Figure 19a shows that the COD samples show a trend, except COD32 which again leaves the general behavior, this can be attributed to the monolith has a narrow micropores limits the interaction with the benzene molecule,

In the case of samples CUD48 and CUD36 which present a larger surface area, there is a greater more CO2 Eo compared to benzene Eo, in these samples increased the concentration of chemical agent degrades carbonaceous matrix producing a widening pore that provides

Figure 24 relates the characteristic adsorption energy in benzene with the immersion enthalpy in this molecule, can be observed for most samples an increase of the immersion enthalpy with the characteristic energy of the process, which is consistent since the characteristic energy is a measure of the magnitude of the interaction between the solid and

**23456**

**no**

**CUD28**

**COD32**

**COD CUD**

The obtained carbon monoliths were tested as potential adsorbents for CO2 finding a retention capacity between 88-164 mgCO2g-1 at 273K and atmospheric pressure, in Figure 22 to observe the isotherms of the samples with higher and lower CO2 adsorption capacity in each series, the monoliths with a better performance in the retention of this gas were COD32 and CUD28.

The table 10 compiles the characteristics of the carbon monoliths prepared, show the data obtained for the interaction of three molecules of interest in the characterization of materials. Additionally, adsorption data were used for the calculation of three parameters: noDR, nmL, KL which are measures of the adsorption capacity.


Table 10. Characteristics of carbon monoliths.

Figure 22 shows the relationship between the number of moles of the monolayer determined by two different models, nm by the Langmuir model and no calculated from Dubinin Raduskevich, shows that the data are a tendency for both precursors although they are calculated from models with different considerations. There are two points that fall outside the general trend CUD28 and COD32 samples, which despite having the highest value of no in each series not have the highest nm

The Dubinin Raduskevich equation is use to determinate, the characteristic adsorption energies of N2 and CO2 (Eo) for each samples, likewise by the Stoeckli y Krahenbüehl equation (equation 14) was determined benzene (Eo), in Figure 23 shows the relationship between the characteristic energies determined by two different characterization techniques and found two trends in the data which shows the heterogeneity of carbonaceous surfaces of the prepared samples. The characteristic energy of CO2 adsorption, is lower in almost all the monoliths compared to Eo of immersion in benzene, this is consistent considering that due to the size of the CO2 molecule 0.33 nm, this can be accessed easily to narrow pores,

The obtained carbon monoliths were tested as potential adsorbents for CO2 finding a retention capacity between 88-164 mgCO2g-1 at 273K and atmospheric pressure, in Figure 22 to observe the isotherms of the samples with higher and lower CO2 adsorption capacity in each series, the monoliths with a better performance in the retention of this gas were COD32

The table 10 compiles the characteristics of the carbon monoliths prepared, show the data obtained for the interaction of three molecules of interest in the characterization of materials. Additionally, adsorption data were used for the calculation of three parameters: noDR, nmL,

COD28 1270 14.19 4.88 6.95 0.029 16.01 130 20.90

COD32 1320 13.86 5.10 6.64 0.031 16.87 147 24.03

COD36 1318 14.15 4.91 6.56 0.035 16.80 132 21.33

COD48 975 11.49 4.75 4.75 0.055 18.58 112 22.43

CUD28 1013 12.12 4.93 5.36 0.054 19.12 123 21.47

CUD32 1397 13.35 4.38 6.87 0.028 16.76 130 21.12

CUD36 1711 18.02 2.92 4.53 0.027 16.85 120 14.80

CUD48 1706 18.65 2.36 3.99 0.025 17.63 96 11.48

Figure 22 shows the relationship between the number of moles of the monolayer determined by two different models, nm by the Langmuir model and no calculated from Dubinin Raduskevich, shows that the data are a tendency for both precursors although they are calculated from models with different considerations. There are two points that fall outside the general trend CUD28 and COD32 samples, which despite having the highest value of no

The Dubinin Raduskevich equation is use to determinate, the characteristic adsorption energies of N2 and CO2 (Eo) for each samples, likewise by the Stoeckli y Krahenbüehl equation (equation 14) was determined benzene (Eo), in Figure 23 shows the relationship between the characteristic energies determined by two different characterization techniques and found two trends in the data which shows the heterogeneity of carbonaceous surfaces of the prepared samples. The characteristic energy of CO2 adsorption, is lower in almost all the monoliths compared to Eo of immersion in benzene, this is consistent considering that due to the size of the CO2 molecule 0.33 nm, this can be accessed easily to narrow pores,

**(m2/g) no no nm K EO** 

**N2 CO2 C6 H6** 

**(KJ/mol)**

**-ΔHimm (J/g)**

**EO (KJ/mol)**

and CUD28.

