Kusrini, E., Utami, C.S., Usman, A., Nasruddin., Tito, K.A., 2018. CO2 Capture using Graphite Waste Composites and Ceria. International Journal of Technology. Volume 9(2), pp. 287-296
|Eny Kusrini||UNIVERSITAS INDONESIA|
|Chairani Utami||Universitas Indonesia|
|Kevin Tito||Universitas Indonesia|
Solid sorbents based on graphite electrode waste and cerium oxide (ceria, CeO2) have been studied with regard to CO2 capture. The acid-base properties of cerium oxide produce a sorbent for the capture of CO2. The aim of the study is to evaluate the performance of CO2 capture using graphite/CeO2 composites at different weights of Ce(NO3)3.6H2O (0.5, 1 and 2 g), namely G0.5, G1 and G2, respectively. Volumetric adsorption studies of CO2 on graphite/CeO2 composites and ceria were conducted at various pressures (P) of 3, 5, 8, 15 and 20 bar, and temperatures (T) of 303, 308, 318 K. Graphite waste before modification (GBM), activated graphite waste (GA), and CeO2 for capturing CO2 were also investigated. By varying the two parameters (P and T), we found that the maximum adsorption capacities of CO2 at 303 K and 20 bar were 0.0713, 0.0316, 0.1574, 0.0987, 0.1137, and 0.0964 kg/kg respectively, for GBM, GA, G0.5, G1, G2 and CeO2. The highest adsorption capacity of CO2 was found in the G0.5 composite. The adsorption performance of CO2 using ceria was almost similar to the G1 composite. We found that CO2 adsorption capacity decreases with an increasing temperature from 303 to 318 K. It was concluded that ceria and composite graphite waste/CeO2 are stable and selective CO2 sorbents. The work allows us to synthesize a new sorbent which can be effectively applied for CO2 capture. The adsorption capacity of CO2 depends significantly on the active site and chemical modifier of the sorbents.
Acid-base properties; Ceria; CO2 Capture; Graphite/CeO2 composite
Controlling the rising carbon dioxide (CO2) level in the atmosphere is a major issue, as the gas caused global warming (Hemalatha et al., 2012). Specifically, the accumulation of carbon dioxide (CO2) emitted into the atmosphere, particularly from fossil fuel combustion in vehicles, industries and power plants, is the cause of this problem (Pham et al., 2016; Zhang et al., 2017). The average CO2 concentration in the atmosphere was 400 ppm in 2015 (Szcz??niak et al., 2017). Clean energy sources and global warming have been among the major issues and challenges for many years, including a reduction in CO2 (Krooss et al., 2002). There have been several efforts to reduce emissions of the gas, most centred on a decrease in the use of fuel oil.
However, natural or bio-gas, which have been explored as replacements for fuel oil, still contain large amounts of CO2, which decreases the calorific value of the gas combustion. Therefore, a purification process is needed to remove CO2 from the fuel gas. On the other hand, CO2 is abundant, non-toxic and easily available, and can also be converted into useful products, such as for renewable carbon resources (Kamimura et al., 2014).
Many technologies for capturing CO2 using the chemical absorption of amine solution have been reported (Du et al., 2017; Deiana et al., 2017). The reaction is influenced by the temperature of absorption, pressure and the pH value of the amine solution (Deiana et al., 2017). Some conventional primary, secondary, tertiary and polyamines solvents are used for capturing CO2 from various industrial process (Singto et al., 2016; Deiana et al., 2017; Bernhardsen & Knuutila, 2017; Du et al., 2017). A state-of-the-art process for capturing CO2 from largely exhausted flue gases has been developed by employing amine-based and regenerative chemical absorption using a primary amine solvent such as aqueous monoethanolamine (MEA) solution ( et al., 2011; Singto et al., 2016; Deiana et al., 2017). A primary amine acts as a weak alkaline and forms a stable carbamate when it reacts with CO2 (Bernhardsen & Knuutila, 2017). Absorption employing amines is an energy-intensive and complex process, requiring a high-energy input for regeneration and handling of the corrosive solvents resulting from the oxidative degradation of the amine-based solutions. The amine solution for capturing CO2 has disadvantages, such as being toxic, flammable and corrosive for some equipment; a high regeneration energy, having a low absorption rate, and suffering amine loss by degradation and volatilization (Du et al., 2017; Zhang et al., 2017). It is a challenge to develop a solid sorbent for the capture of CO2 in the form of a promising technology, as the solid sorbent has the advantage of being energy saving with a stable performance (Yoshikawa et al., 2014; Zhang et al., 2017; Wang et al., 2017).
