Journal of Energy

Volume 2013 (2013), Article ID 949408, 15 pages

http://dx.doi.org/10.1155/2013/949408

Research Article

Chemical Looping Combustion of Methane: A Technology Development View

Rutuja Bhoje,¹ Ganesh R. Kale,¹ Nitin Labhsetwar,² and Sonali Borkhade¹

¹CSIR-National Chemical Laboratory (CSIR-NCL), Pune 411008, India

²CSIR-National Environmental Engineering Research Institute (CSIR-NEERI), Nagpur 440020, India

Received 22 February 2013; Accepted 5 August 2013

Academic Editor: Qingjie Guo

Copyright © 2013 Rutuja Bhoje et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

Methane is a reliable and an abundantly available energy source occurring in nature as natural gas, biogas, landfill gas, and so forth. Clean energy generation using methane can be accomplished by using chemical looping combustion. This theoretical study for chemical looping combustion of methane was done to consider some key technology development points to help the process engineer choose the right oxygen carrier and process conditions. Combined maximum product (H₂O + CO₂) generation, weight of the oxygen carrier, net enthalpy of CLC process, byproduct formation, CO₂ emission from the air reactor, and net energy obtainable per unit weight (gram) of oxygen carrier in chemical looping combustion can be important parameters for CLC operation. Carbon formed in the fuel reactor was oxidised in the air reactor and that increased the net energy obtainable from the CLC process but resulted in CO₂ emission from the air reactor. Use of CaSO₄ as oxygen carrier generated maximum energy (−5.3657 kJ, 800°C) per gram of oxygen carrier used in the CLC process and was found to be the best oxygen carrier for methane CLC. Such a model study can be useful to identify the potential oxygen carriers for different fuel CLC systems.

1. Introduction

Energy demand and thus energy generation are ever increasing in many parts of the world. Carbon-based fossil fuels are the main source of energy for combustion reactions. However, the major product of energy generation using fossil fuels by combustion is CO₂, and growing CO₂ pollution has become a matter of serious concern amongst developed as well as developing countries. CO₂ is mainly emitted from energy sector that uses coal, oil, and natural gas for combustion to generate energy for different purposes using air as an oxygen source. Although CO₂ capture and sequestration is being projected as a potential option to control GHG emissions, CO₂ capture technologies in-vogue are beset with several limitations including cost and energy penalty [1, 2]. Hence, these flue gases are directly vented to the atmosphere without CO₂ separation and became responsible for environmental impacts of energy generation from fossil fuels, for example, global warming and climate change phenomena [3–5]. In 2010, CO₂ emissions have already increased to 389.0 ppm and the burning of fossil fuels is one of the main causes for the same as reported by World Meteorological Organization [6]. This has promoted the development of clean energy technologies as a major research area worldwide. Chemical looping combustion (CLC) is an emerging clean energy technology to generate energy using abundantly available fuels and also provides sequestration ready CO₂ stream [7, 8]. CLC uses a solid oxygen carrier (OC) to oxidize the carbon and hydrogen in the fossil fuel to CO₂ and H₂O in an endothermic fuel reactor. The reduced OC is regenerated by air oxidation in the exothermic air reactor [9, 10] in the next step. Both reactors are interconnected and operate simultaneously. The energy released in the CLC system is considered to be of similar magnitude as direct combustion but with a crucial advantage of having separate CO₂ stream [11, 12]. The pure CO₂ steam can be captured/sequestered easily, thereby reducing CO₂ emissions to atmosphere [13].

Development of chemical looping combustion technology requires the relatively cheap and long term availability of fuel and oxygen carrier. Fossil fuel such as methane is abundantly available as natural gas in many countries [14–21]. It is also available as biogas [22–25], landfill gas [26–31], gas hydrates [32–35], and coal bed methane [36] and can be generated from other organic wastes [37–40], and it is a major source of energy by combustion worldwide [41]. The selection of a suitable oxygen carrier (OC) for methane CLC is one the most important aspects for successful technology development study. Apart from the low-cost and abundant availability criteria, the OC must have suitable reactivity with the fuel, easy reducibility, and regenerability under CLC conditions in addition to some other essential properties such as high melting point, attrition resistance, mechanical stability, negligible loses during operation, negligible toxicity, and environmental impacts. The suitability of the oxygen carrier for a fuel can be determined by trial experiments and also by theoretical studies. Some theoretical (thermodynamic) studies of chemical looping combustion have already been reported [42–44], while experimental research studies of chemical looping combustion using methane as fuel with different oxygen carriers have also been published. Mattisson et al. [45] have proposed kinetic data of a promising oxygen carrier consisting NiO/NiAl₂O₄ from experiments in a small fluidized-bed batch reactor using methane as fuel. Corbella and Palacios [46] have experimentally tested titania-supported iron oxides with different iron loadings in a fixed-bed quartz reactor in multicycle tests in a fixed-bed reactor for methane CLC. Johansson et al. [47] have experimentally studied manganese oxides on pure zirconia and zirconia stabilized by CaO, MgO, or CeO₂ as oxygen carrier in a laboratory fluidized-bed reactor of quartz for CLC of methane. Rydén et al. [48] have experimentally investigated red iron oxide, brown iron oxide and iron oxide scales and NiO-based particles as oxygen carrier in a batch fluidized-bed reactor in CLC of methane. Forero et al. [49] have experimentally evaluated Cu-based oxygen carrier in a continuous CLC plant operating with methane and also H₂S as fuel. Kuusik et al. [50] have studied the NiO-based oxygen carriers under oxidising and reducing conditions using ceramic fluidized-bed furnace at high temperatures in CLC of methane. Zafar et al. [51] have proposed reduction and oxidation kinetics of Mn₃O₄/Mg = ZrO₂ oxygen carrier particles in CLC of methane. Abad et al. [52] have studied CLC of methane with CuO impregnated on alumina and developed mathematical model for fluidized bed. Song et al. [53] have studied the chemical-looping combustion of methane with calcium sulfate as a novel oxygen carrier in a laboratory scale fixed-bed reactor.

These studies are helpful to understand the kinetics/reactivity in CLC of methane with different oxygen carriers. However, a theoretical study about CLC with a focus on some important parameters for technology development view is not yet published in the literature to the best of our knowledge. The present study therefore aimed to determine theoretical aspects that can help the technology development criteria for CLC of methane. This study considers the key technology development issues in CLC of methane to evaluate suitability of the oxygen carriers based on other important process parameters such as net desired product generation, net energy obtainable from the system, byproduct generation, fuel conversion, relative weight of the oxygen carriers, effect of pressure and amount of oxygen carrier, and air requirement in oxidation reactor, which are vital parameters to be considered for CLC process design and its practical exploitation.

