# Examination of Perovskite Structure CaMnO3-δ with MgO Addition as Oxygen Carrier for Chemical Looping with Oxygen Uncoupling Using Methane and Syngas

Authors: Dazheng Jing; Tobias Mattisson; Henrik Leion; Magnus Rydén; Anders Lyngfelt
Journal: International Journal of Chemical Engineering
 (2013)

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## Abstract

Perovskite structure oxygen carriers with the general formula CaMnxMg1-xO3-δ were spray-dried and examined in a batch fluidized bed reactor. The CLOU behavior, reactivity towards methane, and syngas were investigated at temperature 900°C to 1050°C. All particles showed CLOU behavior at these temperatures. For experiments with methane, a bed mass corresponding to 57 kg/MW was used in the reactor, and the average CH4 to CO2 conversion was above 97% for most materials. Full syngas conversion was achieved for all materials utilizing a bed mass corresponding to 178 kg/MW. SEM/EDX and XRD confirmed the presence of MgO in the fresh and used samples, indicating that the Mg cation is not incorporated into the perovskite structure and the active compound is likely pure CaMnO3-δ. The very high reactivity with fuel gases, comparable to that of baseline oxygen carriers of NiO, makes these perovskite particles highly interesting for commercial CLC application. Contrary to NiO, oxygen carriers based on CaMnO3-δ have no thermodynamic limitations for methane oxidation to CO2 and H2O, not to mention that the materials are environmentally friendly and can utilize much cheaper raw materials for production. The physical properties, crystalline phases, and morphology information were also determined in this work.


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## Body

## 1. Introduction

Carbon dioxide is the greenhouse gas which contributes most to anthropogenic climate change. A significant amount of CO2 is emitted into the atmosphere each year, of which combustion of fossil fuels was responsible for over 30000 million tons of CO2 in 2010 [1]. The increasing energy demand of a globally growing economy will likely make fossil fuels the main energy source in the foreseeable future. Hence, reducing CO2 emission from combustion of fossil fuels is a key point in reducing the impact of global warming.CO2 capture and storage (CCS) is one important option to reduce CO2 emission. In this concept, CO2 produced from combustion or industrial processes is captured and stored in closed geological formations where it is stored for long periods of time before being converted to carbonate minerals or other stable phases by natural processes. Some of the carbon dioxide may actually leak to the atmosphere, but if the leakage rate is low enough, this may not be of significant importance as natural mechanisms could sequester the carbon. CO2 capture can be achieved by different technologies and the most discussed are postcombustion, precombustion and oxyfuel combustion. Unfortunately, a substantial energy penalty is required for gas separation in these technologies [2]. Chemical-looping combustion is a process of burning fuel where the air and fuel are never mixed and where CO2 is inherently separated from the rest of the flue gases without any direct energy expenditure. There has been a strong interest for this technology in the last decade, as judged by the number of research groups working in the field and the number of scientific articles published [3, 4].Chemical-looping combustion is an innovative combustion technology in which there is no direct contact between combustion air and fuel. A chemical-looping combustion unit consists of two reactors, an air reactor and a fuel reactor; see Figure1 [5]. Solid oxygen carriers, which are usually metal oxide particles, are oxidized in the air reactor according to reaction (1) and circulated to the fuel reactor, where they are reduced by the fuel according to reaction (2). The oxygen needed for fuel conversion is supplied by the solid oxygen carrier particles. The reduced particles are recirculated to the air reactor and the process is repeated. The heat produced by CLC is the same as a conventional combustion which is revealed by combining reaction (1) and (2). After steam condensation, high purity CO2 ready for compression and storage is obtained after the fuel reactor. By transferring oxygen by solid oxygen carriers, the combustion products are not diluted with N2 from the air. Thus the energy required for gas separation is avoided. Also, the CO2 capture efficiency can reach 100% in chemical-looping combustion [6, 7]. These unique features make chemical-looping combustion a very interesting option for CO2 capture
(1)O2+2MexOy-1⟶2MexOy(2)CnH2m+(2n+m)MexOy⟶nCO2+mH2O+(2n+m)MexOy-1Figure 1
Schematic representation of a CLC unit.In the fuel reactor, some kinds of oxygen-carrier materials are able to release gaseous oxygen according to reaction (3). In a subsequent step, the fuel reacts directly with the released oxygen according to reaction (4). Such a process is referred to as chemical-looping with oxygen uncoupling (CLOU) [8]. Oxygen carriers with the ability to release gas phase O2 are referred to as CLOU materials
(3)2MexOy⟶2MexOy-1+O2(4)CnH2m+(n+12m)O2⟶nCO2+mH2OOxygen carriers are most often based on metal oxides, which can be cyclically oxidized and reduced when exposed to different environments. For a metal oxide to be an oxygen carrier and the CLC process to be operationally feasible with high CO2 capture efficiency, certain properties of a material are required.(a)
Suitable thermodynamic and kinetic properties under combustion conditions. This means that materials can be oxidized and reduced at relevant conditions with sufficient reaction rates. The reactivity towards fuels should be high in CLC, and the rate of oxygen release should be high in the CLOU process.(b)
The performance of an oxygen carrier should be stable in long-term operation.(c)
When using fluidized beds for both the air and the fuel reactor, good fluidizing properties are required, for example, the particles should not form agglomerations.(d)
Resistance against attrition and mechanical strength should be high.(e)
The oxygen carrier should be environmental friendly and have reasonable costs.Mn, Cu, Ni, Co, Cd, and their corresponding oxides have been proposed as possible oxygen carrier candidates [9–11]. Among a large number of studied oxygen carriers, NiO-based oxygen carrier has been successfully demonstrated in 10 kW [12] and 120 kW CLC units [13]. In the 10 kW unit, a NiO-based material has been operated more than 1000 h achieving high CH4 conversion and very low loss of fines, corresponding to over 30 000 h life time [12]. Considering the good experience obtained with Ni-based oxygen carriers with respect to reactivity and stability with gaseous fuels, at present NiO could be considered to be the baseline CLC oxygen carrier. However, Ni-based materials have some important disadvantages, most critically being the high toxicity. In addition, Ni is expensive and has a negative equilibrium restraint for fuel conversion [14]. For CLOU materials, CuO has been investigated extensively [8, 15–19]. Although Cu-based oxygen carriers in general seem to have very high rates of oxygen uncoupling, copper is also fairly expensive, and there have been problems reported related to agglomeration and stability [20–22]. For uplifting chemical-looping combustion to the next scale application, developing new materials with lower cost than Ni and Cu but with CLOU properties would be of significant value.Theoretically, Mn2O3 is capable of releasing oxygen in the fuel reactor during chemical-looping combustion. But the oxidation of Mn3O4 to Mn2O3 is thermodynamically hindered at temperatures above ≈800°C. At lower temperatures, where there are no thermodynamic limitations, the oxidation of Mn3O4 to Mn2O3 is hard to achieve, probably due to kinetic limitations [23]. One option to improve the thermodynamic and kinetic properties of manganese oxides is to combine them with other metal oxides forming combined oxide systems. Mn-Fe combined oxides were studied by Azimi et al. [24, 25], Rydén et al. [26], and Shulman et al. [27] showing that such oxides had CLOU capability and rapid oxidation rate at 850°C. Jing et al. [28] have studied the Mn-Si combined oxide system and CLOU behavior; high methane and syngas conversion were reported. Rydén et al. [29] provided an overview of six combined manganese oxides systems which have been studied so far with respect to CLOU, and Mattisson has provided a general overview of CLOU materials [30].One of the more interesting combined oxides is the perovskite structure calcium manganite, or CaMnO3-δ. This type of materials is of defect perovskite structure with general formula ABO3-δ. In such a structure, the oxygen deficiency δ can vary depending on the surrounding oxygen partial pressure or temperature [31, 32]. When the surrounding oxygen partial pressure decreases, the defect grows by releasing oxygen according to reaction (5), and this oxygen can be utilized by the fuel in accordance with the CLOU process described above
(5)2ABO3-δ⟶2ABO3-δ-a+aO2Another promising feature of such materials is that there is no distinct phase transition between oxidized ABO3-δ and reduced ABO3-δ-a. This may be advantageous and may help in avoiding the attrition problem caused by structural changes between oxidized and reduced phase. CaMn0.875Ti0.125O3 has been examined in TGA, batch fluidized reactor, and small scale fluidized bed reactor showing good CLOU properties, high reactivity towards methane, and good fluidization behavior by Leion et al. [33] and Rydén et al. [34] Another set of CaMn(1-x)MxO3-δ (M=Ti, Fe, Mg) materials with good reactivity results and CLOU properties were examined by Hallberg et al. [35] using a batch fluidized bed reactor system. Here, it was found that a calcium manganite material doped with MgO showed the most promising performance.