To obtain CO2 adsorbents with high selectivity, high capacity, high hydrothermality, good mechanical properties, chemical stability, low synthesis cost and also fast adsorption/desorption kinetics has long been an attractive field of investigation (Pevida et al., 2008; Díez et al., 2015; Sarkera et al., 2017; Szcz??niak et al., 2017; Acar et al., 2018). The adsorption process using certain adsorbents is one of the most effective methods for separating or capturing CO2, due to its easy operation and low energy requirements (Lee & Park, 2015; Pham et al., 2016). This process is widely applied in pollution control, waste management, reaction catalysts, gas storage, cooling systems, and gas purification (Elsayed et al., 2017). The production cost of the adsorbent is also a factor which needs to be considered in order to achieve an economically viable process (Szcz??niak et al., 2017). In this regard, graphite waste is of interest due to its abundance (Kusrini et al., 2018b), low price and the fact that it contains a high level of carbon, so it has porous structure. CO2 has high polarizability and quadrupole energy, thus is conveniently adsorbed in solid materials at room temperature (Hemalatha et al., 2012).
The main requirement of an adsorbent is that it is composed of a highly porous material such as zeolite, activated carbon, graphite, zeolite modified MgO, graphitic carbon nitride nanosheets, graphite oxide (GO), graphitic nanostructure, or graphene (Mishra & Ramaprabhu, 2011a; Hemalatha et al., 2012; Casco et al., 2014; Díez et al., 2015; Shin et al., 2016; Acar et al., 2017; Sarkera et al., 2017; Ghosh & Ramaprabhu 2017; Zukal et al., 2017; Babu et al., 2017), so that adsorption can occur on the pore walls or at certain locations within the particle. To increase the adsorption capacity of graphite waste, the surface functional group can be modified by using a metal oxide (Li et al., 2017; Slostowski et al., 2017). Some studies have reported that various metal oxides such as Li2O are capable of adsorbing CO2 molecules on their surfaces (Baltrusaitis & Grassian, 2005; Mosqueda et al., 2006; Hornebecq et al., 2011).
CO2 has the capability associated with the surface of oxides such as cerium oxide (CeO2) due to its acid-base properties (Slostowski et al., 2017). CeO2 has been widely used in catalysis and adsorption (Yoshikawa et al., 2014; Jamalzadeh et al., 2013). The presence of metal oxides can produce a significant improvement in the CO2 capture due to the CO2 interplay (Li et al., 2017). CeO2 can furnish a favorable catalytic activity, and offer a large area of chemical surface and a high surface reactivity. In addition, CeO2 represented a very easily to adsorb water and/or carbon dioxide molecules at room temperature, has reported based of the FTIR spectra (Slostowski et al., 2017).
The graphite/CeO2 composites were prepared according to the method reported by Kusrini et al. (2018a), and were used as the adsorbent for CO2 capture in this study. Ce(NO3)3.6H2O and CeO2 were purchased from R & M Chemicals (Essex, UK). CO2 gas with a high purity of 99.9% was used as the adsorbate and helium gas (He) as a relatively unabsorbed substance in the degassing process. The isothermal adsorption of CO2 on the adsorbents was carried out to obtain the gas absorption capacity data at a pre-determined temperature and pressure.