Technology development requires the use of low-cost, easily available oxygen carrier that can be tested rigorously and repeatedly during experimentation and must have low weight to enable fluidization and transport at low energy consumption in CLC. A detailed theoretical study is essential before experimentation to reduce the efforts of trial experimentation, which are often quite tedious and with several variables significantly affecting the results. Hence, this theoretical study was limited to low-cost, easily available oxygen carriers, preferably simple inorganic compounds consisting of common oxides and sulphates to enable swift experimentation and put technoeconomic potential and commercialization aspects on fast track. Selection of low-cost and easily available oxygen carriers has been discussed in detail in some studies [54, 55]. Based on a similar analysis, the following oxygen carriers were selected for the present study:

The stoichiometric chemical reactions of the oxygen carrier reduction by methane in the fuel reactor as well as the oxygen carrier regeneration by oxygen (air) in the oxidation reactor are presented in Table 1.

Table 1: Stoichiometric chemical reactions for CLC of methane.

Oxygen carrier
Reaction in fuel reactor
Reaction in air reactor

NiO
4NiO + CH₄(g) = 4Ni + 2H₂O(g) + CO₂(g)
Ni + 0.5O₂(g) = NiO

CuO
4CuO + CH₄(g) = 4Cu +2H₂O(g) + CO₂(g)
Cu + 0.5O₂(g) = CuO

CoO
4CoO + CH₄(g) = 4Co +2H₂O(g) + CO₂(g)
Co + 0.5O₂(g) = CoO

CaSO₄
CaSO₄ + CH₄(g) = CaS +2H₂O(g) + CO₂(g)
CaS + 2O₂ = CaSO₄

Na₂SO₄
Na₂SO₄ + CH₄(g) = Na₂S + 2H₂O(g) + CO₂(g)
Na₂S + 2O₂ = Na₂SO₄

Fe₂O₃
1.33Fe₂O₃ + CH₄(g) = 2.66Fe + 2H₂O(g) + CO₂(g)
Fe + 0.75O₂(g) = 0.5Fe₂O₃

Fe₃O₄ + 0.25O₂(g) = 1.5Fe₂O₃

FeO + 0.25O₂(g) = 0.5Fe₂O₃

Mn₂O₃
1.33Mn₂O₃ + CH₄(g) = 2.66Mn + 2H₂O(g) + CO₂(g)
Mn + 0.75O₂(g) = 0.5Mn₂O₃

MnO + 0.25O₂(g) = 0.5Mn₂O₃

2. Methodology

The main reactions for CLC of methane are

where Me is a divalent metal.

Some side reactions leading to byproducts may also occur in the fuel reactor and are listed below:

The fuel reactor product stream has a complex composition. Hence, thermodynamic equilibrium calculations were used to obtain the composition of the product stream of the fuel reactor. These calculations generally use Gibbs free energy minimization algorithms [56–59], simultaneous solution of nonlinear reaction equations using MATLAB programs, or equilibrium reactor modules of commercial software like Design II, HYSYS, or Aspen Plus. The simultaneous solution of nonlinear reaction equations based on equilibrium constants might sometimes become stiff and nonsolvable. An alternate procedure to calculate equilibrium that takes account of chemical species only (not chemical reactions) based on minimization of the total Gibbs energy is shown by the expression:

It shows that all irreversible processes occurring at some constant (temperature) and (pressure) proceed in a direction to the equilibrium state that has the lowest total Gibbs energy attainable at the given and . The method is based on the set of species and is better than that of independent reactions among the species, as the number and nature of chemical reaction equations are not always known perfectly in a new system. HSC Chemistry version 5.1 [60] has been used for this thermodynamic equilibrium study. It uses the Gibbs free minimization algorithm to find the equilibrium compositions using species and not chemical reaction equations. This software is popular and user friendly [61]. Detailed description about calculation of thermodynamic equilibrium using HSC Chemistry is already discussed [62–65]. The species such as CH₄(g), CO₂(g), H₂O(g), CO(g), H₂(g), and C (solid) are considered in this study. Oxygen carriers such as (solid) NiO [66–68], CuO [69, 70], CoO [71, 72], CaSO₄ [73–76], and Fe₂O₃ [77, 78] have been successfully used in chemical-looping studies. Hence, only these oxygen carriers (including hydroxides and carbonates, all solids) along with Na₂SO₄ and Mn₂O₃ were considered in this study. Table 2 shows the species (with reduced oxygen carrier species) used for each oxygen carrier.

Table 2: Oxygen carrier species used and reduced species considered for each oxygen carrier in CLC process.

