# Comparative Study of Textural Characteristics on Methane Adsorption for Carbon Spheres Produced by CO2 Activation

Authors: Wen Yang; Yanyan Feng; Wei Chu
Journal: International Journal of Chemical Engineering
 (2014)

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## Abstract

Resorcinol-formaldehyde resin polymer was used as raw material for preparation of carbon spheres. Samples were treated with CO2 flow at 850°C by varying activation times. The CO2 activation granted better pore development of pore structure. The experimental data of CH4 adsorption as a function of equilibrium pressure was fitted by Langmuir and Dubinin-Astakhov (D-A) models. It was concluded that the high surface area and micropore volume of carbon spheres did unequivocally determine methane capacities. In addition, a thermodynamic study of the heat of adsorption of CH4 on the carbon spheres was carried out. Adsorption of CH4 on carbon spheres showed a decrease in the adsorption heat with CH4 occupancy, and the heat of adsorption fell from 20.51 to 12.50 kJ/mol at 298 K and then increased to a little higher values at a very high loading (>0.70), indicating that CH4/CH4 interactions within the adsorption layer became significant.


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## Body

## 1. Introduction

Energy sources as an alternative to conventional fuels are required for a sustainable energy supply and progressively more strict environmental rules [1, 2]. With this background, coalbed methane (CBM) [2–6], mainly CH4 with the low level of CO2 and other hydrocarbon gases, is becoming an increasingly important energy resource; that is, CH4 can be considered as a new energy resource [3, 7].However, as one of the most important greenhouse gases, the efficient storage of CH4 is necessary [8–12]. Up to now, many studies have been carried out on the storage of large amounts of CH4 [12]. Compared with liquefaction and compression for storing CH4, adsorption in porous materials has the advantage at relatively low pressure and ambient temperature and is vital to numerous engineering processes and industrial applications [8]. Carbonaceous materials are particularly attractive as the adsorbent because they are lightweight, abundantly available, and simple to produce and can effectively increase the amounts of stored gases [13–17]. The fabrication and tuning of carbonaceous materials such as activated carbons (ACs) and carbon nanotubes [18–20] are important research areas with respect to achieving storage of high amounts of CH4 [21–25].AC is one of the most excellent carbonaceous materials widely developed for various industries [9, 10, 26–32]. As a sort of well-developed porous solid, the nature of the microstructure of AC has been reported to have an effect on their adsorptive capacities for CH4 [1, 33–35]. In addition, the pore structure offers the potential to adjust the thermodynamic properties of adsorption. Herein, an effective approach for investigating the methane adsorption capacity and tuning the thermodynamics of adsorption is by controlling the pore structure [2, 10, 36, 37]. However, the pore structure of ACs is highly dependent on the activation process, among which thermal or physical activation of ACs has been widely used. One-step activation with CO2 has been used to prepare ACs at laboratory scale and carbon atoms are extracted from the structure of the porous carbon according to the following endothermic reactions:
(1)C+CO2⟶2CO
resulting in the well-developed microporosities of the prepared ACs [36].Hence, in the present study, we investigated the effect of the textural characteristics of carbon spheres on their CH4 adsorption capacities. Sample, with resorcinol-formaldehyde resin polymer used as the raw material, was treated with CO2 flow at 850°C by varying activation time to achieve different pore structures. The texture was determined by N2 adsorption/desorption at 77 K, scanning electron microscopy (SEM), and Raman spectroscopy. Detailed analyses of the texture allowed the investigation of pore structures in which the adsorption behaviors took place. The data of CH4 adsorption equilibrium were measured by a volumetric method at pressures up to ~5 MPa and temperature 298 K which was relevant to gas storage under geological conditions and continually fitted to the Langmuir and Dubinin-Astakhov (D-A) equations, respectively. Furthermore, the results of CH4 adsorption were discussed with regard to the textural characteristics, such as the pore structure and degree of graphitization. In addition, a thermodynamic study of the heat of adsorption of CH4 on the carbon spheres was also carried out.