The surface areas of all the samples were characterized by Brunauer-Emmett-Teller (BET), based on a multipoint adsorption-desorption isotherm of N2 at 77K using ASAP 2020 V4.02 (Micromeritics, US), an equilbration interval of 5 seconds, no low-pressure dose and analysis bath temperatures at 77K. Prior to BET analysis, the sample was subjected to degassing under high vacuum at 350°C for 4 hours.
2.3. Volumetric Adsorption Isotherms
To determine the adsorbent isotherms including gas flow, volumetric and gravimetric methods are used (Elsayed et al., 2017). The volumetric adsorption technique is more commonly used and has the advantage of simplicity of design and cost effectiveness (Siriwardane et al., 2001; Elsayed et al., 2017). The volumetric measurements are the pressure, volume and temperature when the adsorbate contacts the adsorbent. After equilibrium is reached, the amount of CO2 adsorbed is calculated from the pressure changes using the ideal gas equation. In this study, we used the volumetric method.
The adsorption capacity of CO2 by graphite/CeO2 composites was determined using adsorption isotherms by the volumetric principle. The adsorption experiments were performed over the pressure range of 3–20 bar and each cycle of adsorption was followed by the degassing of CO2 at 423 K under vacuum conditions.
The adsorption experiments were carried out at different temperatures, 303, 308, and 318 K, and various pressures, 3, 5, 8, 15 and 20 bar. A
mass of 2.6 g of graphite waste as sorbent
was used. In this study, five types of composites, namely graphite waste
before modification (GBM), activated graphite waste (GA), and modified graphite waste with various weights of cerium oxide (CeO2) (0.5, 1, and 2 g), denoted by G0.5, G1, and G2,
respectively, were used. The adsorption capacity of CO2 was calculated to be the weight (kg) of desorbed CO2 per weight of sorbent (kg).
3.1. CO2 Adsorption Measurement
The adsorption capacity of CO2 using the GBM, GA, graphite/CeO2 composites and also ceria (CeO2) versus the gas pressure are presented in Figure 1(A-F). The amount of adsorbed CO2 increased when the temperature was decreased from 31 K to 303 K. A similar phenomeon can be seen in CO2 adsorption using mesoporous ceria, zeolite and activated carbon, as previously reported (Kamimura et al., 2014). On the contrary, when increasing the pressure from 3 to 8 bar, the adsorption capacity of CO2 increased. This pressure-dependent adsorption capacity indicates that the speed or flow rate of the CO2 adsorbed into the surface of graphite/CeO2 composites increases with CO2 pressure. The decrease in the adsorption capacity with temperature can be related to its adsorption isotherm; in such a physisorption process the adsorption capacity decreases with temperature due to the condensation of the CO2 gas on the surface of the adsorbent. The amount of adsorbate adsorbed on the surface is higher at a lower temperature.
For GBM, it appears that the maximum adsorption capacity of CO2 is 0.0713 kg/kg at a temperature of 303 K and a pressure of 20 bar (see in Figure 1a). The graph shows a linear increase in adsorption capacity after reaching a pressure of 8 bar, especially on the graph line temperature at 318 K. The maximum adsorption capacity of CO2 using activated graphite waste (GA) is 0.0316 kg/kg (see in Figure 1b). The resulting graph is linear, with increasing adsorption capacity as pressure increases.
In particular, for G0.5 and G1, an increase in adsorption capacity was only observed at high pressure above 8 and 15 bar, respectively. For the pressure of 20 bar and temperature of 303 K, the maximum adsorption capacities of CO2 are 0.0713, 0.0316, 0.1574, 0.0987 and 0.1137 kg/kg respectively, for GBM, GA, G0.5, G1 and G2. It can be seen that by adding metal salt (Ce(NO3)3.6H2O) to the activated graphite waste using the wet impregnation method, the adsorption capacity of CO2 was slightly different. It is similarly observed that the adsorption capacity did not correlate with the loaded metal oxides, in terms of surface chemistry (Li et al., 2017). The chemically modified graphite waste with CeO2 tends to have a higher adsorption capacity. Incorporation of CeO2 on the graphite surface made it become more reactive and have a higher adsorption ability due to the formation of interaction between Ce3+ ions and oxygen from the CO2 molecules to form bridged, bidentate, monodentate and/or polidentate manners (Yoshikawa et al., 2014; Slostowskia et al., 2017). Strong interaction with oxygen from CO2 molecules occured when introduced the loading metal oxide onto the graphite waste because of the different surface chemistry of oxide to the carbon surface of graphite.