Sr. number
Oxygen carriers
Species considered

1
NiO
NiO, Ni(OH)₂, Ni, NiCO₃, H₂(g), H₂O(g), CH₄(g), CO(g), CO₂(g), C

2
Fe₂O₃
Fe, Fe₂O₃, FeCO₃, FeO, Fe₃O₄, Fe(OH)₂, Fe(OH)₃, H₂(g), H₂O(g), CH₄(g), CO(g), CO₂(g), C

3
Mn₂O₃
Mn₂O₃, Mn, MnO, MnCO₃, Mn₃O₄, Mn(OH)₂, H₂(g), H₂O(g), CH₄(g), CO(g), CO₂(g), C

4
CaSO₄
H₂S, SO₂, SO₃, COS, CaSO₄, CaS, CaO, CaCO₃, Ca(OH)₂, CaSO₃, H₂(g), H₂O(g), CH₄(g), CO(g), CO₂(g), C

5
Na₂SO₄
H₂S, SO₂, SO₃, Na₂SO₄, COS, Na₂CO₃, Na₂S, Na₂O, Na₂SO₃, NaOH, H₂(g), H₂O(g), CH₄(g), CO(g), CO₂(g), C

6
CoO
Co, CoCO₃, CoO, Co(OH)₂, H₂(g), H₂O(g), CH₄(g), CO(g), CO₂(g), C

7
CuO
CuOH, Cu(OH)₂, Cu, CuCO₃, CuO, Cu₂O, H₂(g), H₂O(g), CH₄(g), CO(g), CO₂(g), C

The input species are methane and oxygen carrier at the particular temperature-pressure condition. No other product-byproduct formations are considered in this study. One mole of methane feed is considered in all the calculations and stoichiometric quantities of oxygen carrier have been used (defined by (2) and (3)). The equilibrium study is limited only to the gas-solid reaction in the fuel reactor. It is assumed that the air reactor conversions are complete due to extremely fast oxidation reactions. The material and energy balance calculations were performed using the inbuilt databases in the HSC Chemistry software package. It is also assumed that the CLC fuel and air reactor operate at the same temperature. The reaction products are assumed to be in thermodynamic equilibrium in the exit of the CLC fuel reactor. The operating temperature range for this study was 600 to 1200°C at 1 bar pressure especially considering methane as fuel. The equilibrium composition data generated by the equilibrium composition module was further used to generate the enthalpy data using the reaction equations module of HSC Chemistry package, for example, input of (CH₄(g) + 4NiO) to the equilibrium composition module produced, (0.1554H₂(g) + 1.8448H₂O(g) + 0.0505CO(g) + 0.9459CO₂(g) + 3.7869Ni + 0.2131NiO + 0.0036C) at 700°C. These compositions were compiled in the reaction equation as

This reaction was input to the reaction equations module of HSC Chemistry software, which calculated the reaction enthalpy () as 145.69 kJ at 700°C. The data analysis and use of this data for technology development aspects have been discussed in next section.

3. Results and Discussion

3.1. Desired Product Yield

The most desired products in CLC of methane are CO₂ and H₂O. CLC process conditions to maximise their formation in the CLC fuel reactor are of vital interest for successful technology development. As a preliminary step, the individual CO₂ and H₂O formation in the CLC fuel reactor was studied and discussed in detail in the next section.

3.1.1. H₂O Yield

The maximum possible H₂O yield in the CLC fuel reactor for 1 mole methane input is 2 moles of H₂O. Figure 1 shows the variation of H₂O yield (moles) for CLC of methane fuel reactor within the temperature range from 600 to 1200°C at 1 bar pressure. It was observed that the H₂O yield for selected oxygen carriers showed a mixed trend; that is, for some oxygen carriers, the H₂O formation increased with increase in temperature, while in other cases, the H₂O yield decreased with increase in temperature. From the figure, it was seen that the moles of H₂O slightly decreased from 1.85 to 1.83 moles with increase in temperature from 600°C to 1200°C for NiO. The same trend was observed for CoO; that is, it decreased from 1.705 to 1.62 moles. But the H₂O yield increased from 1.80 to 1.89 moles up to 850°C then it decreased to 1.81 moles (1200°C) for CaSO₄, while the H₂O yield increased with increase in temperature (i.e., 1.16 at 600°C to 1.64 at 1200°C) for Na₂SO₄. It was also observed that the H₂O yield first decreased from 0.83 to 0.78 moles up to 750°C and then increased to 1.03 moles for Fe₂O₃. However, the H₂O yield remained almost constant at all temperatures (that was the maximum moles of H₂O obtainable) for CuO when compared to all other oxygen carriers (e.g., 1.99 moles at 600°C and 1.99 moles at 1200°C). But the H₂O yield decreased from 0.87 to 0.29 moles with increase in temperature from 600 to 1200°C for Mn₂O₃. The minimum moles of H₂O produced were 0.29 moles for Mn₂O₃ at 1200°C, while the maximum H₂O moles produced were 2.00 for CuO at 600°C. The ranking of oxygen carriers with respect to increasing order of moles of H₂O produced from methane was found to be as follows: CuO (1.99, 600°C) > CaSO₄ (1.89, 850°C) > NiO (1.86, 600°C) > CoO (1.70, 600°C) > Na₂SO₄ (1.64, 1200°C) > Fe₂O₃ (1.03, 1200°C) > Mn₂O₃ (0.87, 600°C).

Figure 1: H₂O yield for CLC of methane.

3.1.2. CO₂ Yield

Similarly, the effect of temperature and oxygen carrier on CO₂ formation in the CLC fuel reactor was studied. The net CO₂ obtainable in the CLC fuel reactor was 1 mole per mole of methane feed. The trends in the CO₂ formation with selected oxygen carriers are shown in Figure 2. It was observed that the CO₂ yield also showed mixed trends (similar to H₂O) for different oxygen carriers with increase in temperature from 600 to 1200°C. The maximum CO₂ yield in CLC fuel reactor was 1.00 mole for its reaction with CuO at 600°C, while the minimum CO₂ yield of 0.06 moles for Mn₂O₃ was calculated at 1200°C. The selectivity of the oxygen carriers based on maximum CO₂ yield (moles) was analysed and was found to be as follows: CuO (1.00, 600°C) > NiO (0.96, 600°C) > CaSO₄ (0.95, 900°C) > CoO (0.88, 600°C) > Na₂SO₄ (0.71, 1050°C) > Fe₂O₃ (0.38, 800°C) > Mn₂O₃ (0.21, 700°C).

Figure 2: CO₂ yield for CLC of methane.

3.1.3. (H₂O + CO₂) Yield

It was clearly seen that the ranking of the oxygen carriers with their suitable operating temperatures was not the same for both major products. Hence, selection of the optimum process conditions was done by using a different parameter. In this case, the combined desired product (H₂O and CO₂) yield from the CLC fuel reactor is considered as a better parameter than individual yields. The maximum yield of 3 moles (1 mole CO₂ + 2 moles H₂O) can be obtained from one mole methane in the CLC fuel reactor. The combined yields of H₂O and CO₂ were plotted in Figure 3 for selected oxygen carriers in the considered temperature range. It was observed that similar to the individual H₂O and CO₂ yields, the oxygen carriers showed different trends for combined yield (CO₂ + H₂O) with increase in CLC fuel reactor temperature. It was observed that the (CO₂ + H₂O) yield for NiO decreased from 2.81 to 2.65 moles with increase in temperature from 600 to 1200°C as reported earlier [42]. Similar trend was observed for Mn₂O₃ and CoO, where the (CO₂ + H₂O) yield decreased from 2.59 to 2.25 moles for CoO and from 1.06 moles to 0.35 moles for Mn₂O₃ with increase in temperature from 600 to 1200°C. The (CO₂ + H₂O) yield increased from 1.45 to 2.34 moles up to 1100°C, and then it remained almost constant till 1200°C for Na₂SO₄. The (CO₂ + H₂O) yield increased with increase in temperature, that is, from 1.04 moles (600°C) to 1.33 moles (1200°C) for Fe₂O₃, while for CaSO₄, the (CO₂ + H₂O) yield increased from 2.64 to 2.84 moles up to 850°C and then decreased to 2.65 moles at 1200°C. In case of CuO, the (CO₂ + H₂O) yield remained almost constant at all temperatures, that is, ~3.00 moles. A maximum (CO₂ + H₂O) yield of 3.00 moles was obtained with CuO at almost all temperatures, while the minimum (CO₂ + H₂O) yield of 0.35 moles was observed for Mn₂O₃ at 1200°C. The ranking of oxygen carriers based on the maximum (CO₂ + H₂O) yield was seen as follows: CuO (2.99, 600°C) > CaSO₄ (2.84, 850°C) > NiO (2.81, 600°C) > CoO (2.59, 600°C) > Na₂SO₄ (2.34, 1100°C) > Fe₂O₃ (1.33, 1200°C) > Mn₂O₃ (1.06, 600°C). This combined product criterion for selection of oxygen carriers and process temperature was useful for process operation.