## 2. Experimental

### 2.1. Sample Preparation

The RF resins spheres were typically synthesized by using resorcinol and formaldehyde solution as precursors, similarly described in the previous literature [38]. At first, 6 mL of the ammonia aqueous solution (NH4OH, 25 wt%) was mixed with a solution containing absolute ethanol (EtOH, 480 mL) and deionized water (1200 mL) and stirred for more than 1 h. Subsequently, resorcinol (12 g) was added, followed by adding 16.8 mL of the formaldehyde solution and continually stirring for 24 h with the speed of 300 r/min at 30°C, and then kept at 100°C for 24 h in a Teflon-lined autoclave. The solid product was obtained by centrifugation and air-dried at 100°C for 24 h. Lastly, the RF resin spheres were heated to 700°C under Ar atmosphere with a heating rate of 2°C/min and then maintained at 700°C for 2 h (named as CS0) for carbonization.After carbonization, the resulting products were taken out and used for CO2 activation. The products were heated up to 850°C with a heating rate of 2°C/min, and CO2 stream with a flow rate of 100 mL/min was used for 3~9 h to obtain carbon spheres with different pore structures (denoted by CS3, CS6, and CS9, resp.) [36].


### 2.2. Characterization

The textural characterization of the four samples was obtained by N2 adsorption/desorption isotherms, determined at 77 K with a NOVA1000e surface area and pore size analyzer (Quantachrome Company). The specific surface areas were determined according to the BET method. Total pore volume was directly calculated from the volume of nitrogen held at p/p0 = 0.98~0.99; the volume of micropore and pore size distributions (PSDs) were estimated using the D-A equation [2, 3].Surface morphology was investigated by scanning electron microscopy (SEM) (Hitachi S-4800, Japan) [39].The Raman spectroscopy of the samples was measured with a Raman microspectrometer (Renishaw SystemInVia) using an argon laser as the excitation (λ=514.5 nm). The spectra were recorded in the wave number range of 400~4000 cm−1 [40, 41], and the intensities of D and G bands were measured using a Lorentzian curve-fitting procedure [25, 42].


### 2.3. Methane Adsorption

Methane adsorption measurements were conducted using a volumetric method similar to that previously described [2–4]. The experimental devices were placed in a temperature-controlled oven to ensure the constant temperature throughout the adsorption process. The purities of helium and methane were 99.999% and 99.99%, respectively. Before the measurement, the sample was degassed for about 3 h. After degassing, helium expansion was performed for the calibration of the void volume in the adsorption setup. Subsequently, methane adsorption was measured at 298 K under the pressure range 0~5.0 MPa.


## 2.1. Sample Preparation

The RF resins spheres were typically synthesized by using resorcinol and formaldehyde solution as precursors, similarly described in the previous literature [38]. At first, 6 mL of the ammonia aqueous solution (NH4OH, 25 wt%) was mixed with a solution containing absolute ethanol (EtOH, 480 mL) and deionized water (1200 mL) and stirred for more than 1 h. Subsequently, resorcinol (12 g) was added, followed by adding 16.8 mL of the formaldehyde solution and continually stirring for 24 h with the speed of 300 r/min at 30°C, and then kept at 100°C for 24 h in a Teflon-lined autoclave. The solid product was obtained by centrifugation and air-dried at 100°C for 24 h. Lastly, the RF resin spheres were heated to 700°C under Ar atmosphere with a heating rate of 2°C/min and then maintained at 700°C for 2 h (named as CS0) for carbonization.After carbonization, the resulting products were taken out and used for CO2 activation. The products were heated up to 850°C with a heating rate of 2°C/min, and CO2 stream with a flow rate of 100 mL/min was used for 3~9 h to obtain carbon spheres with different pore structures (denoted by CS3, CS6, and CS9, resp.) [36].


## 2.2. Characterization

The textural characterization of the four samples was obtained by N2 adsorption/desorption isotherms, determined at 77 K with a NOVA1000e surface area and pore size analyzer (Quantachrome Company). The specific surface areas were determined according to the BET method. Total pore volume was directly calculated from the volume of nitrogen held at p/p0 = 0.98~0.99; the volume of micropore and pore size distributions (PSDs) were estimated using the D-A equation [2, 3].Surface morphology was investigated by scanning electron microscopy (SEM) (Hitachi S-4800, Japan) [39].The Raman spectroscopy of the samples was measured with a Raman microspectrometer (Renishaw SystemInVia) using an argon laser as the excitation (λ=514.5 nm). The spectra were recorded in the wave number range of 400~4000 cm−1 [40, 41], and the intensities of D and G bands were measured using a Lorentzian curve-fitting procedure [25, 42].