The adsorption performance of CO2 using CeO2 as adsorbent was also evaluated in the same operating conditions. Figure 1F shows the adsorption isotherm of CO2 using CeO2; the adsorption capacity also decreases with temperature. It is similarly observed that CO2 adsorption capacity decreases with increasing temperature using graphene and graphene-based materials as sorbents, as reported in a previous study (Szcz??niak et al., 2017).
In this study, the maximum adsorption capacity of CO2 using CeO2 is 0.0964 kg/kg at 303 K and 20 bar. This value is comparable to that of the G1 composite (0.0987 kg/kg). This finding may be related to a high affinity of CO2 to interact with the surface of CeO2. It can be understood that CO2 molecules are a Lewis acid, while surface oxygen and/or hydroxyl species in the CeO2 network act as Lewis basic sites. The CO2 could also form hydrogencarbonate and bridged carbonate, producing a weak interaction at room temperature (25°C) (Slostowskia et al., 2017), while by increasing the temperature from 573 to 773K a strong interaction with the CeO2 surface is formed in monodentate, bidentate and polydentate carbonate manners (Yoshikawa et al. 2014; Slostowskia et al., 2017). Although various formations of carbonate species were considered, the interaction of CO2 with the surface of CeO2 seems to be energetically low, where the isosteric heat of adsorption of as-made mesoporous CeO2 was in the range of 30-43 kJ/mol at low coverage of CO2 (Kamimura et al., 2014). Therefore, physisorption mainly takes place, rather than chemisorption.
In this study, the adsorption performance of graphite waste, graphite waste/CeO2 composites, and CeO2 compared to commercial adsorbents such as activated carbon for capturing CO2, where AC2K-300 (activated carbon washed with HCl, then oxidized with air, followed by 10% K2CO3 impregnation and calcination at 300°C) had the highest adsorption capacity, of 110 mg/g at 1000 mbar CO2 and at 25°C (Acar et al., 2018). This value (0.110 kg/g) at 1 bar is slightly higher than those found in this study for GBM (0.0713 kg/kg), GA (0.0316 kg/kg), G1 (0.0987 kg/kg) and CeO2 (0.0964 kg/kg). For the other comparison, the conventional activated carbon with a surface area of 1334 m2/g showed an adsorption capacity of CO2 of 40 cm3/mL at 10 bar, and 70 cm3/mL at 30 bar at 298 K (Kamimura et al., 2014). These values (0.04 and 0.07 kg/kg) are quite similar to the adsorption capacity for GA (0.0316 kg/kg) and GBM (0.0713 kg/kg).
The CeO2 powder with a specific surface area of 199 m2/g reported an adsorption capacity of CO2 of approximately 50 mg of CO2 per gram of CeO2 or 1,130 mmol of CO2/kg CeO2 (Slostowskia et al., 2017). In other study, the CeO2 sample was calcined at 773 K with a surface area of 166 m2/g that was purchased from Daiichi Kigenso Kagaku Kogyo (Yoshikawa et al. 2014), showing an adsorption capacity of CO2 of about 132 mmol/kg. On the other hand, Kamimura et al. (2014) reported that synthesized mesoporous ceria with the highest surface area of 198 m2/g had a CO2 adsorption capacity of 160 cm3/mL at 10 bar and 226 cm3/mL at 30 bar at 298K. The activated modified carbon (AMC) with a loading (10%) of metal oxide (CeO2) had an adsorption capacity of CO2 of 0.32 mmol/g at 0.1 bar and ~1.85 mmol/g at 1 bar when measured at a temperature of 303 K (Li et al., 2017), while AMC showed an adsorption capacity of CO2 of 0.32 and 2.25 mmol/g at 0.1 and 1 bar (Li et al., 2017), respectively.
