**4. Adsorbent performance**

*Carbon Capture*

and a small amount of Ca(OH)2. Both the quail eggshell and the oyster shell share

This suggests a similar mineralogical identity. After calcination (thermal treatment process), the diffraction lines attributed to rhombohedral phase for CaCO3 disappeared, with new diffraction patterns arising around 2θ = 32.3°, 37.4°, 53.7°, 63.9°, and 67.3° assigned to cubic phase for lime (CaO) appeared (**Figure 3**). It is worthy to note that the quail eggshell exhibited a crystallite size of 315 nm (CaCO3), while its calcined counterpart showed a size of 240 nm, CaO [23]. This crystallite size decrease can be ascribed to the exothermic natures of the calcination process. However, the lower intensity peaks for calcined eggshell and oyster shell could be related to the reduction in the crystallite size [21, 23]. Hence, the changes in the XRD pattern as a result of calcination are because of the release of carbon dioxide

The associated complexity and high cost for the production of carbon dioxide capture adsorbent materials such as activated carbon or zeolite has shifted attention to exploiting and developing cheap and renewable materials such as eggshells and seashells biomaterials. **Figure 4** shows the procedure involved in the preparation of sorbent material from eggshells and seashells. The waste eggshells and seashells first undergo pre-treatment, which begins with acetic acid treatment with a concentration in the range of 1–10 molar to remove dirt, membrane layer, fibrous matters, proteins and other impurities as well as improve pore structure of the biomaterial [24]. Exposing the waste shells to acetic acid promotes the detachment of protein-collagen membrane depending on the extent, concentration and duration. At the end of this process, the sample is filtered and rinsed with distilled or deionised water. The separated eggshell or seashell is dried at 100–200°C for 5 h [16]. The dried biomaterials are crushed and then sieved into different particle size ranges depending on the application. The particles are calcined; the calcination process involves heat treatment to decompose the major component CaCO3 into CaO. The temperature of calcination could range from 500 to 1000°C depending on the application. It has been reported that at 900°C, the CaCO3 undergoes complete conversion into CaO [21]. The material produced after calcination is the sorbent material, which is placed in a desiccator to curtail the chances of coming in contact

In the pre-treatment phase, the reaction of acetic acid with CaCO3 results in the formation of calcium acetate, which has a larger molar volume than CaCO3 and CaO [25]. The acetic acid treatment helps to expand and improve particle pore structure. As a result of the expanded and enhanced pore network structure, improve performance is achieved over multiple carbonation-calcination reaction

identical diffraction patterns for both the natural and calcined forms.

from the decomposition of CaCO3 into CaO.

with humidity and carbon dioxide in the air.

*Adsorbent material preparation procedure from eggshell and seashells.*

**3. Methods of sorbent preparation**

**88**

**Figure 4.**

The continuing reliance on fossil fuels such as coal, natural gas and crude oil emits greenhouse gas (GHG) especially carbon dioxide (CO2), a major contributor to global warming. The application of physical and chemical absorption using solvents such as selexol, rectisol, and mono-ethanol-amine (MEA) to remove carbon dioxide from flue gas streams is limited by low-temperature, cost and energy-intensive to regenerate [11]. Produced CaO sorbent material from eggshells or seashells through the method outlined in **Figure 4**, has proven a good candidate for carbon dioxide capture from flue gas stream of power plants. This is owing to their affinity to carbonate in the presence of CO2; resulting in the formation of CaCO3 which is regenerated back to CaO via calcinations while pure CO2 is released for sequestration in the process as shown in **Figure 5**.

Unlike the adsorption process for CO2 capture using activated carbon or zeolite adsorbent materials, eggshells and seashells biomaterials are low-cost and offer exclusive environmental and economic benefits. Additionally, eggshell or seashell-derived CaO sorbent are abundant, renewable, simple to prepare and also possesses excellent thermal stability. The mechanism of CO2 capture by these biomaterials comprises of a series of carbonation-calcination reactions (CCR): calcium oxide (CaO) derived from eggshell or seashell reacts with CO2 in the flue gas stream, leading to calcium carbonate (CaCO3), which then undergoes calcination resulting in the release of a pure CO2 stream for sequestration, and at the same time is regenerated into CaO as shown in **Figure 5** [24]. The pilot-scale demonstration of the concept has been reported for eggshell and oyster shell in the literature [24, 26–29]. The reactions are summarised as follows: carbonation (CaO + CO2 → CaCO3) of the eggshell-derived CaO through reaction with CO2 forms calcium carbonate (CaCO3), while the calcination process (CaCO3 → CaO + CO2), regenerates the CaO bio-composite material, and liberate pure stream of CO2 for sequestration. Sacia et al. [27] investigated CaO sorbents derived from chicken eggshell for CO2 from coal-fired power plants. In the work, they discovered that the pre-treatment of the eggshell with acetic acid enhanced

*Schematic of the eggshell or seashell carbonation – calcination processes for carbon dioxide capture.*

and expanded the derived-sorbent material pore structure and surface area, which favoured CO2 diffusion as mass transport is improved.