## 2.3. Methane Adsorption

Methane adsorption measurements were conducted using a volumetric method similar to that previously described [2–4]. The experimental devices were placed in a temperature-controlled oven to ensure the constant temperature throughout the adsorption process. The purities of helium and methane were 99.999% and 99.99%, respectively. Before the measurement, the sample was degassed for about 3 h. After degassing, helium expansion was performed for the calibration of the void volume in the adsorption setup. Subsequently, methane adsorption was measured at 298 K under the pressure range 0~5.0 MPa.


## 3. Results and Discussion

### 3.1. Textural and Structural Characteristics

The weight loss (burn-off) as a function of residence time of activated carbon spheres was plotted in Figure1. With the activation time increasing, the burn-off became much higher. As the burn-off increased, the elementary crystallites and defects became exposed to the activating agent CO2 for further development of porosity [43–45].Figure 1
Evolution of burn-off versus activation time for carbon spheres treated in CO2.The N2 adsorption-desorption isotherms, pore size distribution (PSD), and textural characteristics of the pristine sample and the corresponding CO2 activated samples were presented in Figures 2 and 3 and Table 1, respectively. As shown in Figure 2, the samples of CS3, CS6, and CS9 presented largely similar adsorption-desorption isotherms between types I and IV, indicating that not only micropores but also mesopores were developed in these porous samples. For the activated carbon spheres, the increase in the activation time provoked a progressive increase in N2 adsorption capacity. For the maximum activation time of 9 h, a BET surface area of 1145.0 m2/g and a D-A micropore volume of 0.639 cm3/g were reached. It was clear to see that the prepared samples had similar PSDs determined from the isotherms with similar shapes.Table 1
Structural characteristics of the studied samples.
Sample
Specific surface area (BET, m2/g)
Micropore volume(D-A, cm3/g)
Total pore volume (cm3/g)
V
micro/Vtotal (%)
Average pore diameter (nm)
CS0
422.7
0.219
0.238
92.02
2.254
CS3
658.4
0.336
0.428
78.50
2.602
CS6
881.7
0.461
0.557
82.76
2.529
CS9
1145.0
0.639
0.732
87.30
2.556Figure 2
N2 adsorption-desorption isotherms (77 K) corresponding to the four samples. □: CS0; ○: CS3; △: CS6; and ▽: CS9.Figure 3
Pore size distributions obtained applying the D-A equation to the N2 adsorption-desorption data. □: CS0; ○: CS3; △: CS6; and ▽: CS9.The specific surface area and micropore volume of the prepared carbon spheres were summarized in Table1. The fraction of microporosity depended heavily on the degree of activation to which the pristine carbon spheres were subjected. We observed that this parameter has an important role in determining the textural characteristics of the porous samples. It could be seen that the pore structure of the prepared samples strongly relied on the activation time. As displayed in Table 1, the carbon spheres activated at 9 h possessed higher surface area, larger than 1100 m2/g, while the samples activated at shorter times had a much lower surface area, especially for the pristine sample CS0. Maximum surface area was obtained for the sample of CS9 (1145.0 m2/g), which may be because most of CO2 could efficiently diffuse onto and act with the carbons on the particle surface of the samples during the activation process, resulting in the well-developed microporosity. Moreover, the longer the sample is activated, the more the burn-off is, thus affecting the pore structure of the treated sample and leading to the higher pore volume.More interestingly, the porosity of these carbon spheres was made up of pores in the micropore-mesopore range (sizes between 0.8 nm and 3 nm) as evidenced by the PSDs shown in Figure3. At high activation times, a development of some micropores and the widening of PSDs continued, resulting in the development of wider micropores and a right shift of the maximum peak to mesopores. In summary, the CO2 activation process carried out promoted the N2 adsorption capacity (Figure 2) together with a modest widening of the PSDs (Figure 3).To further investigate the effect of activation time on the porous carbon spheres, SEM observation was employed to obtain the morphology of the resulting samples. As shown in Figure4, the pristine carbon spheres exhibited a sphere-like morphology, and the primary particle size was about 400~500 nm. It could be seen that, in spite of the activation time, the samples of CS3, CS6, and CS9 presented no apparent differences in morphology. Comparatively, the CS9 carbon displayed a much rougher surface with more defects on the particle surface due to the accelerated activation process at high activation time, suggesting that a drastic surface morphological change has occurred during the activation process.SEM images of the prepared samples. (a) CS0, (b) CS3, (c) CS6, and (d) CS9.
(a)
(b)
(c)
(d)The Raman spectra of the four samples, shown in Figure5, presented a prominent G-band (graphite) at 1580 cm−1 and a less-intense D-band (defects) at 1350 cm−1 in the first-order region. The second-order Raman spectrum showed the G′ band which is characteristic of tridimensional ordered materials. The D-band and G-band strengths were suggested to be proportional to the likely of a 6-fold aromatic ring in the sample [6], and ID/IG was chosen to represent the evolution of the microstructure of the carbon spheres during the activation process. Figure 5 showed almost a linear correlation between activation time and defects. When subjected to high activation time, it was enough for the growth of disordered structure and was tending to a worse orientation of the sample. With the increase of activation time, the D-band intensity of the samples went higher, and the intensity of G-band changed little. The D-band presented more intensely, suggesting more defects, and an increasing amount of disordered structure of the sample occurred. As a result, compared with the pristine carbon spheres without activation treatment, the CO2 activated samples became more disordered. The increase in the specific surface area, PSDs, the average pore diameter, and the results of SEM also reflected the structure disordering with an increasing activation time.Figure 5
Raman spectra for the samples prepared by CO2 activation.