## 2. Objective

In the previous screening work of CaMn(1-x)MxO3-δ (M=Ti, Fe, Mg) materials [35], CaMn(1-x)MgxO3-δ with 2.7 wt% and 5.6 wt% MgO exhibited CLOU behavior and high methane conversion at 950°C. These two materials were selected and their performance was further examined. The ability to release gas phase oxygen and the reactivity towards methane and syngas at different temperatures as well as the stability over many red-ox cycles were investigated. Also, physical and chemical properties, for instance the crushing strength and the crystalline phases, of the oxygen carrier particles were analyzed.


## 3. Experimental Section

### 3.1. Manufacture of Oxygen Carriers

The oxygen carriers examined in this work were manufactured by VITO, Belgium, using spray-drying. Spray-drying is an industrial process for producing high spherical, free-flowing, homogeneous granulated powder of uniform bulk density. Inorganic raw materials Ca(OH)2, Mn3O4, and MgO were weighed and dispersed in deionized water with appropriate amounts of organic binders and dispersants. The water based suspension was homogenized by milling in a planetary ball mill. The slurry was continuously stirred with a propeller blade mixer while being pumped into an atomizer which was located in the drying chamber. Under the effects of surface tension, the pumped slurry was broken into a large number of droplets which quickly dried by heated air due to a large surface-to-volume ratio of the droplets thus transformed rapidly into dry powders and separated from the hot air. The particles synthesized were sieved and sintered at 1100°C, 1200°C, or 1300°C for 4 h in air to obtain sufficient mechanical strength. Oxygen carriers in the diameter range 125–180 μm were selected for reactivity testing and 180–212 μm for crushing strength (CS) measurements. The compositions of the examined oxygen carriers are presented in Table 1. In the screening work of Hallberg et al. [35], the 5.6% MgO and 2.7% MgO oxygen carriers were presented as C13 and C14, respectively. Källén et al. [36] used CaMn0.9Mg0.1O3 to notate the 2.7% MgO material which was used in continuous operation.Table 1
Composition of Ca-Mn-Mg oxygen carriers.
Notation
Molar composition
Synthesis composition
Sintering temperature
Sintering time(h)
(wt%)
(°C)
5.6% MgO
CaMn0.8Mg0.2O3
42.6% Mn3O4
1100, 1200, 1300
4
51.8% Ca(OH)2
5.6% MgO
2.7% MgO
CaMn0.9Mg0.1O3
46.8% Mn3O4
1100, 1200, 1300
4
50.5% Ca(OH)2
2.7% MgO


### 3.2. Characterization of Oxygen Carriers

The hardness of an oxygen carrier is measured by the force needed to fracture a particle and is typically referred to as crushing strength (CS) [37]. In this work, crushing strength was measured with a Shimpo FNG-5 apparatus on fresh particles with diameter 180–212 μm. 30 particles were measured for each sample, and the average value is given as the CS for the sample.The chemical compositions and crystalline structures of the oxygen carriers were identified by X-ray powder diffraction using a Siemens D5000 diffractometer utilizing copper Kα1 radiation. Light microscopy and scanning electron microscopy (SEM), FEI Quanta 200 Environmental, were used to provide morphology information of the materials. With the help of an Oxford Inca Energy dispersive X-ray system (EDX) attached to SEM, the elemental composition on particles’ surface was obtained.


### 3.3. Batch Fluidized Bed Reactor System

The reactivity tests were conducted in a quartz fluidized bed reactor with total length of 870 mm and inner diameter of 22 mm. A porous plate supporting bed material was placed 370 mm from the bottom. The temperature was measured 25 mm above and 5 mm underneath the porous plate by Pentronic CrAl/NiAl thermocouples enclosed in inconel-600 alloys inside quartz shells. Honeywell pressure transducers with 20 Hz frequency was used to measure the pressure drop over the particle bed and the porous plate.A specified amount of oxygen carrier with diameter 125–180μm was placed on the porous plate for the reactivity test. Initially, the particles were heated to the reaction temperature in a gas mixture of 5% O2 in N2. The reacting gases were then introduced from the bottom of the reactor. Flue gases leaving from the top of the reactor were cooled by an electric cooler. After condensation of water, the concentrations of CO, CO2, CH4, and O2, as well as the volume flow of the dry gas, were measured with a Rosemount NGA-2000 gas analyzer. Figure 2 is a schematic representation of the reactor system. The same system has been used previously by Jerndal et al. [37], Arjmand et al. [17], Azimi et al. [24, 25], Shulman et al. [27], Jing et al. [28], Sundqvist et al. [38], and Hallberg et al. [35].Figure 2
Schematic representation of the laboratory set-up of the batch fluidized bed system.


### 3.4. Reactivity Tests

#### 3.4.1. Uncoupling Properties and Reactivity with CH4 and Syngas

A sample of 15 g oxygen carrier with diameter 125–180μm was placed in the quartz reactor and was then heated from room temperature to 900°C in 5% O2. Table 2 outlines the experimental scheme. Firstly, three inert cycles were performed by exposing the particles alternatingly to 100% N2 and 5% O2 at 900°C. By measuring the oxygen concentration during such inert cycles, the oxygen carriers CLOU property could be examined. Subsequently, the particles were exposed to three methane cycles and three syngas (50% CO and 50% H2) cycles at 950°C. Then, three more inert cycles were carried out at 900°C. Afterwards, one 1800 s inert cycle was performed at 1000°C to calculate the materials’ oxygen capacity with respect to CLOU. Finally, the oxygen carriers were cooled down to room temperature during fluidization with 5% O2. The gas flows applied were 900 mLN/min for 5% O2 (in N2), 600 mLN/min for N2, and 450 mLN/min for CH4 and syngas. These flows correspond to 8–28 umf in the oxidation period and 3–9 umf in the reduction period. The experimental procedure, with the injection time for N2 and fuel, is stated in Table 2 for different cycles. N2 was used to flush the reactor for 60 s before and after fuel introduction to prevent back mixing.Table 2
Experimental scheme for oxygen carriers’ reactivity test.
No. of cycles
Inert/reducing gas
t
CLOU
t
In
t
Red
T
Ox
T
Red/TCLOU
(s)
(s)
(s)
(°C)
(°C)
3
Nitrogena
360
900
900
3
Methane
60
20
950
950
3
Syngas
60
80
950
950
3
Nitrogen
360
900
900
1
Nitrogen
1800
900
1000
aThe oxygen concentration was measured during the inert periods in order to evaluate the ability of the oxygen carriers’ to release oxygen in the gas phase.


#### 3.4.2. Temperature Influence on Oxygen Carriers’ Reactivity

The effect of temperature on the performance of oxygen carrier was studied by conducting cyclic reactivity tests in the batch fluidized reactor. As can be seen from Table3, the experiments started at 900°C followed by cycles at 950°C, 1000°C, and 1050°C. Finally, the temperature was reduced to 950°C. The last test was made in order to judge if the redox cycles at higher temperatures had any permanent effect on the particle reactivity behavior. At each temperature, two methane reduction cycles and two inert cycles were carried out, as seen in the table. As before, 15 g of fresh sample was used in this series of tests. After the cycles the material was cooled down to room temperature in 600 mLN/min 100% N2. Gas flows were the same as those used for the experiments described in Section 3.4.1.Table 3
Experimental scheme used for investigation of the effect of temperature on the oxygen carrier reactivity.
No. of cycles
Inert/reducing gas
t
CLOU
t
In
t
Red
T
Ox
T
Red/TCLOU
(s)
(s)
(s)
(°C)
(°C)
2
Methane
60
20
900
900
2
Nitrogen
360
900
900
2
Methane
60
20
950
950
2
Nitrogen
360
950
950
2
Methane
60
20
1000
1000
2
Nitrogen
360
1000
1000
2
Methane
60
20
1050
1050
2
Nitrogen
360
1050
1050
2
Methane
60
20
950
950
2
Nitrogen
360
950
950


#### 3.4.3. Investigation of Reactivity Stability and Reduction Time

The reactivity over many redox cycles was also investigated in this work. A sample of 2 g of CaMn0.8Mg0.2O3 sintered at 1300°C (short for 5.6% MgO 1300) which had previously been used in general reactivity screening was placed in the quartz reactor. The particles were exposed alternatingly to 10% O2 in N2, 100% N2 and pure CH4. The inlet flows were 900 mLN/min for all components. As seen in Table 4, two sets of experiments were done, with the methane injection period set to 2 s and 14 s, respectively, for the different experiments. A total of 50 cycles were conducted for each experiment.Table 4
Experimental scheme for stability tests.
Sample batch
No. of cycles
Reducing gas
t
In
t
Red
T
Ox
T
Red
(s)
(s)
(°C)
(°C)
1
50
Methane
60
2
950
950
2
50
Methane
60
14
950
950