**Figure 6** shows the effect of acetic acid concentration and treatment time on CO2 capture over multiple cycles. It is clear that the acetic acid treated eggshell outperformed the untreated counterpart. On the other hand, derived CaO from eggshell treated with a low concentration of acetic acid exhibited better reactivity and CO2 capture capacity than that treated with higher concentration. This can be attributed to the improved reactivity and porous surface structure within the biomaterials when treated with an optimised concentration of acetic acid [24, 26, 27].

**Figure 6** also demonstrates that subjecting the eggshell or seashell to a higher strength acetic acid solution or for a longer treatment time could affect the pore structure, strength and stability of the derived CaO sorbent biomaterial. This is consistent with the result of the investigation reported by Sacia [17], on the use of eggshell for CO2 capture. Hence, the observed decrease in the reactivity and CO2 capture capacity under this condition. More also, the data shows that the derived sorbent from eggshell or seashell cannot be continuously regenerated over multiple cycles, as a result, fresh sorbent would be added as make-up during the process to sustain capture capacity (**Figure 6**). Depending on the acetic pre-treatment time, it has been reported that the CO2 capture ranges from 70 to 80% in the first cycle, and gradually drop to about 40% in the fifth cycle [27].

**Figure 7** shows simulated thermogravimetric analyser (TGA) results to prove CO2 capture capacity of eggshell-derived sorbent using a typical flue gas stream (10% CO2 for 60 min cycles at 700°C). The weight of the sample indicates reactivity, while the weight increase signifies carbonation due to CO2 capture; the decrease represents the calcination process because of CO2 liberation. It is clear that the CO2 capture performance and reactivity gradually diminishes for multicycles over time.

The reactivity and CO2 capture capacity of the eggshell or seashell derived CaO sorbent decline over time, so regeneration of sorbents in-situ is pivotal to maintaining CO2 capture. The regeneration can be carried out using deionised water and acetic acid solutions [27]. The effect of regeneration of the eggshell derived CaO sorbent on CO2 capture is shown in **Figure 8**. It is clear that regeneration with acetic acid is more effective than with water. Sacia [17] ascribed this observation to two factors. First, the use of acetic acid resulted in calcium acetate, which exhibited a higher molar volume than only Ca(OH)2 formed when water is used. Also, the combination of water and acetic acid allows for a surface structure rearrangement due to the solubility of calcium acetate in water. It has been found that the use of

**91**

*Eggshell and Seashells Biomaterials Sorbent for Carbon Dioxide Capture*

*Weight vs. time of eggshell-derived adsorbent for CO2 capture using TGA [24].*

2 M acetic acid offers the best performance after multiple cycle regeneration in terms of reactivity and CO2 capture [17, 24]. It can be observed that over three

*Conversion vs. regenerations of eggshell derived CaO sorbent treated with a 1 M acetic acid for 30 min [17].*

In the investigation of Sacia et al. [27], it was found that regeneration restored the reactivity of the eggshell-derived CaO sorbent, and subsequently, CO2 capture capacity in the range of 70–80% was achieved. The CO2 capture capacity increased on average after successive regeneration, as can be seen in **Figure 8**. This suggests that periodic regeneration can effectively increase the reactivity of the spent eggshell or seashell-derived CaO sorbent. In another study by Banerjee et al. [30], it was reported that after four successive regenerations over multi-cycles usage, the carbon dioxide capture capacity of the eggshell-derived sorbent material decreased from 6824 mg CO2/g to 1608 mg CO2/g an average compared to the fresh material. This indicates that the eggshell-derived CaO sorbent biomaterial could hold about eight times its own weight of CO2 from flue gas. Furthermore, Ma and Teng [31] investigated and reported the carbonation – calcination loop of CaO/CaCO3 process for CO2 capture using CaO derived sorbent from oyster shells. Though compared to reagent grade CaO from CaCO3, the oyster shell derived CaO possess bigger crystallite size and lower specific surface area. It was reported that at 740°C carbonation temperature, the oyster shell-derived CaO sorbent in cyclic carbonation exhibited superior performance to the reagent-grade CaO obtained from CaCO3. Therefore, utilising this waste biomaterial in CO2 capture encourages the reuse of materials in the industries, which will reduce the risk, cost and energy associated with mining

regenerations, all of the sorbent showed similar results trend.