### 3.2. Methane Adsorption Performance

The methane adsorption isotherms of the carbon spheres at 298 K and pressures up to 5.0 MPa were presented in Figures6 and 7, respectively. The methane adsorption isotherms were Type I of IUPAC, and the capacity of methane adsorbed increased with the increase in activation time. The adsorption isotherms were then analyzed by two models, that is, Langmuir (dotted lines in Figure 6) and D-A models (dotted lines in Figure 7). It can be seen that both models fitted the data well, and the adsorption parameters of the two models were given in Table 2.Table 2
Adsorption parameters of the Langmuir model and D-A model of methane adsorption at 298 K.
Sample
Langmuir model
D-A model
n
0 (mg/g)
b (MPa−1)
W
0 (mg/g)
E (KJ/mol)
t
CS0
49.31
0.775
44.87
7.112
1.714
CS3
70.78
0.653
64.41
6.648
1.598
CS6
102.47
0.447
81.71
6.205
1.724
CS9
115.55
0.611
90.27
6.898
2.325Figure 6
Equilibrium isotherms of methane adsorption on carbon spheres at 298 K. □: CS0; ○: CS3; △: CS6;▽: CS9; and dotted line: Langmuir model.Figure 7
Equilibrium isotherms of methane adsorption on carbon spheres at 298 K. □: CS0; ○: CS3; △: CS6;▽: CS9; and dotted line: D-A model.The parameters obtained from Langmuir model have been widely used in evaluating the methane adsorption capacities.n0 represents the Langmuir maximum adsorption capacity and Langmuir constant b is the reciprocal of the pressure when the adsorption capacity reaches 50% of the maximum adsorption capacity. The parameter t in D-A model describes the surface heterogeneity. It has been reported that the surface of the adsorbent is less heterogeneous when the t value is approaching 3 more (t<3). The parameter E in D-A model is the characteristic energy describing the strength of interaction between adsorbate and adsorbent [2, 4]. Comparing with the D-A model, Langmuir model displayed a higher value of maximum adsorption capacity for the samples.It is well known that the methane adsorption is a physical adsorption, which is mainly dependent on the micropore volume and surface area. The greatest adsorption capacity (115.55 mg/g, Langmuir model) was obtained for the CS9 sample due to its higher surface area and abundant micropores. The carbon spheres of CS3 and CS6 exhibited much higher adsorption capacity (70.78 and 102.47 mg/g, resp., Langmuir model) than the pristine sample which exhibited the smallest adsorption capacity (49.31 mg/g, Langmuir model) among all the prepared carbon spheres.To determine the strength of the interaction between methane and the prepared samples, the heat of adsorption,Hads, was evaluated based on the Clausius-Clapeyron equation using the methane adsorption isotherms, and these were plotted in Figure 8 against the surface loading W/W0. Invoking the D-A model in Clausius-Clapeyron equation, an explicit expression for Hads can be written as below [37] for T>Tcri:
(2)Hads=2RT+E[(ln⁡W0Cυa)1/t+αTt(ln⁡W0Cυa)1-t/t].Figure 8
Heat of adsorption(Hads) for methane/carbon spheres pair against different surface loading (W/W0) at 298 K. ■: CS0; □: CS3; ●: CS6; and ○: CS9.As shown in Figure8, the Hads varied largely with the surface loading W/W0 for all the samples. Before the W/W0 approached about 0.70, the value of the Hads over the carbon spheres all decreased with the increase in the W/W0. This variation of the Hads with the surface loading was due to the surface heterogeneity of the carbon spheres and the stronger interaction between carbon materials and methane. However, the plots of the CS0, CS6, and CS9 then increased to a little higher value at very high loading (>0.70), indicating that the interaction between the carbon spheres and methane was weaker and methane/methane interactions within the adsorption layer became obvious. For methane adsorption, the average heat of adsorption is typically 12~20 kJ/mol, consistent with the result of our study that the Hads fell from 20.51 to 12.50 kJ/mol with methane occupancy at 298 K. It could be further seen that the Hads of the prepared carbon spheres dropped with the increase in activation time, which may be due to the decrease in interaction between methane and carbon materials. The high Hads value indicated that the prepared sample strongly interacted with methane molecules [2, 37].