Figure 3: (H₂O + CO₂) yield for CLC of methane.

3.2. Undesired Product Formation

Some undesired products are also formed in the CLC fuel reactor due to side reactions and thermodynamic limitations under the CLC conditions. An estimation of the nature and amount of the byproducts is important for technology development and hence was studied in detail.

3.2.1. Syngas (H₂ + CO) Formation

Syngas (H₂ + CO) is one of the undesired products of the CLC process. The data of syngas formation in the CLC fuel reactor with selected oxygen carriers within the temperature range from 600 to 1200°C was analyzed and is shown in Figure 4. From the figure, it was observed that the syngas formation increased with increase in process temperature from 600 to 1200°C for all oxygen carriers except for Fe₂O₃, where it was slightly decreased at higher temperature. The syngas formation (moles) increased from 1.13 to 2.64 (Mn₂O₃), 0.35 to 0.75 (CoO), 0.17 to 0.35 (NiO), 0.16 to 0.49 (Na₂SO₄), 0.05 to 0.29 (CaSO₄), and 0.00 to 0.01 moles (CuO) with increase in temperature from 600 to 1200°C. But it was also seen that the syngas formation increased from 1.16 to 1.75 moles up to 900°C and then slightly decreased to 1.67 moles at 1200°C in the case of Fe₂O₃. CuO produced negligible syngas when compared to all other oxygen carriers at all temperatures. The minimum syngas moles produced were negligible for CuO, while the maximum syngas of 2.64 moles was produced by Mn₂O₃ at 1200°C in this study. The ranking of the oxygen carriers based on minimum syngas production (moles) in the CLC fuel reactor was observed as follows: CuO (0.00) > CaSO₄ (0.05) > Na₂SO₄ (0.16) > NiO (0.17) > CoO (0.35) > Mn₂O₃ (1.13) > Fe₂O₃ (1.16) at 600°C.

Figure 4: Syngas formation for CLC of methane.

3.2.2. Carbon Formation

Carbon formation is undesirable in the CLC process as coking may reduce the activity of the solid oxygen carriers. Figure 5 shows the carbon formation in the CLC fuel reactor for methane fuel within the temperature range of 600°C to 1200°C at 1 bar pressure. From the figure, it was observed that the carbon formation was higher at lower temperatures (till ~700°C) due to carbon formation side reactions (5), (6), and (7). It was also seen that the carbon formation decreased with increase in temperature from 600 to 1200°C for all oxygen carriers except for CuO (as found earlier [1]) and CaSO₄ as it was almost zero at all temperatures. The carbon formation steeply decreased from 0.68 at 600°C to 0.010 at 1200°C for Mn₂O₃, while it decreased from 0.63 to 0.001 moles for Fe₂O₃. The carbon formation slightly decreased with increase in temperature, that is, from 0.06 moles at 600°C to 0.00 at 1200°C for CoO. The carbon formation also decreased from 0.013 moles to 0.00 (NiO), from 0.003 moles to 0.00 (Na₂SO₄) within 600 to 1200°C. Fe₂O₃ and Mn₂O₃ produced higher carbon in comparison with the rest of the oxygen carriers at the same temperatures. The maximum carbon yield was 0.68 moles with Mn₂O₃ at 600°C. This solid carbon can be separated from gas stream but cannot be separated from the oxygen carrier, and it is carried to the air reactor where it is oxidised to CO₂. This combustion generates energy but also contaminates the N₂ stream from the air reactor with some CO₂ and increases the air requirement in CLC air reactor. It was seen that all oxygen carriers gave their maximum carbon yield at 600°C. The selectivity of the oxygen carrier as per the decreasing yield of carbon (in moles) is observed as follows: Mn₂O₃ (0.677) < Fe₂O₃ (0.625) < CoO (0.06) < NiO (0.013) < Na₂SO₄ (0.003) < CaSO₄ (0.0002) < CuO (0.00) at 600°C.

Figure 5: Carbon formation for CLC of methane.

3.2.3. SO₂ and H₂S Formation

The possibility of SO₂, COS, and H₂S formation in the CLC fuel reactor while using sulphates as oxygen carriers was also considered in this study, as it was reported by other researchers [79, 80]. Both SO₂ and H₂S are highly undesirable for the process. The results showed that SO₂ and H₂S formation takes place in the CLC fuel reactor.

Figure 6 shows the H₂S and SO₂ formation for the 3 sulphate-based oxygen carriers within the temperature range from 600 to 1200°C at 1 bar pressure per mole methane used in the feed. It was observed that the H₂S formation decreased with increase in temperature for all sulphates. The H₂S formation (moles) decreased from 0.16 to 0.06 for CaSO₄ and from 0.69 to 0.08 moles for Na₂SO₄ with increase in temperature from 600 to 1200°C. The maximum H₂S yield was found to be 0.69 moles at 600°C for Na₂SO₄, while the minimum H₂S yield was found to be 0.06 moles at 1200°C for CaSO₄. Figure 6 also showed that the SO₂ formation increased with increase in temperature for all sulphates. The SO₂ formation increased from 0.00 to 0.1 moles for CaSO₄ and from 0.00 to 0.02 moles for Na₂SO₄ with increase in temperature from 600 to 1200°C. The maximum SO₂ yield was found to be 0.1 moles at 1200°C for CaSO₄, while zero SO₂ formation was observed at lower temperatures till 850°C for Na₂SO₄ and till 650°C for CaSO₄. Hence, according to the data analysis, the choice of better oxygen carrier amongst sulphates was CaSO₄ > Na₂SO₄. H₂S or SO₂ formation reduces the sulphate to its oxide (e.g., CaO and Na₂O), which can be regenerated by using an acid but may require additional processing cost. Commercial systems to trap SO₂ as well as H₂S are available; however, deterioration of sulphate-based oxygen carrier is always a matter of greater concern. Depending on the cost and availability of the sulphate, smart choice of sulphate oxygen carrier can be made.