If we compare with the same precursor from graphite electrode waste, only different in the chemical modifier, the adsorption capacity of CO2 using the graphite waste/Fe3O4 20% composite (0.453 kg/kg) (Kusrini et al., 2017) is higher than that found using the G0.5 composite (0.1574 kg/kg) at a similar temperature (30°C) and pressure (20 bar). This finding has been proven to increase the capacity for capturing CO2 when using magnetite nanoparticles Fe3O4 (Kusrini et al., 2017) and that it is much better than that found for cerium nitrate hexahydrate (Ce(NO3)3.6H2O) and/or CeO2 as modifier.
3.2. Surface Area Analysis
Among the three graphite modifications with metal salt (Ce(NO3)3.6H2O), the highest adsorption capacity (0.1574 kg/kg) was given by G0.5 composite. From our previous report, the surface area of G0.5 is 20.03 m2/g (Kusrini et al., 2018a). For comparison, GBM and G2 have a surface area of 26.35 and 26.82 m2/g respectiely, which is slightly larger than G0.5 composite.
The composites of G0.5, G1 and G2 showed BET surface areas of 20.032, 18.569 and 26.815 m2/g (Kusrini et al., 2018a). In particular, the as-made graphite/CeO2 composites have surface areas higher than the non-porous ceria (4 m2/g and 0.01 cm3/g) (Kamimura et al., 2014).
In this study, their Langmuir surface areas are in agreement with their BET surface areas determined from multilayer adsorption, as shown in Table 1. The t-plot of the external surface area is more effective than that of the micropore area. This can also be indicative of the non- porous composites. In this case, the external surface area is bigger than the internal one (micropore), so it contributed for effectively in the calculation of the BET surface area. The adsorption of CO2 by the graphite/CeO2 composites is most likely to be a physisorption process. It occurs when the intermolecular attraction between the CO2 gas and adsorbent is greater than the intermolecular forces between the solid molecules themselves. This causes the adsorption to occur as an exothermic process.
Note that a BET surface area of graphite non modified (GNM) of 8.490 m2/g was reported by Kusrini et al. (2017). This is significantly lower compared to the when GBM in this study (26.348 m2/g). CO2 capture using GNM has an adsorption capacity of CO2 (0.283 kg/kg), which is higher than that found using GBM (0.0713 kg/kg). Increasing the BET surface area of the sorbents did not have a linear correlation for CO2 capture in this study. Because CO2 capture is higher by the physisorption process, it therefore depends on the active site and chemical modifier itself, such as Ce(NO3)3.6H2O and magnetite nanoparticles Fe3O4 (Kusrini et al., 2017).
CO2 adsorption has been studied in relation to graphite waste composite, activated graphite waste and CeO2 using a volumetric adsorption isotherms. The adsorption is physisorption; the adsorption capacity increases with CO2 pressure, but decreases with temperature. By varying the concentration of Ce salt (Ce(NO3)3.6H2O) in the graphite/CeO2 composites, we found that the maximum adsorption capacity of CO2 was 0.1574 kg/kg when we used the adsorbent type of G0.5 composite at a temperature of 303K and a pressure of 20 bar. This work allows us to synthesise a new sorbent effective for applicability in CO2 capture. The adsorption capacity of CO2 significantly depends on the active site and chemical modifier of the sorbents. Further studies should be carried out on the performance and development of these composites with other types of lanthanides and/or nanoparticles for further commercial applications as adsorbents.
The authors greatly acknowledge the Universitas Indonesia as financial
support through Hibah PITTA No. 2431/UN2.R3.1/KHP.05.00/2018. The referee is
greatly acknowledged for his/her critical and detailed comments as well as
his/her suggestive discussions which are useful and helpful to improve this
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