## 3.1. Textural and Structural Characteristics

The weight loss (burn-off) as a function of residence time of activated carbon spheres was plotted in Figure1. With the activation time increasing, the burn-off became much higher. As the burn-off increased, the elementary crystallites and defects became exposed to the activating agent CO2 for further development of porosity [43–45].Figure 1
Evolution of burn-off versus activation time for carbon spheres treated in CO2.The N2 adsorption-desorption isotherms, pore size distribution (PSD), and textural characteristics of the pristine sample and the corresponding CO2 activated samples were presented in Figures 2 and 3 and Table 1, respectively. As shown in Figure 2, the samples of CS3, CS6, and CS9 presented largely similar adsorption-desorption isotherms between types I and IV, indicating that not only micropores but also mesopores were developed in these porous samples. For the activated carbon spheres, the increase in the activation time provoked a progressive increase in N2 adsorption capacity. For the maximum activation time of 9 h, a BET surface area of 1145.0 m2/g and a D-A micropore volume of 0.639 cm3/g were reached. It was clear to see that the prepared samples had similar PSDs determined from the isotherms with similar shapes.Table 1
Structural characteristics of the studied samples.
Sample
Specific surface area (BET, m2/g)
Micropore volume(D-A, cm3/g)
Total pore volume (cm3/g)
V
micro/Vtotal (%)
Average pore diameter (nm)
CS0
422.7
0.219
0.238
92.02
2.254
CS3
658.4
0.336
0.428
78.50
2.602
CS6
881.7
0.461
0.557
82.76
2.529
CS9
1145.0
0.639
0.732
87.30
2.556Figure 2
N2 adsorption-desorption isotherms (77 K) corresponding to the four samples. □: CS0; ○: CS3; △: CS6; and ▽: CS9.Figure 3
Pore size distributions obtained applying the D-A equation to the N2 adsorption-desorption data. □: CS0; ○: CS3; △: CS6; and ▽: CS9.The specific surface area and micropore volume of the prepared carbon spheres were summarized in Table1. The fraction of microporosity depended heavily on the degree of activation to which the pristine carbon spheres were subjected. We observed that this parameter has an important role in determining the textural characteristics of the porous samples. It could be seen that the pore structure of the prepared samples strongly relied on the activation time. As displayed in Table 1, the carbon spheres activated at 9 h possessed higher surface area, larger than 1100 m2/g, while the samples activated at shorter times had a much lower surface area, especially for the pristine sample CS0. Maximum surface area was obtained for the sample of CS9 (1145.0 m2/g), which may be because most of CO2 could efficiently diffuse onto and act with the carbons on the particle surface of the samples during the activation process, resulting in the well-developed microporosity. Moreover, the longer the sample is activated, the more the burn-off is, thus affecting the pore structure of the treated sample and leading to the higher pore volume.More interestingly, the porosity of these carbon spheres was made up of pores in the micropore-mesopore range (sizes between 0.8 nm and 3 nm) as evidenced by the PSDs shown in Figure3. At high activation times, a development of some micropores and the widening of PSDs continued, resulting in the development of wider micropores and a right shift of the maximum peak to mesopores. In summary, the CO2 activation process carried out promoted the N2 adsorption capacity (Figure 2) together with a modest widening of the PSDs (Figure 3).To further investigate the effect of activation time on the porous carbon spheres, SEM observation was employed to obtain the morphology of the resulting samples. As shown in Figure4, the pristine carbon spheres exhibited a sphere-like morphology, and the primary particle size was about 400~500 nm. It could be seen that, in spite of the activation time, the samples of CS3, CS6, and CS9 presented no apparent differences in morphology. Comparatively, the CS9 carbon displayed a much rougher surface with more defects on the particle surface due to the accelerated activation process at high activation time, suggesting that a drastic surface morphological change has occurred during the activation process.SEM images of the prepared samples. (a) CS0, (b) CS3, (c) CS6, and (d) CS9.
(a)
(b)
(c)
(d)The Raman spectra of the four samples, shown in Figure5, presented a prominent G-band (graphite) at 1580 cm−1 and a less-intense D-band (defects) at 1350 cm−1 in the first-order region. The second-order Raman spectrum showed the G′ band which is characteristic of tridimensional ordered materials. The D-band and G-band strengths were suggested to be proportional to the likely of a 6-fold aromatic ring in the sample [6], and ID/IG was chosen to represent the evolution of the microstructure of the carbon spheres during the activation process. Figure 5 showed almost a linear correlation between activation time and defects. When subjected to high activation time, it was enough for the growth of disordered structure and was tending to a worse orientation of the sample. With the increase of activation time, the D-band intensity of the samples went higher, and the intensity of G-band changed little. The D-band presented more intensely, suggesting more defects, and an increasing amount of disordered structure of the sample occurred. As a result, compared with the pristine carbon spheres without activation treatment, the CO2 activated samples became more disordered. The increase in the specific surface area, PSDs, the average pore diameter, and the results of SEM also reflected the structure disordering with an increasing activation time.Figure 5
Raman spectra for the samples prepared by CO2 activation.