Figure 6: H₂S and SO₂ gases formation for CLC of methane.

3.3. Reactant Conversions

A study of conversion of the reactants is also important for CLC technology development and hence studied in detail and discussed in the following section.

3.3.1. CH₄ Conversion

Methane conversion in the CLC fuel reactor is one of the important aspects for choosing the oxygen carrier and operating temperature range, as the reactivity of oxygen carriers with methane may be different. Figure 7 depicts the trends in CH₄ conversion with increase in temperature from 600 to 1200°C at 1 bar pressure for the selected oxygen carriers. It was observed from Figure 7 that the CH₄ conversion was almost 100% for all oxygen carriers except for Fe₂O₃ and Mn₂O₃, where lower methane conversion was seen at lower temperatures. The CH₄ conversion increased from 94.22% to 100% for Fe₂O₃, while it was increased from 95.46% to 100% for Mn₂O₃ (also experimentally demonstrated earlier [81]), with increase in CLC fuel reactor temperature from 600 to 1200°C. Complete conversion of CH₄ was achieved for all oxygen carriers in the conditions considered in this study, as these oxygen carriers gave almost 100% methane conversion above 800°C only.

Figure 7: CH₄ conversion for CLC of methane.

3.3.2. Oxygen Carrier Reduction

The reduction of oxygen carrier in the fuel reactor is a key reaction responsible for oxygen availability in CLC reaction and is controlled by the thermodynamic limitations. A study of oxygen carrier conversions in the fuel reactor is also important for calculating the air requirement for regeneration of the oxygen carrier. Hence, all possible reduced states of the oxygen carrier were considered in this study. It was observed that oxygen carriers like NiO, CuO, and CoO were reduced to their respective metals in the fuel reactor. However, oxygen carriers like Fe₂O₃ and Mn₂O₃ were reduced to different reduced states. Similarly, many other species were also formed with the sulfate oxygen carriers in the CLC fuel reactor. The species formed in the CLC fuel reactor of Fe₂O₃ and CaSO₄ were discussed in detail.

3.3.3. Reduced Species of Fe₂O₃

Figure 8(a) shows the different reduced species of Fe₂O₃ for CLC of methane in the temperature range from 600 to 1200°C at 1 bar pressure. From the figure, it was observed that Fe₂O₃ was almost reduced completely into its different reduced species like Fe, FeO, and Fe₃O₄. The moles of FeO and Fe produced increased with increase in temperature; that is, for FeO, it increased from 0.99 to 1.31 moles and for Fe, it increased from 0.44 to 1.08 moles, while the moles of Fe₃O₄ produced decreased with increase in temperature; that is, it decreased from 0.41 to 0.09 moles, while negligible amount of Fe₂O₃ was observed remaining at all temperatures.

(a)

(b)

Figure 8: (a) Reduced species of Fe₂O₃ for CLC of methane. (b) Reduced species of CaSO₄ for CLC of methane.

3.3.4. Reduced Species of CaSO₄

Figure 8(b) shows the different reduced species of CaSO₄ for CLC of methane process in the temperature range from 600 to 1200°C at 1 bar pressure. Reduction behaviour of sulphur containing oxygen carrier is even more important due to the possibility of formation of sulphur-based compounds. From Figure 8(b), it was observed that CaSO₄ almost reduced completely into its different species like CaS, CaO, CaCO₃, Ca(OH)₂, COS, H₂S, and SO₂. The moles of SO₂ and CaO produced were increased with increase in temperature; that is, it increased from 0.00 to 0.1 moles for SO₂ and increased from 0.00 to 0.15 moles for CaO, while moles of CaCO₃ produced decreased with increase in temperature; that is, it decreased from 0.15 moles to its lowest value. Moles of H₂S produced decreased till 950°C, and then slightly increased with increase in temperature; that is, it decreased from 0.16 to 0.05 moles and then increased to 0.06 moles while reverse trend was observed for CaS, that is, moles of CaS produced increased till 850°C and then slightly decreased with increase in temperature, for example, it increased from 0.83 to 0.93 moles and then decreased to 0.84 moles. CaS being the most desirable reduced state, the CLC fuel reactor temperature can be limited to 950°C when CaSO₄ is used as oxygen carrier. Negligible amount of COS and Ca(OH)₂ formation was observed with increase in temperature.

It was observed that the sulfate oxygen carriers suffer losses due to conversion to the oxide and carbonate in the CLC fuel reactor. The oxide and carbonate cannot be separated from the solid stream in continuous operation. Hence, a small amount of sulfate oxygen carrier needs to be added to the process continuously to keep the amount of active oxygen carrier intact. This will also require a continuous small purge of the spent oxygen carrier from the system to avoid overloading of the system. This purged oxygen carrier can be reacted with dilute H₂SO₄, filtered, and dried to convert the oxide and carbonate back to the sulfate for reuse in the system. This modification will be governed by the throughput of the CLC plant, operating cost, and cost of the oxygen carrier.

3.4. Process Energy

The CLC system consists of two reactors in which energy and oxygen carrier transfer occurs between the exothermic (air) reactor and the endothermic (fuel) reactor. It is generally considered that the magnitude of energy obtained in CLC is same as the energy of combustion of the fuel. However, the energy obtainable in CLC depends on the conversion of fuel to different products at different temperatures. As seen in the earlier sections, some other byproducts are also formed in the CLC fuel reactor apart from CO₂ and H₂O. This affects the net energy obtainable from the CLC system for the different oxygen carriers. The study of fuel and air reactor enthalpy trends within the selected temperature range from 600 to 1200°C was essential to calculate the optimum conditions and is discussed in the next section.