### 3.5. Data Evaluation

Fuel conversion, or fuel yield, is defined as a degree of how much introduced fuel has been fully converted into CO2. It is used to quantify an oxygen carrier’s reactivity towards fuels. Methane and syngas conversion are presented as (6) showing the CH4 and CO conversion to CO2 respectively
(6)γCH4=pCO2pCO2+pCO+pCH4,γsyn=pCO2pCO2+pCO,
where pi is the outlet partial pressure of component i.Oxygen carrier conversion (or solid conversion) is defined as(7)ωi=mimox,
where mi is the mass of the oxygen carrier at time i and mox is the mass of the fully oxidized oxygen carrier. Here, mox is simply the mass of the fresh particles used in the experiments, and no account has been taken to the possible oxygen deficiency at higher temperatures [29]. In a fuel reduction period, ωi can also be calculated as a function of time. Equation (8) shows the oxygen carrier conversion during a methane and syngas reduction period, respectively, as follows:
(8)ωi=ωi-1-∫ti-1tin˙outMomoxPtot(4pCO2,out+3pCO,out-pH2,out)dt,ωi=ωi-1-∫ti-1tin˙outMomoxPtot(2pCO2,out+pCO,out-pH2,out)dt,
where n˙out is the molar flux of flue gas after water condensation and Mo is the molar mass of oxygen. For a specific reduction cycle, γCH4, is sometimes given as an average value from ω=1 to 0.99. The concentration of H2 was not measured during experiments. H2 concentration can be assumed to be low enough to be neglected since H2 generally has a higher reactivity than CO [39] and the CO concentration was very low under all conditions.


## 3.1. Manufacture of Oxygen Carriers

The oxygen carriers examined in this work were manufactured by VITO, Belgium, using spray-drying. Spray-drying is an industrial process for producing high spherical, free-flowing, homogeneous granulated powder of uniform bulk density. Inorganic raw materials Ca(OH)2, Mn3O4, and MgO were weighed and dispersed in deionized water with appropriate amounts of organic binders and dispersants. The water based suspension was homogenized by milling in a planetary ball mill. The slurry was continuously stirred with a propeller blade mixer while being pumped into an atomizer which was located in the drying chamber. Under the effects of surface tension, the pumped slurry was broken into a large number of droplets which quickly dried by heated air due to a large surface-to-volume ratio of the droplets thus transformed rapidly into dry powders and separated from the hot air. The particles synthesized were sieved and sintered at 1100°C, 1200°C, or 1300°C for 4 h in air to obtain sufficient mechanical strength. Oxygen carriers in the diameter range 125–180 μm were selected for reactivity testing and 180–212 μm for crushing strength (CS) measurements. The compositions of the examined oxygen carriers are presented in Table 1. In the screening work of Hallberg et al. [35], the 5.6% MgO and 2.7% MgO oxygen carriers were presented as C13 and C14, respectively. Källén et al. [36] used CaMn0.9Mg0.1O3 to notate the 2.7% MgO material which was used in continuous operation.Table 1
Composition of Ca-Mn-Mg oxygen carriers.
Notation
Molar composition
Synthesis composition
Sintering temperature
Sintering time(h)
(wt%)
(°C)
5.6% MgO
CaMn0.8Mg0.2O3
42.6% Mn3O4
1100, 1200, 1300
4
51.8% Ca(OH)2
5.6% MgO
2.7% MgO
CaMn0.9Mg0.1O3
46.8% Mn3O4
1100, 1200, 1300
4
50.5% Ca(OH)2
2.7% MgO


## 3.2. Characterization of Oxygen Carriers

The hardness of an oxygen carrier is measured by the force needed to fracture a particle and is typically referred to as crushing strength (CS) [37]. In this work, crushing strength was measured with a Shimpo FNG-5 apparatus on fresh particles with diameter 180–212 μm. 30 particles were measured for each sample, and the average value is given as the CS for the sample.The chemical compositions and crystalline structures of the oxygen carriers were identified by X-ray powder diffraction using a Siemens D5000 diffractometer utilizing copper Kα1 radiation. Light microscopy and scanning electron microscopy (SEM), FEI Quanta 200 Environmental, were used to provide morphology information of the materials. With the help of an Oxford Inca Energy dispersive X-ray system (EDX) attached to SEM, the elemental composition on particles’ surface was obtained.


## 3.3. Batch Fluidized Bed Reactor System

The reactivity tests were conducted in a quartz fluidized bed reactor with total length of 870 mm and inner diameter of 22 mm. A porous plate supporting bed material was placed 370 mm from the bottom. The temperature was measured 25 mm above and 5 mm underneath the porous plate by Pentronic CrAl/NiAl thermocouples enclosed in inconel-600 alloys inside quartz shells. Honeywell pressure transducers with 20 Hz frequency was used to measure the pressure drop over the particle bed and the porous plate.A specified amount of oxygen carrier with diameter 125–180μm was placed on the porous plate for the reactivity test. Initially, the particles were heated to the reaction temperature in a gas mixture of 5% O2 in N2. The reacting gases were then introduced from the bottom of the reactor. Flue gases leaving from the top of the reactor were cooled by an electric cooler. After condensation of water, the concentrations of CO, CO2, CH4, and O2, as well as the volume flow of the dry gas, were measured with a Rosemount NGA-2000 gas analyzer. Figure 2 is a schematic representation of the reactor system. The same system has been used previously by Jerndal et al. [37], Arjmand et al. [17], Azimi et al. [24, 25], Shulman et al. [27], Jing et al. [28], Sundqvist et al. [38], and Hallberg et al. [35].Figure 2
Schematic representation of the laboratory set-up of the batch fluidized bed system.


## 3.4. Reactivity Tests

### 3.4.1. Uncoupling Properties and Reactivity with CH4 and Syngas

A sample of 15 g oxygen carrier with diameter 125–180μm was placed in the quartz reactor and was then heated from room temperature to 900°C in 5% O2. Table 2 outlines the experimental scheme. Firstly, three inert cycles were performed by exposing the particles alternatingly to 100% N2 and 5% O2 at 900°C. By measuring the oxygen concentration during such inert cycles, the oxygen carriers CLOU property could be examined. Subsequently, the particles were exposed to three methane cycles and three syngas (50% CO and 50% H2) cycles at 950°C. Then, three more inert cycles were carried out at 900°C. Afterwards, one 1800 s inert cycle was performed at 1000°C to calculate the materials’ oxygen capacity with respect to CLOU. Finally, the oxygen carriers were cooled down to room temperature during fluidization with 5% O2. The gas flows applied were 900 mLN/min for 5% O2 (in N2), 600 mLN/min for N2, and 450 mLN/min for CH4 and syngas. These flows correspond to 8–28 umf in the oxidation period and 3–9 umf in the reduction period. The experimental procedure, with the injection time for N2 and fuel, is stated in Table 2 for different cycles. N2 was used to flush the reactor for 60 s before and after fuel introduction to prevent back mixing.Table 2
Experimental scheme for oxygen carriers’ reactivity test.
No. of cycles
Inert/reducing gas
t
CLOU
t
In
t
Red
T
Ox
T
Red/TCLOU
(s)
(s)
(s)
(°C)
(°C)
3
Nitrogena
360
900
900
3
Methane
60
20
950
950
3
Syngas
60
80
950
950
3
Nitrogen
360
900
900
1
Nitrogen
1800
900
1000
aThe oxygen concentration was measured during the inert periods in order to evaluate the ability of the oxygen carriers’ to release oxygen in the gas phase.