**Sample** 

KL which are measures of the adsorption capacity.

Table 10. Characteristics of carbon monoliths.

in each series not have the highest nm

**SBET** 

while benzene has a size of 0.37 nm for slit-shape pores and 0.56 nm for cylindrical restricts its accessibility and generates an increase in Eo. In Figure 19a shows that the COD samples show a trend, except COD32 which again leaves the general behavior, this can be attributed to the monolith has a narrow micropores limits the interaction with the benzene molecule, generating a higher Eo.

In the case of samples CUD48 and CUD36 which present a larger surface area, there is a greater more CO2 Eo compared to benzene Eo, in these samples increased the concentration of chemical agent degrades carbonaceous matrix producing a widening pore that provides access to benzene and leads to a decrease in Eo.

Figure 24 relates the characteristic adsorption energy in benzene with the immersion enthalpy in this molecule, can be observed for most samples an increase of the immersion enthalpy with the characteristic energy of the process, which is consistent since the characteristic energy is a measure of the magnitude of the interaction between the solid and the adsorbate is ratified with the increase of enthalpy value.

Fig. 22. Relationship between nm and no samples of each series.

Thermodynamic of the Interactions Between

**10**

**15**

**Eo Benzene** 

immersion enthalpy.

(**Stoeckli et al., 1989**).

**(kJ/mol)**

**20**

**25**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 193

**100 120 140 160**

**Immersion Enthalpy (J/g)**

Fig. 24. Relationship between the characteristic adsorption energy in benzene and the

Additionally, establishing correlations between energetic parameters determined by different models and textural characteristics, figure 25 a) and b) show the relationship between the characteristic energy and BET area of the COD samples, different behaviors can be observed for each molecule, in the case characteristic adsorption energy of benzene shows a decrease with increasing area of the discs for samples COD28, COD48, but there was an increase in the COD36 and COD32 samples with higher values for surface area. To CUD, as shown in Figure 25 c) and d) in the case of benzene adsorption, for all samples shows a decrease in Eo. The characteristic adsorption energy carbon dioxide molecule shows a decrease with increasing the BET area, for COD32, COD36 there is a slight increase in Eo attributed to these samples have more narrow micropores that can be seen in the value of no CO2. A similar trend shows the CUD discs; the decrease in the characteristic energy with increasing surface area of the monoliths is related to the increased amount of mesopores in the material, since the adsorption energy decreases with increasing pore size

**COD**

 **CUD**

Fig. 23. Relationship between the characteristic immersion energy of benzene and the characteristic adsorption energy of CO2.

**15 16 17 18 19**

**16 17 18 19 20**

**Eo (kJ/mol) Adsorption**

Fig. 23. Relationship between the characteristic immersion energy of benzene and the

**CUD48**

**COD32**

**Eo (kJ/mol) Adsorption**

**22 CUD28**

**COD**

**CUD**

**18**

**10**

characteristic adsorption energy of CO2.

**12**

**14**

**CUD36**

**CUD32**

**16**

**Eo (kJ/mol) Calorimetry**

**18**

**20**

**21**

**24**

**Eo (kJ/mol) Calorimetry**

**27**

Fig. 24. Relationship between the characteristic adsorption energy in benzene and the immersion enthalpy.

Additionally, establishing correlations between energetic parameters determined by different models and textural characteristics, figure 25 a) and b) show the relationship between the characteristic energy and BET area of the COD samples, different behaviors can be observed for each molecule, in the case characteristic adsorption energy of benzene shows a decrease with increasing area of the discs for samples COD28, COD48, but there was an increase in the COD36 and COD32 samples with higher values for surface area. To CUD, as shown in Figure 25 c) and d) in the case of benzene adsorption, for all samples shows a decrease in Eo. The characteristic adsorption energy carbon dioxide molecule shows a decrease with increasing the BET area, for COD32, COD36 there is a slight increase in Eo attributed to these samples have more narrow micropores that can be seen in the value of no CO2. A similar trend shows the CUD discs; the decrease in the characteristic energy with increasing surface area of the monoliths is related to the increased amount of mesopores in the material, since the adsorption energy decreases with increasing pore size (**Stoeckli et al., 1989**).

Thermodynamic of the Interactions Between

**10**

**16**

**17**

**18**

**Eo (kJ/mol)**

c,d) CUD.

**19**

**20**

**15**

**Eo (KJ/mmol)**

**20**

**25**

Gas-Solid and Solid-Liquid on Carbonaceous Materials 195

**C6H6**

**CO2**

**900 1200 1500 1800**

**BET Area (m2/g)**

c)

**800 1200 1600**

d) Fig. 25. Relationship between the characteristic energy and BET area of the series. a,b) COD.