3.4.1. Enthalpy of the Fuel Reactor

Methane undergoes oxidation in the fuel reactor generating primarily CO₂ and H₂O, and the oxygen carrier is reduced to its lower oxidation state. The enthalpy of this reaction is plotted against temperature in Figure 9 for different oxygen carriers, based on the equilibrium compositions obtained at those conditions. The CLC fuel reactor enthalpy showed different trends for different oxygen carriers. It was observed that the fuel reactor enthalpy increased with increase in temperature from 600 to 1200°C for CoO (135.15 kJ to 156.22 kJ), while it increased till ~1100°C and then became almost constant with further increase in temperature for Fe₂O₃, Mn₂O₃, and CaSO₄; that is, it increased from 150.09 kJ to 263.04 kJ and remained almost constant (Fe₂O₃), increased from 30.66 kJ to 124.41 kJ and remained almost constant (Mn₂O₃), and also increased from 137.42 kJ to 161.80 kJ (from 600 to 1150°C) and remained almost constant for CaSO₄. However, the reaction enthalpy decreased with increase in temperature in the case of NiO, where it decreased from 146.33 kJ (600°C) to 139.61 kJ (1200°C). The reaction enthalpy showed some increase-decrease trend with increase in temperature for CuO and Na₂SO₄ as shown in the figure. The ranking of oxygen carriers based on the minimum fuel reactor enthalpy is as follows: Fe₂O₃ (263.04 kJ, 1100°C) < Na₂SO₄ (194.90 kJ, 1200°C) < CaSO₄ (161.80 kJ, 1150°C) < CoO (156.22 kJ, 1200°C) < NiO (146.33 kJ, 600°C) < Mn₂O₃ (124.41 kJ, 1100°C) < CuO (−161.48 kJ, 1100°C). However, it was observed that some of the oxygen carriers did not get completely converted to the desired reduced state, and hence there was some loss of oxygen carrier material. Table 3 shows the conversion of the oxygen carrier to its lower oxidation states, some of which can be regenerated by acid reaction. However, this loss was found to be negligible, and assuming that the oxygen carriers are very cheap, the CLC process did not seem to suffer any major cost issues on this point.

Table 3: Conversion of the oxygen carriers during methane CLC.

Sr. number
Oxygen carrier
Initial moles
Reduced state
Waste

1
CuO
4
Cu (4 moles) 100%

2
NiO
4
Ni (3.80 mole) 95.05%

3
CoO
4
Co (3.51 mole ) 87.75%

4
Fe₂O₃
1.33
Fe (1.08 mole) 40.55%,

FeO (1.31 mole) 49.14%

Fe₃O₄ (0.09 mole) 3.29%

5
Mn₂O₃
1.33
MnO (2.68 mole) 99.99%

6
CaSO₄
1
CaO (0.04 mole) 3.88%

CaS (0.93 mole) 92.55%

CaCO₃ (0.02 mole) 2.15%
CaO (0.04 mole) 3.88%

CaCO₃ (0.02 mole) 2.15%

7
Na₂SO₄
1
Na₂S (0.87 mole) 86.677%

Na₂CO₃ (0.033 mole) 3.23%

NaOH (0.02 mole 1.69%)
Na₂CO₃ (0.033 mole) 3.23%

Figure 9: Fuel reactor enthalpy for CLC of methane.

3.4.2. Enthalpy of the Air Reactor

The reduced oxygen carrier along with solid carbon is continuously circulated back to the air reactor for regeneration. Air is passed through the air reactor, and the reduced oxygen carrier and carbon get oxidized completely in the air reactor. This carbon oxidation to CO₂ in the air reactor increases the exothermicity of the air reactor as shown below:

Figure 10 shows the variation of air reactor enthalpy within the temperature range from 600 to 1200°C at 1 bar pressure. It was observed that exothermicity of oxidation increased with increase in air reactor temperature for Na₂SO₄; that is, it increased from −268.51 to −787.29 kJ for Na₂SO₄, while the exothermicity decreased with increase in temperature for NiO, CoO, and Mn₂O₃; it decreased from −903.24 kJ to −852.05 kJ for NiO, decreased from −845.94 kJ to −762.33 kJ for CoO, and decreased from −513.18 kJ to −240.21 kJ for Mn₂O₃ with increase in air reactor temperature from 600 to 1200°C. A different trend was observed for CaSO₄, where the exothermicity of oxidation first increased and then decreased with increase in temperature; that is, it increased from −794.68 kJ (600°C) to −877.44 kJ (800°C) and then decreased to −784.08 kJ (1200°C), while mixed trend was observed for CuO. An enthalpy decrease-increase-decrease trend was observed for Fe₂O₃ as seen in the figure. The selectivity of oxygen carriers according to the maximum exothermicity of the reaction is as follows: NiO (−903.24 kJ, 600°C) > CaSO₄ (−877.44 kJ, 800°C) > CoO (−845.94 kJ, 600°C) > Na₂SO₄ (−787.29 kJ, 1200°C) > CuO (−640.17 kJ, 1100°C) > Fe₂O₃ (−629.23 kJ, 1200°C) > Mn₂O₃ (−513.18 kJ, 600°C).

Figure 10: Air reactor enthalpy for CLC of methane.

3.4.3. Net Process Heat

The net energy required for the CLC process was calculated by summing up the energies of the exothermic air reactor and endothermic fuel reactor for identical oxygen carrier and carbon processing for 1 mole methane feed. The energy generated due to the exothermic air reactor is utilized for reduction of the oxygen carrier in the fuel reactor. The carbon formed in the fuel reactor and its oxidation to CO₂ in the air reactor provided additional energy.