### 3.4.2. Temperature Influence on Oxygen Carriers’ Reactivity

The effect of temperature on the performance of oxygen carrier was studied by conducting cyclic reactivity tests in the batch fluidized reactor. As can be seen from Table3, the experiments started at 900°C followed by cycles at 950°C, 1000°C, and 1050°C. Finally, the temperature was reduced to 950°C. The last test was made in order to judge if the redox cycles at higher temperatures had any permanent effect on the particle reactivity behavior. At each temperature, two methane reduction cycles and two inert cycles were carried out, as seen in the table. As before, 15 g of fresh sample was used in this series of tests. After the cycles the material was cooled down to room temperature in 600 mLN/min 100% N2. Gas flows were the same as those used for the experiments described in Section 3.4.1.Table 3
Experimental scheme used for investigation of the effect of temperature on the oxygen carrier reactivity.
No. of cycles
Inert/reducing gas
t
CLOU
t
In
t
Red
T
Ox
T
Red/TCLOU
(s)
(s)
(s)
(°C)
(°C)
2
Methane
60
20
900
900
2
Nitrogen
360
900
900
2
Methane
60
20
950
950
2
Nitrogen
360
950
950
2
Methane
60
20
1000
1000
2
Nitrogen
360
1000
1000
2
Methane
60
20
1050
1050
2
Nitrogen
360
1050
1050
2
Methane
60
20
950
950
2
Nitrogen
360
950
950


### 3.4.3. Investigation of Reactivity Stability and Reduction Time

The reactivity over many redox cycles was also investigated in this work. A sample of 2 g of CaMn0.8Mg0.2O3 sintered at 1300°C (short for 5.6% MgO 1300) which had previously been used in general reactivity screening was placed in the quartz reactor. The particles were exposed alternatingly to 10% O2 in N2, 100% N2 and pure CH4. The inlet flows were 900 mLN/min for all components. As seen in Table 4, two sets of experiments were done, with the methane injection period set to 2 s and 14 s, respectively, for the different experiments. A total of 50 cycles were conducted for each experiment.Table 4
Experimental scheme for stability tests.
Sample batch
No. of cycles
Reducing gas
t
In
t
Red
T
Ox
T
Red
(s)
(s)
(°C)
(°C)
1
50
Methane
60
2
950
950
2
50
Methane
60
14
950
950


## 3.4.1. Uncoupling Properties and Reactivity with CH4 and Syngas

A sample of 15 g oxygen carrier with diameter 125–180μm was placed in the quartz reactor and was then heated from room temperature to 900°C in 5% O2. Table 2 outlines the experimental scheme. Firstly, three inert cycles were performed by exposing the particles alternatingly to 100% N2 and 5% O2 at 900°C. By measuring the oxygen concentration during such inert cycles, the oxygen carriers CLOU property could be examined. Subsequently, the particles were exposed to three methane cycles and three syngas (50% CO and 50% H2) cycles at 950°C. Then, three more inert cycles were carried out at 900°C. Afterwards, one 1800 s inert cycle was performed at 1000°C to calculate the materials’ oxygen capacity with respect to CLOU. Finally, the oxygen carriers were cooled down to room temperature during fluidization with 5% O2. The gas flows applied were 900 mLN/min for 5% O2 (in N2), 600 mLN/min for N2, and 450 mLN/min for CH4 and syngas. These flows correspond to 8–28 umf in the oxidation period and 3–9 umf in the reduction period. The experimental procedure, with the injection time for N2 and fuel, is stated in Table 2 for different cycles. N2 was used to flush the reactor for 60 s before and after fuel introduction to prevent back mixing.Table 2
Experimental scheme for oxygen carriers’ reactivity test.
No. of cycles
Inert/reducing gas
t
CLOU
t
In
t
Red
T
Ox
T
Red/TCLOU
(s)
(s)
(s)
(°C)
(°C)
3
Nitrogena
360
900
900
3
Methane
60
20
950
950
3
Syngas
60
80
950
950
3
Nitrogen
360
900
900
1
Nitrogen
1800
900
1000
aThe oxygen concentration was measured during the inert periods in order to evaluate the ability of the oxygen carriers’ to release oxygen in the gas phase.


## 3.4.2. Temperature Influence on Oxygen Carriers’ Reactivity

The effect of temperature on the performance of oxygen carrier was studied by conducting cyclic reactivity tests in the batch fluidized reactor. As can be seen from Table3, the experiments started at 900°C followed by cycles at 950°C, 1000°C, and 1050°C. Finally, the temperature was reduced to 950°C. The last test was made in order to judge if the redox cycles at higher temperatures had any permanent effect on the particle reactivity behavior. At each temperature, two methane reduction cycles and two inert cycles were carried out, as seen in the table. As before, 15 g of fresh sample was used in this series of tests. After the cycles the material was cooled down to room temperature in 600 mLN/min 100% N2. Gas flows were the same as those used for the experiments described in Section 3.4.1.Table 3
Experimental scheme used for investigation of the effect of temperature on the oxygen carrier reactivity.
No. of cycles
Inert/reducing gas
t
CLOU
t
In
t
Red
T
Ox
T
Red/TCLOU
(s)
(s)
(s)
(°C)
(°C)
2
Methane
60
20
900
900
2
Nitrogen
360
900
900
2
Methane
60
20
950
950
2
Nitrogen
360
950
950
2
Methane
60
20
1000
1000
2
Nitrogen
360
1000
1000
2
Methane
60
20
1050
1050
2
Nitrogen
360
1050
1050
2
Methane
60
20
950
950
2
Nitrogen
360
950
950


## 3.4.3. Investigation of Reactivity Stability and Reduction Time

The reactivity over many redox cycles was also investigated in this work. A sample of 2 g of CaMn0.8Mg0.2O3 sintered at 1300°C (short for 5.6% MgO 1300) which had previously been used in general reactivity screening was placed in the quartz reactor. The particles were exposed alternatingly to 10% O2 in N2, 100% N2 and pure CH4. The inlet flows were 900 mLN/min for all components. As seen in Table 4, two sets of experiments were done, with the methane injection period set to 2 s and 14 s, respectively, for the different experiments. A total of 50 cycles were conducted for each experiment.Table 4
Experimental scheme for stability tests.
Sample batch
No. of cycles
Reducing gas
t
In
t
Red
T
Ox
T
Red
(s)
(s)
(°C)
(°C)
1
50
Methane
60
2
950
950
2
50
Methane
60
14
950
950


## 3.5. Data Evaluation

Fuel conversion, or fuel yield, is defined as a degree of how much introduced fuel has been fully converted into CO2. It is used to quantify an oxygen carrier’s reactivity towards fuels. Methane and syngas conversion are presented as (6) showing the CH4 and CO conversion to CO2 respectively
(6)γCH4=pCO2pCO2+pCO+pCH4,γsyn=pCO2pCO2+pCO,
where pi is the outlet partial pressure of component i.Oxygen carrier conversion (or solid conversion) is defined as(7)ωi=mimox,
where mi is the mass of the oxygen carrier at time i and mox is the mass of the fully oxidized oxygen carrier. Here, mox is simply the mass of the fresh particles used in the experiments, and no account has been taken to the possible oxygen deficiency at higher temperatures [29]. In a fuel reduction period, ωi can also be calculated as a function of time. Equation (8) shows the oxygen carrier conversion during a methane and syngas reduction period, respectively, as follows:
(8)ωi=ωi-1-∫ti-1tin˙outMomoxPtot(4pCO2,out+3pCO,out-pH2,out)dt,ωi=ωi-1-∫ti-1tin˙outMomoxPtot(2pCO2,out+pCO,out-pH2,out)dt,
where n˙out is the molar flux of flue gas after water condensation and Mo is the molar mass of oxygen. For a specific reduction cycle, γCH4, is sometimes given as an average value from ω=1 to 0.99. The concentration of H2 was not measured during experiments. H2 concentration can be assumed to be low enough to be neglected since H2 generally has a higher reactivity than CO [39] and the CO concentration was very low under all conditions.