**BET Area (m2**/**g)**

a)

**900 1000 1100 1200 1300 1400**

**BET Area (m2/g)**

**900 1000 1100 1200 1300 1400**

**BET Area (m2/g)**

b)

a)

**C6H6**

**CO2**

**20**

**15**

**16**

**17**

**Eo (kJ/mmol)**

**18**

**19**

**22**

**Eo (kJ/mol)**

**24**

**26**

d)

Fig. 25. Relationship between the characteristic energy and BET area of the series. a,b) COD. c,d) CUD.

Thermodynamic of the Interactions Between

No. 1, pp. 7-16.

Gas-Solid and Solid-Liquid on Carbonaceous Materials 197

Garcia-Cuello, V., Moreno-Piraján, J. C., Giraldo-Gutiérrez, L., Sapag, K., Zgrablich, G.

Giraldo, L., García-Cuello, V., Moreno-Piraján, J. C. (2008). Caracterización superficial en

Giraldo, L., Moreno, J.C. (2008) Pb(II) and Cr(VI) adsorption from aqueous solution on

Hemminger, W. & Höhne, G. (1984). Calorimetry: Fundamentals and Practice, Verlag

Jiménez, O. (2000). Preparación de carbón activado a partir de distintos tipos de material

Kraus, G. (1955). The heat of immersion of carbon black in water, methanol and n-hexane. *J.* 

Llewellyn, P. L. & Maurin, G. (2005). Gas adsorption microcalorimetry and modelling to characterize zeolites and related materials, *C. R. Chim.*, Vol. 8 No. 1, pp. 283–302. López-Ramón, M.V., Stoeckli, F., Moreno-Castilla, C., Carrasco-Marín, F. (2000) Specific and

Marsh, H., Rodriguez-Reinoso, F.( 2007) Encyclopedia of Materials: Science and Technology.

Marsh, Harry., Rodriguez-Reinoso, Francisco. (2006). Activated Carbon (Origins). En:

Martin Matinez, J.M. (1988). Adsorción física de gases y vapores por carbones . Universidad

Menéndez, J. A. (1998). On the use of calorimetric techniques for the characterization of carbons: A brief review. *Thermochim. Acta*, Vol. 312, No. 1, pp. 79 – 86. Molina-Sabio, M., Nakagawa, Y., Rodríguez-Reinoso, F. (2008). Possible errors in

Montes-Morán, M.A., Suárez, D., Menéndez, J.A., Fuente, E.(2004) On the nature of basic sites on carbon surfaces: an overview. *Carbon*. Vol. 42*, No. 7*, pp.1219*-1225.*  Moreno, J. C. & Giraldo, L. (2005). Setups for simultaneous measurement of isotherms and

Moreno, J. C. (1996). Microcalorímetro de conducción de calor: diseño, construcción,

Moreno, J.C., Gómez, R., Giraldo, L. (2010). Removal of Mn, Fe, Ni and Cu Ions from Wastewater Using Cow Bone Charcoal, *Materials*, Vol. 3, pp. 452-466.

Activated carbon, Elsevier Science Ltd ISBN: 0080444636, pp. 13-81.

enthalpies. *Micropor. Mesopor. Mat*. Vol. 120 No. 1, pp. 239–245.

*and Applied Pyrolysis*, Vol. 81, No. 2, pp 278-284.

Nacional de Colombia. Bogotá, Colombia.

calorimetry. *Carbon*. Vol. 38*, No. 6*, pp.825*-829.* 

Universidad de Alicante. Alicante, España.

calorimetry. *Carbon,* Vol. 46, No. 1, pp. 329-334.

adsorption heats. *Rev. Sci. Instrum.* Vol. 76, No. 1, pp. 1-8.

Universidad Nacional de Colombia, Bogotá,Colombia.

*phys. Chem*. Vol. 59, No. 4, pp. 343-345.

Activated Carbon. 542 p.

Chemie, ISBN 2-87352-027-2, Florida, United States.

(2009). A new microcalorimeter of adsorption for the determination of differential

fase gas y líquida de carbones activados. *Rev.Ing.Universidad de los Andes*, Vol. 27,

activated carbons obtained from sugar cane husk and sawdust. *Journal of Analytical* 

vegetal colombiano de desechos con posible aplicación en la remoción de fenol en agua residuales, Trabajo de Grado. Departamento de Química. Universidad

non-specific interactions of water molecules with carbon surfaces from immersion

de Alicante. 465 p. ISBN: 84-86809-33-9. Edita: Secretariado de Publicaciones de la

microporosity in chemically activated carbon deduced from immersion

calibración y su aplicación al estudio de sólidos porosos. Tesis doctoral,