## 3.2. Methane Adsorption Performance

The methane adsorption isotherms of the carbon spheres at 298 K and pressures up to 5.0 MPa were presented in Figures6 and 7, respectively. The methane adsorption isotherms were Type I of IUPAC, and the capacity of methane adsorbed increased with the increase in activation time. The adsorption isotherms were then analyzed by two models, that is, Langmuir (dotted lines in Figure 6) and D-A models (dotted lines in Figure 7). It can be seen that both models fitted the data well, and the adsorption parameters of the two models were given in Table 2.Table 2
Adsorption parameters of the Langmuir model and D-A model of methane adsorption at 298 K.
Sample
Langmuir model
D-A model
n
0 (mg/g)
b (MPa−1)
W
0 (mg/g)
E (KJ/mol)
t
CS0
49.31
0.775
44.87
7.112
1.714
CS3
70.78
0.653
64.41
6.648
1.598
CS6
102.47
0.447
81.71
6.205
1.724
CS9
115.55
0.611
90.27
6.898
2.325Figure 6
Equilibrium isotherms of methane adsorption on carbon spheres at 298 K. □: CS0; ○: CS3; △: CS6;▽: CS9; and dotted line: Langmuir model.Figure 7
Equilibrium isotherms of methane adsorption on carbon spheres at 298 K. □: CS0; ○: CS3; △: CS6;▽: CS9; and dotted line: D-A model.The parameters obtained from Langmuir model have been widely used in evaluating the methane adsorption capacities.n0 represents the Langmuir maximum adsorption capacity and Langmuir constant b is the reciprocal of the pressure when the adsorption capacity reaches 50% of the maximum adsorption capacity. The parameter t in D-A model describes the surface heterogeneity. It has been reported that the surface of the adsorbent is less heterogeneous when the t value is approaching 3 more (t<3). The parameter E in D-A model is the characteristic energy describing the strength of interaction between adsorbate and adsorbent [2, 4]. Comparing with the D-A model, Langmuir model displayed a higher value of maximum adsorption capacity for the samples.It is well known that the methane adsorption is a physical adsorption, which is mainly dependent on the micropore volume and surface area. The greatest adsorption capacity (115.55 mg/g, Langmuir model) was obtained for the CS9 sample due to its higher surface area and abundant micropores. The carbon spheres of CS3 and CS6 exhibited much higher adsorption capacity (70.78 and 102.47 mg/g, resp., Langmuir model) than the pristine sample which exhibited the smallest adsorption capacity (49.31 mg/g, Langmuir model) among all the prepared carbon spheres.To determine the strength of the interaction between methane and the prepared samples, the heat of adsorption,Hads, was evaluated based on the Clausius-Clapeyron equation using the methane adsorption isotherms, and these were plotted in Figure 8 against the surface loading W/W0. Invoking the D-A model in Clausius-Clapeyron equation, an explicit expression for Hads can be written as below [37] for T>Tcri:
(2)Hads=2RT+E[(ln⁡W0Cυa)1/t+αTt(ln⁡W0Cυa)1-t/t].Figure 8