## 4. Results

### 4.1. Crushing Strength and Effective Density

The crushing strengths and effective densities of the calcium manganite oxygen carriers are presented in Table5. Effective density is calculated from measurement of the volume and mass of a small bed of particles. By assuming a void fraction of 0.37, the effective density can be calculated as
(9)Effectivedensity=msolidsVsolids*(1-0.37).
Figure 3 shows the crushing strength and effective density versus sintering temperature. Obviously, particles sintered at higher temperature are denser and have higher mechanical strength. Oxygen carriers with higher crushing strength are likely preferred in CLC since it may indicate a reasonable resistance against attrition and fragmentation. But particles with high density may be more prone to defluidization, especially at low velocities. The crushing strengths of the samples sintered at 1100°C were judged to be too low, and these samples were excluded from batch reactor testing.Table 5
Crushing strength and effective density of MgO added CaMnO3-δ materials.
Notation
Molar composition
Sintering temperature
Crushing strength
Effective  density
(°C)
(N)
(kg/m3)
5.6% MgO
CaMn0.8Mg0.2O3
1100
0.4
1001.2
1200
0.7
1238.7
1300
1.3
1704.9
2.7% MgO
CaMn0.9Mg0.1O3
1100
0.3
1041.3
1200
0.6
1437.6
1300
1.4
2254.6Crushing strength (a) and effective density (b) as a function of sintering temperature for all investigated particles.
(a)
(b)


### 4.2. General Screening of Oxygen Carriers’ Reactivity

#### 4.2.1. CLOU Property at 900°C and 1000°C

The ability of oxygen carrier particles to release oxygen in the gas phase, or the so-called oxygen uncoupling properties, was investigated by exposing the particles to inert periods both before and after fuel cycles; see Table2. By gauging the difference in oxygen uncoupling properties from before and after fuel testing, it is possible to see if the particles become deactivated during the exposure to fuel. Figure 4(a) shows the oxygen concentration profile of 7 inert cycles tested at 900°C on the sample with 5.6% MgO, sintered at 1300°C. Here, 3 cycles are conducted before exposure to fuel (solid lines), 3 cycles are taken after exposure to fuel (dashed lines), and 1 blank reference cycle is included. In the reference, 15 g of inert silica sand was used in the bed, and the air was switched to inert in the same way as when the oxygen carrier particles were bed material. Of course, no uncoupling properties are expected from this reference experiment.O2 concentration profile in inert cycles. Tests were carried out on the 5.6% MgO 1300 sample. (a) inert cycles at 900°C; (b) 1800 s inert cycle at 1000°C. For the experiments in Figure 4(a), three cycles were conducted before and following the fuel cycles. In Figure 4(b), the oxidation was performed at 900°C
(a)
(b)Att=0 s in Figure 4(a), 100% N2 was injected to the system instead of 5% O2. Due to a delay in the measuring system, oxygen concentration stays at 5% for the first 20 s. For a material without CLOU property, for instance, the sand reference, the oxygen concentration drops sharply to 0 as shown by the reference plot. On the other hand, the sample, 5.6% MgO 1300, releases gaseous oxygen yielding the smooth gradually decreased oxygen concentration. It can be seen from the figures that the materials exhibit stable uncoupling properties as a function of time for the first three cycles. The reactivity is somewhat less after the fuel cycles, but in general there seems to be very little deactivation caused by the exposure to fuel. The amount of oxygen removed by the uncoupling reactions after 360 s corresponded to approximately 0.5 wt% of the total mass of oxygen carrier.To be able to calculate the oxygen uncoupling capacity of the oxygen carrier particles, one 1800 s inert cycle was performed at 1000°C. Here, the oxidation was carried out at 900°C, but the temperature was increased to 1000°C during the oxidation. Figure4(b) presents the oxygen concentration profile of the 1800 s inert cycle performed on 5.6% MgO 1300 sample. The small peak at around t=175 s resulted from the temperature increase to 1000°C. At the end of the cycle, the concentration of uncoupled oxygen was almost zero indicating that little oxygen was available for CLOU. By integrating the concentration difference between blank reference and tested sample, the material’s CLOU oxygen capacity is estimated to about 1 wt%.Table6 summarizes the data for the CLOU experiments at 900°C. Here, the concentration of O2 after 360 s is given, averaged for the three cycles before and after fuel cycles. Clearly, there is a decreased CLOU activity following the fuel cycles. For the 5.6% MgO 1200 sample, the O2 concentration after the fuel cycles dropped 0.1%-unit compared with the concentration before fuel cycles. This may be due to some physical or chemical deactivation in the fuel cycles; for instance, it is possible that other phases besides the calcium manganite is formed during the reduction, for instance, CaMn2O4 or Ca2MnO4, which could affect the reactivity [32].Table 6
Oxygen concentration at the end of the CLOU period for tested oxygen carrier particles.
Notation
Molar composition
Sintering temperature
Conc. (O2) end of inert  (T = 900°C)
(°C)
Before fuel
After fuel
(%)
(%)
5.6% MgO
CaMn0.8Mg0.2O3
1200
0.5
0.1
1300
0.4
0.3
2.7% MgO
CaMn0.9Mg0.1O3
1200
0.5
0.3
1300
0.5
0.4


#### 4.2.2. Reactivity of Oxygen Carriers towards Fuels at 950°C

All investigated oxygen carriers exhibited high reactivity towards gaseous fuels. Methane conversion of over 97% and full conversion of syngas were achieved for all samples. Figure5 shows the dry flue gas concentration profile of the second methane cycle at 950°C performed on sample 5.6% MgO 1300. At t=0 s, 5% O2 was switched off and N2 was injected for 60 s. The O2 concentration in the reactor drops immediately after around t=20 s, a lag time which is due to the system delay, however remaining at around 1.5% at the end of inert step resulting from the CLOU behavior of the oxygen carrier. At t=60 s, the N2 flow was turned off and methane was switched on for 20 s. Inlet methane was immediately converted to CO2, and the high reactivity of the material gives a high and sharp CO2 peak. In Figure 5, the breakthrough of CO2 does not come until about t=80 s, once again due to the time delay in the system. Flushing of N2 is seen at t=100 s in Figure 5, after which the concentrations of detected gaseous species decrease to zero rapidly.Figure 5
Dry gas concentration profile of the second methane cycle at 950°C on the 5.6% MgO 1300 sample.Figure6 presents the methane yield versus solid conversion for all 4 samples. The second methane reduction cycle was selected for comparison. At the beginning of reduction, injected methane was fully converted into CO2 giving full conversion for all samples. As reduction proceeds, less oxygen becomes available in the oxygen carrier. So the material becomes less reactive, which is logical considering that the equilibrium partial pressure of O2 becomes less at higher degrees of reduction, and thus likely also the release rate. Since less oxygen is available for methane conversion, this may be the reason of the increased methane concentration from t=90 s to t=100 s in Figure 5. This leads to the slightly decrease of methane conversion at the end of the reduction. Still the material has very high reactivity throughout the reduction period, exceeding 97% in the ω range 1 to 0.99.Figure 6
Methane yield as a function of solid conversion of the second methane cycle at 950°C.Figures7 and 8 demonstrate the dry gas concentration profile and syngas yield as a function of solid conversion for tested samples. Syngas consisting 50% CO and 50% H2 is apparently easier to oxidize, as compared with methane. Another factor is the fact that syngas needs less oxygen per mole fuel in order to be converted to CO2 and H2O. So there was complete syngas conversion, that is, for ω from 1 to 0.99, for all samples.Figure 7
Dry gas concentration profile of the second syngas cycle at 950°C for the 5.6% MgO 1300 sample.Figure 8
Syngas yield as a function of solid conversion for the second syngas cycle at 950°C.


### 4.3. Influence of Temperature on the Reactivity of the Oxygen Carriers

The methane yield as a function of solid conversion at different temperatures is presented in Figure9 for the particles 5.6% MgO 1300. In Figure 9(b), which compares the reactivity at 950°C, before and after testing at 1050°C, “1” indicates the temperature before 1050°C cycles, and “2” represents the temperature after the 1050°C cycles. Decrease of the methane yield as a function of decreasing omega indicates that less methane was converted when the oxygen carrier was further reduced. Figure 10 summarizes the average methane yield at different temperatures for all samples along the temperature stair described in Section  3.4.2, with the exception of the last cycles at 950°C (2). The average γCH4 is an average value of methane conversions of two reduction cycles operated at the same temperature.The methane yield as a function of solids conversion for 20 s reduction of 5.6% MgO 1300 oxygen carrier; (a) methane yield versus solid conversion for different temperatures and (b) the comparison of methane conversions at 950°C before and after 1050°C cycles. Data obtained from the second cycle is presented.
(a)
(b)Figure 10
The average methane yield of 5.6% MgO and 2.7% MgO oxygen carriers as a function of temperature (data was selected forω from 1 to 0.99). The single dots separated from the lines present the results at 950°C (2) cycles.The effect of temperature on the oxygen carriers’ reactivity is clearly seen in the figures, especially from 900°C to 950°C. At 950°C, methane conversion of all the samples is already around 99%, making it hard to see the effect of further temperature change. The methane yield at 1000°C is a little bit lower than 950°C for the oxygen carrier 5.6% MgO 1300, but the difference is very small. Although high temperature improves methane conversion, it may cause deactivation in the oxygen carriers’ reactivity. This was examined by comparing the reactivity at 950°C, before (1), and after (2) testing at the maximum temperature; see Figure9(b). The particles reactivity at 950°C (1) (dashed and dotted lines) is apparently somewhat higher than the reactivity after the high temperature cycles (the dashed line). This indicates that materials suffer some deactivation, likely caused during the high temperature cycles. Some deactivation was seen for all investigated samples, as seen in Figure 10.The ability of the oxygen carrier particles to release oxygen in the gas phase was also investigated at different temperatures. The results of the materials CLOU properties are summarized in Figures11 and 12. The oxygen concentration profile presented in Figure 11 was similar to the other tested samples, with only small variations. For each inert cycle, the oxygen concentration at the end of 360 s was collected and shown as a function of temperature in Figure 12 for each investigated material.The O2 concentration profile of inert cycles for the 5.6% MgO 1300 oxygen carrier; (a) oxygen concentration versus time as a function of temperature and (b) the comparison of oxygen profiles at 950°C before and after 1050°C cycles. Data obtained from the second conducted cycle is presented.
(a)
(b)Figure 12
Released gaseous oxygen concentrations at the end of 360 s inert cycles by 5.6% MgO and 2.7% MgO oxygen carriers at different temperatures. The single dots separated from the lines present the results at 950°C (2) cycles.As can be seen, operational temperature does not influence the materials CLOU properties in a significant way, although the particles release somewhat more oxygen as a function of temperature in the interval between 900°C and 950°C, and there is a drop at the highest temperature of 1050°C for all materials. The lower concentration of oxygen release for the 5.6% MgO 1300 sample at 950°C (2) cycles compared with the one at 950°C (1) indicates some deactivation of the material; see Figure11(b). This was seen for all investigated particles; see Figure 12. The samples containing less MgO releases a little bit more oxygen at temperatures lower than 1050°C. The lower degree of oxygen release at the higher temperatures may be explained by the fact that the material is oxidized to a lesser extent at the higher temperatures [29, 31], meaning that the (3-δ) in reaction (5) decreases. This means that the oxygen capacity for the uncoupling reactions may decrease. The lower degree of oxygen release could also due to the formation of spinel, such as CaMn2O4, see discussion for further information.