Figure 11 shows that net process heat was obtained by using different oxygen carriers within the temperature range from 600 to 1200°C at 1 bar pressure. It was observed that the net process exothermicity decreased with increase in temperature for NiO, Mn₂O₃, and CoO; that is, it decreased from −756.91 kJ to −712.44 kJ for NiO, decreased from −482.52 kJ to −116.99 kJ for Mn₂O₃, and decreased from −710.79 kJ to −606.11 kJ for CoO, while net process heat increased with increase in temperature for Na₂SO₄; that is, it increased from −164.35 kJ to −592.38 kJ for Na₂SO₄. The net exothermicity first increased and then decreased with increase in temperature; that is, it increased from −657.26 kJ (600°C) to −730.48 kJ (800°C) and then decreased to −623.75 kJ (1200°C) for CaSO₄, while the exothermicity first decreased and then increased with increase in temperature for Fe₂O₃; that is, it decreased from −464.15 kJ (600°C) to −346.2 kJ (900°C) and then increased to −366.46 kJ (1200°C). It was observed that the net process exothermicity remained almost constant for CuO. The oxygen carriers were ranked according to the increase in the net process exothermicity (kJ), and the trend was observed as follows: CuO (−801.68 kJ, 1150°C) > NiO (−756.91 kJ, 600°C) > CaSO₄ (−730.48 kJ, 800°C) > CoO (−710.79 kJ, 600°C) > Na₂SO₄ (−592.38 kJ, 1200°C) > Mn₂O₃ (−482.52 kJ, 600°C) > Fe₂O₃ (−464.15 kJ, 600°C). These values were compared with the value of energy of methane combustion. It was observed that the CLC did not exactly give the complete energy that can be obtained from 1 mole methane by air oxidation. This is due to the byproduct formation in the fuel reactor. Although carbon formed in the CLC fuel reactor is oxidized in the air reactor, the syngas and unconverted methane escape in the CLC fuel reactor product stream mainly causing the loss in fuel and subsequent energy. This loss can be reduced by adding excess of oxygen carrier in the fuel reactor. However, this large additional amount of oxygen carrier for small conversion in the fuel reactor thereby increases the process operating cost. Hence, adding a secondary fuel reactor using some more oxygen carriers to oxidise the H₂, CO, and CH₄ completely in the second stage seems to be a better option.

Figure 11: Net process heat for CLC of methane.

3.5. Weight of Oxygen Carrier

The CLC system involves circulation of the hot oxygen carrier from the air reactor to fuel reactor for reduction. The reduced oxygen carrier is then sent back to the air reactor for oxidation. This continuous recirculation of the solid oxygen carrier requires considerable energy. Hence, an estimate of weight of the oxygen carrier is important for the process engineer to help choose the right oxygen carrier. Table 4 shows the oxygen carrier requirement per mole methane used in the CLC process. It was observed that 4 moles of CuO, NiO, and CoO were required per mole methane used in the CLC process; hence, their weight is much higher than the sulfate oxygen carriers. The CuO, NiO, and CoO oxygen carriers were the heaviest, followed by Fe₂O₃ and Mn₂O₃. The Ca and Na sulfates were found to have lowest weight for use in this study. The favorable oxygen carrier was the lowest amount of the required oxygen carrier (in weight), and the ranking based on this criterion was found to be CaSO₄ > Na₂SO₄ > Mn₂O₃ > Fe₂O₃ > NiO > CoO > CuO. However, the trend of net energy obtainable with stoichiometric amount of oxygen carrier was found to be different. Hence, this criterion was compared on the basis of maximum net energy obtained per gram of the oxygen carrier (Table 4) and the ranking based on this criterion was observed to follow the sequence: CaSO₄ (−5.3657 kJ, 800°C) > Na₂SO₄ (−4.1705 kJ, 1200°C) > NiO (−2.5334 kJ, 600°C) > CuO (−2.5196 kJ, 1150°C) > CoO (−2.3714 kJ, 600°C) > Mn₂O₃ (−2.2981 kJ, 600°C) > Fe₂O₃ (−2.1855 kJ, 600°C).

Table 4: Weight of oxygen carriers.

Oxygen carrier
Molecular wt. of oxygen carrier (for 1 mole)
Moles of oxygen carrier
Oxygen carrier weight (gram)
(max) Net process heat (kJ/gram) of oxygen carrier

CuO
79.55
4
318.18
−2.5196

NiO
74.7
4
298.77
−2.5334

CoO
74.93
4
299.73
−2.3714

Fe₂O₃
159.69
1.33
212.38
−2.1855

Mn₂O₃
157.87
1.33
209.97
−2.2981

CaSO₄
136.14
1
136.14
−5.3657

Na₂SO₄
142.04
1
142.04
−4.1705

3.6. Air Requirement

The CLC of methane can be accomplished by using a variety of oxygen carriers. The reduction of oxygen carriers is different to different potentials depending on CLC conditions. The regeneration of the reduced oxygen carrier as well as carbon oxidation reaction requires air for regeneration. The (stiochometric) requirement of air moles in the air reactor per mole of methane used in CLC was calculated to understand the operating costs related to air input. Figure 12 shows the total air moles required for different oxygen carriers in CLC of methane process in the temperature range from 600°C to 1200°C. The oxygen carrier and carbon were oxidised by air in the air reactor. It was observed that total moles of air used decreased with increase in temperature for NiO, Mn₂O₃, and CoO; it decreased from 9.11 to 8.69 moles for NiO, decreased from 6.40 to 3.24 moles for Mn₂O₃, and decreased from 8.68 to 7.73 moles for CoO, while the total air moles used remained almost constant at 9.50 moles for CuO and it increased with increase in temperature for Na₂SO₄, that is, from 2.56 to 7.55 moles for Na₂SO₄, while for Fe₂O₃, it first decreased from 6.21 (600°C) to 5.35 moles (850°C) and then increased to 5.55 moles (1200°C). The total air moles used first increased till 850°C and then slightly decreased with increase in temperature for CaSO₄; that is, it increased from 7.93 to 8.81 moles and then slightly decreased to 8.04 moles. Selectivity of the oxygen carriers according to the lowest amount of air moles used in the process was as follows: Na₂SO₄ (2.56 moles, 600°C) > Mn₂O₃ (3.24 moles, 1200°C) > Fe₂O₃ (5.35 moles, 850°C) > CoO (7.73 moles, 1200°C) > CaSO₄ (7.93 moles, 600°C) > NiO (8.69 moles, 1200°C) > CuO (9.49 moles, 1200°C).

Figure 12: Air moles required for CLC of methane.

3.7. Effect of Pressure and Amount of Oxygen Carrier on Methane CLC Process

Pressure is an important process parameter. According to Le Chatelier’s principle, the effect of increase in process pressure on the reaction in the CLC fuel reactor seems negative; that is, the H₂O and CO₂ yield decreased with increase in pressure at constant temperature for all oxygen carriers. The amount of oxygen carrier in the CLC system is based on the stoichiometric reaction. However, formation of syngas is seen due to thermodynamic limitations. An increase in the amount of oxygen carrier (greater than the stoichiometric amount) can enhance the conversion of fuel selectively to CO₂ and H₂O. However, this increase in the oxygen carrier quantity can put load on the solid conveying system of CLC. Table 5 shows the increase in the CO₂ yield by using different amounts (S—stoichiometric amount, 2S and 3S) of the oxygen carrier (NiO) at different temperatures. It can be seen that increase in the amount of oxygen carrier increases the solid input to the system in a huge quantity, but the CO₂ yield increases only meagrely. Hence, stoichiometric amount of the oxygen carrier is the optimum quantity to be used in the CLC system.