Heat of adsorption(Hads) for methane/carbon spheres pair against different surface loading (W/W0) at 298 K. ■: CS0; □: CS3; ●: CS6; and ○: CS9.As shown in Figure8, the Hads varied largely with the surface loading W/W0 for all the samples. Before the W/W0 approached about 0.70, the value of the Hads over the carbon spheres all decreased with the increase in the W/W0. This variation of the Hads with the surface loading was due to the surface heterogeneity of the carbon spheres and the stronger interaction between carbon materials and methane. However, the plots of the CS0, CS6, and CS9 then increased to a little higher value at very high loading (>0.70), indicating that the interaction between the carbon spheres and methane was weaker and methane/methane interactions within the adsorption layer became obvious. For methane adsorption, the average heat of adsorption is typically 12~20 kJ/mol, consistent with the result of our study that the Hads fell from 20.51 to 12.50 kJ/mol with methane occupancy at 298 K. It could be further seen that the Hads of the prepared carbon spheres dropped with the increase in activation time, which may be due to the decrease in interaction between methane and carbon materials. The high Hads value indicated that the prepared sample strongly interacted with methane molecules [2, 37].


## 4. Conclusion

In this paper, the textural characteristics of the carbon spheres were related to their methane adsorption capacities. Resorcinol-formaldehyde resin polymer was used as the raw material for the preparation of carbon spheres. Samples were treated with CO2 flow at 850°C by varying activation times to achieve carbon spheres of different pore structures. The CO2 activation process, granting better development of pore structure, provoked a continuous increase in the N2 adsorption capacity together with a modest widening of the PSDs. Comparatively, the CS9 displayed a much rougher surface with more defects on the particle surface due to the accelerated carbonization process at high activation time. It was long enough for the growth of disordered structure of the samples when subjected to high activation time.The adsorption characteristics of methane onto carbon spheres were performed at 298 K and pressures up to 5.0 MPa by a volumetric method. The experimental data of methane adsorption as a function of equilibrium pressure was determined by fitting isotherms to Langmuir and D-A models. The methane adsorption over the carbon spheres was involved in their physical structures. It was concluded that the high surface area and micropore volume of carbon spheres did unequivocally determine methane capacities. In addition, a thermodynamic study of the heat of adsorption of methane on the carbon spheres was carried out. Adsorption of methane on carbon spheres showed a decrease in the heat of adsorption with the increase in surface loadingW/W0, and the heat of adsorption fell from 20.51 to 12.50 kJ/mol at 298 K and then increased to a little higher values at very high loading (>0.70), indicating that methane/methane interactions within the adsorption layer became obvious.



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