### 4.4. Stability of Oxygen Carriers’ Reactivity

To study the stability of the oxygen carrier, 50 short reduction cycles with methane were performed on 5.6% MgO 1300 particles. The reduction period was set to 2 s and 14 s to investigate the effect of reduction period length on the oxygen carriers’ activity. Figure13 shows the average methane conversion for 50 cycles at an operation temperature of 950°C. In both 2 s reduction and 14 s reduction tests, the material’s reactivity maintained well during 50 cycles, and a slight growth in reactivity is noticed. In stability test, less bed material (2 g) and higher methane flow (900 mLN/min) were applied. The low methane conversion, in the range of 20%–50%, compared with full methane conversion in Sections 4.2 and 4.3, is reasonable.Methane conversion, (γCH4) as a function of number of cycles for 5.6% MgO 1300 oxygen carrier.
(a)
2 s reduction
(b)
14 s reduction


### 4.5. Characterization of Oxygen Carriers

The morphology of 5.6% MgO 1300 particles was investigated by light microscopy and SEM. Figure14 shows the light microscope pictures of fresh and used samples after 50 cycles. In Figure 14, the blue grids are 1 mm squares of the background millimeter paper. The images marked with (a) are fresh particles. The pictures marked with (b) and (c) exhibit the particles exposed to 2 s and 14 s methane reduction, respectively. Comparing the size of the particles, one can find that the particles after 14 s reduction cycles are somewhat bigger than other samples, while the difference between fresh and particles used for 2 s reduction cycles was quite small. This result may suggest that the oxygen carriers expand when reacting with methane.Light microscope pictures of 5.6% MgO 1300 particles both fresh and used after 50 cycles. (a) fresh particles; (b) particles on which 50 cycles of 2 s reduction was performed; (c) particles on which 50 cycles of 14 s reduction was performed.
(a)
(b)
(c)The SEM pictures of fresh and used (after general reactivity test, cooled down in 5% O2) 5.6% MgO 1300 particles are shown in Figure 15. The material maintains good spherical shape after experiments under different conditions. The cracks on some of the particles seen in the pictures were likely caused during the manufacture since they were found on fresh particles and on used ones. No obvious dust formation was noticed during the experiments. On careful examination of the particle surface using energy-dispersive X-ray spectroscopy, it was discovered that there were many small heterogeneous inclusions on the surface which were identified as MgO. Hence, it does not appear that the MgO was included in the perovskite structure, rather the MgO seems to present mainly as a separate phase and in small grains.SEM image of 5.6% MgO 1300 sample. (a) Fresh sample. (b) Used sample (cooled down to room temperature by 5% O2 in N2).
(a)
(b)The crystalline phases of the oxygen carriers are summarized in Table7. Images were taken for fresh samples, used samples which were finished after inert cycle at 1000°C and cooled in 5% O2, and used samples after reduction at 950°C and cooled in pure N2. The phases for the used samples which were cooled in N2 after the temperature stair were difficult to interpret due to low peak intensities of the XRD peaks. The crystalline phases are thus not provided for these samples. In the fresh samples, CaMnO3-δ and MgO were identified in all samples. The multiple phases characterized match the EDX results, where free MgO was identified on the oxygen carrier particle surface. This confirms that MgO was not incorporated into the perovskite structure and hence the oxygen carriers consist of separated CaMnO3-δ and MgO phases. In most cases, the same crystalline phases were identified in fresh particles and particles after tests which were removed after oxidation. This suggests that these CaMnO3-δ materials have a good stability in the CLC process. The minor phase CaMn2O4 identified in used 5.6% MgO 1200 sample was reported as a decomposition product of CaMnO3-δ at lower oxygen deficiency values [32]. Formation of a small amount of CaMn2O4 after the reactivity test could be reasonable considering the sample had been reduced with both methane and syngas. During preparation of the oxygen carrier particles, the molar ratio of calcium and manganese is higher than one. However, CaMnO3-δ is the only XRD detected phase containing Ca and Mn. This means that the oxygen carriers should contain other calcium phases, such as CaO or Ca2MnO4-δ, which were not identified by XRD. The reason could be that the amounts of other calcium phases are too low (<5 wt%) to be detected with the used apparatus; see below for further discussion.Table 7
Crystalline phases identified in investigated samples.
Sample
Sintering temperature
Fresh
Used (cooled in 5%O2)
5.6% MgO
1200°C
CaMnO
2.97, MgO
CaMnO2.98, CaMn2O4, MgO
1300°C
CaMnO
2.95, MgO
CaMnO2.95, MgO
2.7% MgO
1200°C
CaMnO
2.95,  MgO
CaMnO2.95, MgO
1300°C
CaMnO
2.95, MgO
CaMnO2.95, MgO


## 4.1. Crushing Strength and Effective Density

The crushing strengths and effective densities of the calcium manganite oxygen carriers are presented in Table5. Effective density is calculated from measurement of the volume and mass of a small bed of particles. By assuming a void fraction of 0.37, the effective density can be calculated as
(9)Effectivedensity=msolidsVsolids*(1-0.37).
Figure 3 shows the crushing strength and effective density versus sintering temperature. Obviously, particles sintered at higher temperature are denser and have higher mechanical strength. Oxygen carriers with higher crushing strength are likely preferred in CLC since it may indicate a reasonable resistance against attrition and fragmentation. But particles with high density may be more prone to defluidization, especially at low velocities. The crushing strengths of the samples sintered at 1100°C were judged to be too low, and these samples were excluded from batch reactor testing.Table 5
Crushing strength and effective density of MgO added CaMnO3-δ materials.
Notation
Molar composition
Sintering temperature
Crushing strength
Effective  density
(°C)
(N)
(kg/m3)
5.6% MgO
CaMn0.8Mg0.2O3
1100
0.4
1001.2
1200
0.7
1238.7
1300
1.3
1704.9
2.7% MgO
CaMn0.9Mg0.1O3
1100
0.3
1041.3
1200
0.6
1437.6
1300
1.4
2254.6Crushing strength (a) and effective density (b) as a function of sintering temperature for all investigated particles.
(a)
(b)