Table 5: Variation of CO₂ moles with increase in stoichiometric amount (S) of NiO.

(a)  

(S = stoichiometric amount of NiO)
1S
2S
3S

Weight (grams) of oxygen carrier (NiO)
318.2
636.4
954.6

(b)  

Temperature (°C)
CO₂ moles
% increase (1S-2S)
% increase (1S–3S)

(1S)
(2S)
(3S)

600
0.9588
0.9984
0.9992
4.1335
4.2159

750
0.9353
0.9960
0.9980
6.4931
6.7037

1000
0.8696
0.9884
0.9941
13.6714
14.3269

1200
0.8151
0.9791
0.9893
20.1251
21.3765

3.8. Discussion

Properties of oxygen carrier significantly affect the overall performance of CLC process. The oxygen carriers selected for this study have been reported by researchers as potential oxygen carriers under experimental reaction and regeneration trials. The results obtained in this study inferred valuable information for selection of oxygen carrier for methane CLC. Table 6 shows the preferable oxygen carriers for the different criteria. From Table 6, it is observed that CuO and NiO showed better results among the oxide-based oxygen carriers. CuO and NiO have good desired product yield with negligible undesired product formation. Net process heat per gram of oxygen carrier is found to be maximum for NiO, followed by CuO. Among the sulphate-based oxygen carriers, CaSO₄ showed better results under most of the conditions considered. CLC operation involves the fluidization of oxygen carrier particles, and the energy required for solid oxygen carrier transport is a critical parameter for process operation. Hence, it is desirable to obtain maximum energy in CLC using lowest weight (amount) of oxygen carrier. Although the performance of oxygen carriers like NiO and CaSO₄ is similar, CaSO₄ produces higher net process heat in methane CLC per gram of oxygen carrier used in the process.

Table 6: Ranking of oxygen carrier.

Sr. number
Criteria for section of oxygen carrier
Ranking of oxygen carrier

1
H₂O yield (moles)
CuO > CaSO₄ > NiO > CoO > Na₂SO₄ > Fe₂O₃ > Mn₂O₃

2
CO₂ yield (moles)
CuO > NiO > CaSO₄ > CoO > Na₂SO₄ > Fe₂O₃ > Mn₂O₃

3
H₂O + CO₂ yield (moles)
CuO > CaSO₄ > NiO > CoO > Na₂SO₄ > Fe₂O₃ > Mn₂O₃

4
Carbon formation (moles)
Mn₂O₃ < Fe₂O₃ < CoO < NiO < Na₂SO₄ < CaSO₄ < CuO

5
Syngas yield (moles)
CuO > CaSO₄ > Na₂SO₄ > NiO > CoO > Mn₂O₃ > Fe₂O₃

6
Net process heat (kJ)
CuO > NiO > CaSO4 > CoO > Na₂SO₄ > Mn₂O3 > Fe₂O₃

7
Oxygen carriers used (gram)
CaSO₄ > Na₂SO₄ > Mn₂O₃ > Fe₂O₃ > NiO > CoO > CuO

8
Air moles required in CLC process of methane (moles)
Na₂SO₄ > Mn₂O₃ > Fe₂O₃ > CoO > CaSO₄ > NiO > CuO

9
Net process heat/gram of oxygen carriers (kJ/g)
CaSO₄ (−5.3657 kJ, 800°C) > Na₂SO₄ (−4.1705 kJ, 1200°C) > NiO (−2.5334 kJ, 600°C) > CuO (−2.5196 kJ, 1150°C) > CoO (−2.3714 kJ, 600°C) > Mn₂O₃ (−2.2929 kJ, 600°C) > Fe₂O₃ (−2.1805 kJ, 600°C)

4. Conclusion

A theoretical study of CLC of methane process was done for some important criteria related to technology development using different low-cost, easily available inorganic solids as oxygen carriers and some interesting results were obtained. While oxygen carrier plays very crucial role in technoeconomic feasibility of CLC process, the choice of the oxygen carrier in CLC for a particular fuel is affected by several factors. The combined desired product yield (H₂O + CO₂) is a better criterion than individual products yield to obtain optimum condition in CLC. Carbon formation in the fuel reactor eventually forms CO₂ in the air reactor, and hence the oxygen carrier/process condition resulting in negligible carbon formation in fuel reactor must be chosen. The CLC process should be operated at the desired condition to get maximum net obtainable energy. The oxygen carrier can result in several reduced species. The oxygen carrier that delivers the maximum net energy per unit weight in the CLC process should be preferred for the reasons discussed. The oxygen carrier requiring lowest continuous air input in the air reactor is also preferable. Oxides such as Fe₂O₃ and Mn₂O₃ showed multiple reduced states, while CuO, CoO, and NiO had only one reduced state. H₂S, SO₂, oxide, and carbonate formation were observed in sulfates as oxygen carriers; however, in this case, the operating weight of oxygen carrier as well as operating air requirement was less as compared to the oxide-based oxygen carriers. The combined desired product yield (CO₂ + H₂O) was maximum for CuO and CaSO₄. It was observed that CuO resulted in zero carbon formation over the operating temperature range, while CaSO₄ had almost negligible carbon formation. The net energy obtained per gram of the oxygen carrier and CH₄ conversion was found to be maximum for CaSO₄. The reduced species of CaSO₄ like CaS can be regenerated by air oxidation, while CaO can be reacted with dil. H₂SO₄ to form CaSO₄. Use of CaSO₄ results in slight formation of H₂S and SO₂. The formation of syngas is found to be negligible for CaSO₄. Even though CuO shows better results for few cases, CaSO₄ is more preferable because of the limitation of the operating temperature range for CuO as it could not be reoxidized to its original state due to sintering, which has been studied by some researchers [82, 83]. This also explained some discrepancy in graphs observed for CuO at higher temperatures. Overall, considering the complexity of CLC operations with large number of variables as well as significantly different behaviours of various oxygen carriers at different temperatures, it is essential to understand their thermodynamic properties and theoretical estimations of various parameters. These findings can also be extended to other similar materials and fuels for CLC.

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