*DOI: http://dx.doi.org/10.5772/intechopen.93870*

**Figure 7.**

**Figure 8.**

**Figure 6.** *Effect of acetic acid and treatment time on weight per cent CO2 capture using chicken eggshell [24].*

*Eggshell and Seashells Biomaterials Sorbent for Carbon Dioxide Capture DOI: http://dx.doi.org/10.5772/intechopen.93870*

**Figure 7.**

*Carbon Capture*

and expanded the derived-sorbent material pore structure and surface area, which

**Figure 6** shows the effect of acetic acid concentration and treatment time on CO2 capture over multiple cycles. It is clear that the acetic acid treated eggshell outperformed the untreated counterpart. On the other hand, derived CaO from eggshell treated with a low concentration of acetic acid exhibited better reactivity and CO2 capture capacity than that treated with higher concentration. This can be attributed to the improved reactivity and porous surface structure within the biomaterials when treated with an optimised concentration of acetic acid [24, 26, 27]. **Figure 6** also demonstrates that subjecting the eggshell or seashell to a higher strength acetic acid solution or for a longer treatment time could affect the pore structure, strength and stability of the derived CaO sorbent biomaterial. This is consistent with the result of the investigation reported by Sacia [17], on the use of eggshell for CO2 capture. Hence, the observed decrease in the reactivity and CO2 capture capacity under this condition. More also, the data shows that the derived sorbent from eggshell or seashell cannot be continuously regenerated over multiple cycles, as a result, fresh sorbent would be added as make-up during the process to sustain capture capacity (**Figure 6**). Depending on the acetic pre-treatment time, it has been reported that the CO2 capture ranges from 70 to 80% in the first cycle, and

**Figure 7** shows simulated thermogravimetric analyser (TGA) results to prove CO2 capture capacity of eggshell-derived sorbent using a typical flue gas stream (10% CO2 for 60 min cycles at 700°C). The weight of the sample indicates reactivity, while the weight increase signifies carbonation due to CO2 capture; the decrease represents the calcination process because of CO2 liberation. It is clear that the CO2 capture performance and reactivity gradually diminishes for

*Effect of acetic acid and treatment time on weight per cent CO2 capture using chicken eggshell [24].*

The reactivity and CO2 capture capacity of the eggshell or seashell derived CaO sorbent decline over time, so regeneration of sorbents in-situ is pivotal to maintaining CO2 capture. The regeneration can be carried out using deionised water and acetic acid solutions [27]. The effect of regeneration of the eggshell derived CaO sorbent on CO2 capture is shown in **Figure 8**. It is clear that regeneration with acetic acid is more effective than with water. Sacia [17] ascribed this observation to two factors. First, the use of acetic acid resulted in calcium acetate, which exhibited a higher molar volume than only Ca(OH)2 formed when water is used. Also, the combination of water and acetic acid allows for a surface structure rearrangement due to the solubility of calcium acetate in water. It has been found that the use of

favoured CO2 diffusion as mass transport is improved.

gradually drop to about 40% in the fifth cycle [27].

multicycles over time.

**90**

**Figure 6.**

*Weight vs. time of eggshell-derived adsorbent for CO2 capture using TGA [24].*

**Figure 8.** *Conversion vs. regenerations of eggshell derived CaO sorbent treated with a 1 M acetic acid for 30 min [17].*

2 M acetic acid offers the best performance after multiple cycle regeneration in terms of reactivity and CO2 capture [17, 24]. It can be observed that over three regenerations, all of the sorbent showed similar results trend.

In the investigation of Sacia et al. [27], it was found that regeneration restored the reactivity of the eggshell-derived CaO sorbent, and subsequently, CO2 capture capacity in the range of 70–80% was achieved. The CO2 capture capacity increased on average after successive regeneration, as can be seen in **Figure 8**. This suggests that periodic regeneration can effectively increase the reactivity of the spent eggshell or seashell-derived CaO sorbent. In another study by Banerjee et al. [30], it was reported that after four successive regenerations over multi-cycles usage, the carbon dioxide capture capacity of the eggshell-derived sorbent material decreased from 6824 mg CO2/g to 1608 mg CO2/g an average compared to the fresh material. This indicates that the eggshell-derived CaO sorbent biomaterial could hold about eight times its own weight of CO2 from flue gas. Furthermore, Ma and Teng [31] investigated and reported the carbonation – calcination loop of CaO/CaCO3 process for CO2 capture using CaO derived sorbent from oyster shells. Though compared to reagent grade CaO from CaCO3, the oyster shell derived CaO possess bigger crystallite size and lower specific surface area. It was reported that at 740°C carbonation temperature, the oyster shell-derived CaO sorbent in cyclic carbonation exhibited superior performance to the reagent-grade CaO obtained from CaCO3. Therefore, utilising this waste biomaterial in CO2 capture encourages the reuse of materials in the industries, which will reduce the risk, cost and energy associated with mining

limestone and dolomite for CaCO3 and CaO, and subsequently offers economic and environmental benefits. However, these benefits will be significant if the system is scaled-up to industrial standards.