## 4.2. General Screening of Oxygen Carriers’ Reactivity

### 4.2.1. CLOU Property at 900°C and 1000°C

The ability of oxygen carrier particles to release oxygen in the gas phase, or the so-called oxygen uncoupling properties, was investigated by exposing the particles to inert periods both before and after fuel cycles; see Table2. By gauging the difference in oxygen uncoupling properties from before and after fuel testing, it is possible to see if the particles become deactivated during the exposure to fuel. Figure 4(a) shows the oxygen concentration profile of 7 inert cycles tested at 900°C on the sample with 5.6% MgO, sintered at 1300°C. Here, 3 cycles are conducted before exposure to fuel (solid lines), 3 cycles are taken after exposure to fuel (dashed lines), and 1 blank reference cycle is included. In the reference, 15 g of inert silica sand was used in the bed, and the air was switched to inert in the same way as when the oxygen carrier particles were bed material. Of course, no uncoupling properties are expected from this reference experiment.O2 concentration profile in inert cycles. Tests were carried out on the 5.6% MgO 1300 sample. (a) inert cycles at 900°C; (b) 1800 s inert cycle at 1000°C. For the experiments in Figure 4(a), three cycles were conducted before and following the fuel cycles. In Figure 4(b), the oxidation was performed at 900°C
(a)
(b)Att=0 s in Figure 4(a), 100% N2 was injected to the system instead of 5% O2. Due to a delay in the measuring system, oxygen concentration stays at 5% for the first 20 s. For a material without CLOU property, for instance, the sand reference, the oxygen concentration drops sharply to 0 as shown by the reference plot. On the other hand, the sample, 5.6% MgO 1300, releases gaseous oxygen yielding the smooth gradually decreased oxygen concentration. It can be seen from the figures that the materials exhibit stable uncoupling properties as a function of time for the first three cycles. The reactivity is somewhat less after the fuel cycles, but in general there seems to be very little deactivation caused by the exposure to fuel. The amount of oxygen removed by the uncoupling reactions after 360 s corresponded to approximately 0.5 wt% of the total mass of oxygen carrier.To be able to calculate the oxygen uncoupling capacity of the oxygen carrier particles, one 1800 s inert cycle was performed at 1000°C. Here, the oxidation was carried out at 900°C, but the temperature was increased to 1000°C during the oxidation. Figure4(b) presents the oxygen concentration profile of the 1800 s inert cycle performed on 5.6% MgO 1300 sample. The small peak at around t=175 s resulted from the temperature increase to 1000°C. At the end of the cycle, the concentration of uncoupled oxygen was almost zero indicating that little oxygen was available for CLOU. By integrating the concentration difference between blank reference and tested sample, the material’s CLOU oxygen capacity is estimated to about 1 wt%.Table6 summarizes the data for the CLOU experiments at 900°C. Here, the concentration of O2 after 360 s is given, averaged for the three cycles before and after fuel cycles. Clearly, there is a decreased CLOU activity following the fuel cycles. For the 5.6% MgO 1200 sample, the O2 concentration after the fuel cycles dropped 0.1%-unit compared with the concentration before fuel cycles. This may be due to some physical or chemical deactivation in the fuel cycles; for instance, it is possible that other phases besides the calcium manganite is formed during the reduction, for instance, CaMn2O4 or Ca2MnO4, which could affect the reactivity [32].Table 6
Oxygen concentration at the end of the CLOU period for tested oxygen carrier particles.
Notation
Molar composition
Sintering temperature
Conc. (O2) end of inert  (T = 900°C)
(°C)
Before fuel
After fuel
(%)
(%)
5.6% MgO
CaMn0.8Mg0.2O3
1200
0.5
0.1
1300
0.4
0.3
2.7% MgO
CaMn0.9Mg0.1O3
1200
0.5
0.3
1300
0.5
0.4


### 4.2.2. Reactivity of Oxygen Carriers towards Fuels at 950°C

All investigated oxygen carriers exhibited high reactivity towards gaseous fuels. Methane conversion of over 97% and full conversion of syngas were achieved for all samples. Figure5 shows the dry flue gas concentration profile of the second methane cycle at 950°C performed on sample 5.6% MgO 1300. At t=0 s, 5% O2 was switched off and N2 was injected for 60 s. The O2 concentration in the reactor drops immediately after around t=20 s, a lag time which is due to the system delay, however remaining at around 1.5% at the end of inert step resulting from the CLOU behavior of the oxygen carrier. At t=60 s, the N2 flow was turned off and methane was switched on for 20 s. Inlet methane was immediately converted to CO2, and the high reactivity of the material gives a high and sharp CO2 peak. In Figure 5, the breakthrough of CO2 does not come until about t=80 s, once again due to the time delay in the system. Flushing of N2 is seen at t=100 s in Figure 5, after which the concentrations of detected gaseous species decrease to zero rapidly.Figure 5
Dry gas concentration profile of the second methane cycle at 950°C on the 5.6% MgO 1300 sample.Figure6 presents the methane yield versus solid conversion for all 4 samples. The second methane reduction cycle was selected for comparison. At the beginning of reduction, injected methane was fully converted into CO2 giving full conversion for all samples. As reduction proceeds, less oxygen becomes available in the oxygen carrier. So the material becomes less reactive, which is logical considering that the equilibrium partial pressure of O2 becomes less at higher degrees of reduction, and thus likely also the release rate. Since less oxygen is available for methane conversion, this may be the reason of the increased methane concentration from t=90 s to t=100 s in Figure 5. This leads to the slightly decrease of methane conversion at the end of the reduction. Still the material has very high reactivity throughout the reduction period, exceeding 97% in the ω range 1 to 0.99.Figure 6
Methane yield as a function of solid conversion of the second methane cycle at 950°C.Figures7 and 8 demonstrate the dry gas concentration profile and syngas yield as a function of solid conversion for tested samples. Syngas consisting 50% CO and 50% H2 is apparently easier to oxidize, as compared with methane. Another factor is the fact that syngas needs less oxygen per mole fuel in order to be converted to CO2 and H2O. So there was complete syngas conversion, that is, for ω from 1 to 0.99, for all samples.Figure 7
Dry gas concentration profile of the second syngas cycle at 950°C for the 5.6% MgO 1300 sample.Figure 8
Syngas yield as a function of solid conversion for the second syngas cycle at 950°C.


## 4.2.1. CLOU Property at 900°C and 1000°C

The ability of oxygen carrier particles to release oxygen in the gas phase, or the so-called oxygen uncoupling properties, was investigated by exposing the particles to inert periods both before and after fuel cycles; see Table2. By gauging the difference in oxygen uncoupling properties from before and after fuel testing, it is possible to see if the particles become deactivated during the exposure to fuel. Figure 4(a) shows the oxygen concentration profile of 7 inert cycles tested at 900°C on the sample with 5.6% MgO, sintered at 1300°C. Here, 3 cycles are conducted before exposure to fuel (solid lines), 3 cycles are taken after exposure to fuel (dashed lines), and 1 blank reference cycle is included. In the reference, 15 g of inert silica sand was used in the bed, and the air was switched to inert in the same way as when the oxygen carrier particles were bed material. Of course, no uncoupling properties are expected from this reference experiment.O2 concentration profile in inert cycles. Tests were carried out on the 5.6% MgO 1300 sample. (a) inert cycles at 900°C; (b) 1800 s inert cycle at 1000°C. For the experiments in Figure 4(a), three cycles were conducted before and following the fuel cycles. In Figure 4(b), the oxidation was performed at 900°C
(a)
(b)Att=0 s in Figure 4(a), 100% N2 was injected to the system instead of 5% O2. Due to a delay in the measuring system, oxygen concentration stays at 5% for the first 20 s. For a material without CLOU property, for instance, the sand reference, the oxygen concentration drops sharply to 0 as shown by the reference plot. On the other hand, the sample, 5.6% MgO 1300, releases gaseous oxygen yielding the smooth gradually decreased oxygen concentration. It can be seen from the figures that the materials exhibit stable uncoupling properties as a function of time for the first three cycles. The reactivity is somewhat less after the fuel cycles, but in general there seems to be very little deactivation caused by the exposure to fuel. The amount of oxygen removed by the uncoupling reactions after 360 s corresponded to approximately 0.5 wt% of the total mass of oxygen carrier.To be able to calculate the oxygen uncoupling capacity of the oxygen carrier particles, one 1800 s inert cycle was performed at 1000°C. Here, the oxidation was carried out at 900°C, but the temperature was increased to 1000°C during the oxidation. Figure4(b) presents the oxygen concentration profile of the 1800 s inert cycle performed on 5.6% MgO 1300 sample. The small peak at around t=175 s resulted from the temperature increase to 1000°C. At the end of the cycle, the concentration of uncoupled oxygen was almost zero indicating that little oxygen was available for CLOU. By integrating the concentration difference between blank reference and tested sample, the material’s CLOU oxygen capacity is estimated to about 1 wt%.Table6 summarizes the data for the CLOU experiments at 900°C. Here, the concentration of O2 after 360 s is given, averaged for the three cycles before and after fuel cycles. Clearly, there is a decreased CLOU activity following the fuel cycles. For the 5.6% MgO 1200 sample, the O2 concentration after the fuel cycles dropped 0.1%-unit compared with the concentration before fuel cycles. This may be due to some physical or chemical deactivation in the fuel cycles; for instance, it is possible that other phases besides the calcium manganite is formed during the reduction, for instance, CaMn2O4 or Ca2MnO4, which could affect the reactivity [32].Table 6
Oxygen concentration at the end of the CLOU period for tested oxygen carrier particles.
Notation
Molar composition
Sintering temperature
Conc. (O2) end of inert  (T = 900°C)
(°C)
Before fuel
After fuel
(%)
(%)
5.6% MgO
CaMn0.8Mg0.2O3
1200
0.5
0.1
1300
0.4
0.3
2.7% MgO
CaMn0.9Mg0.1O3
1200
0.5
0.3
1300
0.5
0.4


## 4.2.2. Reactivity of Oxygen Carriers towards Fuels at 950°C

All investigated oxygen carriers exhibited high reactivity towards gaseous fuels. Methane conversion of over 97% and full conversion of syngas were achieved for all samples. Figure5 shows the dry flue gas concentration profile of the second methane cycle at 950°C performed on sample 5.6% MgO 1300. At t=0 s, 5% O2 was switched off and N2 was injected for 60 s. The O2 concentration in the reactor drops immediately after around t=20 s, a lag time which is due to the system delay, however remaining at around 1.5% at the end of inert step resulting from the CLOU behavior of the oxygen carrier. At t=60 s, the N2 flow was turned off and methane was switched on for 20 s. Inlet methane was immediately converted to CO2, and the high reactivity of the material gives a high and sharp CO2 peak. In Figure 5, the breakthrough of CO2 does not come until about t=80 s, once again due to the time delay in the system. Flushing of N2 is seen at t=100 s in Figure 5, after which the concentrations of detected gaseous species decrease to zero rapidly.Figure 5
Dry gas concentration profile of the second methane cycle at 950°C on the 5.6% MgO 1300 sample.Figure6 presents the methane yield versus solid conversion for all 4 samples. The second methane reduction cycle was selected for comparison. At the beginning of reduction, injected methane was fully converted into CO2 giving full conversion for all samples. As reduction proceeds, less oxygen becomes available in the oxygen carrier. So the material becomes less reactive, which is logical considering that the equilibrium partial pressure of O2 becomes less at higher degrees of reduction, and thus likely also the release rate. Since less oxygen is available for methane conversion, this may be the reason of the increased methane concentration from t=90 s to t=100 s in Figure 5. This leads to the slightly decrease of methane conversion at the end of the reduction. Still the material has very high reactivity throughout the reduction period, exceeding 97% in the ω range 1 to 0.99.Figure 6
Methane yield as a function of solid conversion of the second methane cycle at 950°C.Figures7 and 8 demonstrate the dry gas concentration profile and syngas yield as a function of solid conversion for tested samples. Syngas consisting 50% CO and 50% H2 is apparently easier to oxidize, as compared with methane. Another factor is the fact that syngas needs less oxygen per mole fuel in order to be converted to CO2 and H2O. So there was complete syngas conversion, that is, for ω from 1 to 0.99, for all samples.Figure 7
Dry gas concentration profile of the second syngas cycle at 950°C for the 5.6% MgO 1300 sample.Figure 8
Syngas yield as a function of solid conversion for the second syngas cycle at 950°C.


## 4.3. Influence of Temperature on the Reactivity of the Oxygen Carriers

The methane yield as a function of solid conversion at different temperatures is presented in Figure9 for the particles 5.6% MgO 1300. In Figure 9(b), which compares the reactivity at 950°C, before and after testing at 1050°C, “1” indicates the temperature before 1050°C cycles, and “2” represents the temperature after the 1050°C cycles. Decrease of the methane yield as a function of decreasing omega indicates that less methane was converted when the oxygen carrier was further reduced. Figure 10 summarizes the average methane yield at different temperatures for all samples along the temperature stair described in Section  3.4.2, with the exception of the last cycles at 950°C (2). The average γCH4 is an average value of methane conversions of two reduction cycles operated at the same temperature.The methane yield as a function of solids conversion for 20 s reduction of 5.6% MgO 1300 oxygen carrier; (a) methane yield versus solid conversion for different temperatures and (b) the comparison of methane conversions at 950°C before and after 1050°C cycles. Data obtained from the second cycle is presented.
(a)
(b)Figure 10
The average methane yield of 5.6% MgO and 2.7% MgO oxygen carriers as a function of temperature (data was selected forω from 1 to 0.99). The single dots separated from the lines present the results at 950°C (2) cycles.The effect of temperature on the oxygen carriers’ reactivity is clearly seen in the figures, especially from 900°C to 950°C. At 950°C, methane conversion of all the samples is already around 99%, making it hard to see the effect of further temperature change. The methane yield at 1000°C is a little bit lower than 950°C for the oxygen carrier 5.6% MgO 1300, but the difference is very small. Although high temperature improves methane conversion, it may cause deactivation in the oxygen carriers’ reactivity. This was examined by comparing the reactivity at 950°C, before (1), and after (2) testing at the maximum temperature; see Figure9(b). The particles reactivity at 950°C (1) (dashed and dotted lines) is apparently somewhat higher than the reactivity after the high temperature cycles (the dashed line). This indicates that materials suffer some deactivation, likely caused during the high temperature cycles. Some deactivation was seen for all investigated samples, as seen in Figure 10.The ability of the oxygen carrier particles to release oxygen in the gas phase was also investigated at different temperatures. The results of the materials CLOU properties are summarized in Figures11 and 12. The oxygen concentration profile presented in Figure 11 was similar to the other tested samples, with only small variations. For each inert cycle, the oxygen concentration at the end of 360 s was collected and shown as a function of temperature in Figure 12 for each investigated material.The O2 concentration profile of inert cycles for the 5.6% MgO 1300 oxygen carrier; (a) oxygen concentration versus time as a function of temperature and (b) the comparison of oxygen profiles at 950°C before and after 1050°C cycles. Data obtained from the second conducted cycle is presented.
(a)
(b)Figure 12
Released gaseous oxygen concentrations at the end of 360 s inert cycles by 5.6% MgO and 2.7% MgO oxygen carriers at different temperatures. The single dots separated from the lines present the results at 950°C (2) cycles.As can be seen, operational temperature does not influence the materials CLOU properties in a significant way, although the particles release somewhat more oxygen as a function of temperature in the interval between 900°C and 950°C, and there is a drop at the highest temperature of 1050°C for all materials. The lower concentration of oxygen release for the 5.6% MgO 1300 sample at 950°C (2) cycles compared with the one at 950°C (1) indicates some deactivation of the material; see Figure11(b). This was seen for all investigated particles; see Figure 12. The samples containing less MgO releases a little bit more oxygen at temperatures lower than 1050°C. The lower degree of oxygen release at the higher temperatures may be explained by the fact that the material is oxidized to a lesser extent at the higher temperatures [29, 31], meaning that the (3-δ) in reaction (5) decreases. This means that the oxygen capacity for the uncoupling reactions may decrease. The lower degree of oxygen release could also due to the formation of spinel, such as CaMn2O4, see discussion for further information.


## 4.4. Stability of Oxygen Carriers’ Reactivity

To study the stability of the oxygen carrier, 50 short reduction cycles with methane were performed on 5.6% MgO 1300 particles. The reduction period was set to 2 s and 14 s to investigate the effect of reduction period length on the oxygen carriers’ activity. Figure13 shows the average methane conversion for 50 cycles at an operation temperature of 950°C. In both 2 s reduction and 14 s reduction tests, the material’s reactivity maintained well during 50 cycles, and a slight growth in reactivity is noticed. In stability test, less bed material (2 g) and higher methane flow (900 mLN/min) were applied. The low methane conversion, in the range of 20%–50%, compared with full methane conversion in Sections 4.2 and 4.3, is reasonable.Methane conversion, (γCH4) as a function of number of cycles for 5.6% MgO 1300 oxygen carrier.
(a)
2 s reduction
(b)
14 s reduction


## 4.5. Characterization of Oxygen Carriers

The morphology of 5.6% MgO 1300 particles was investigated by light microscopy and SEM. Figure14 shows the light microscope pictures of fresh and used samples after 50 cycles. In Figure 14, the blue grids are 1 mm squares of the background millimeter paper. The images marked with (a) are fresh particles. The pictures marked with (b) and (c) exhibit the particles exposed to 2 s and 14 s methane reduction, respectively. Comparing the size of the particles, one can find that the particles after 14 s reduction cycles are somewhat bigger than other samples, while the difference between fresh and particles used for 2 s reduction cycles was quite small. This result may suggest that the oxygen carriers expand when reacting with methane.Light microscope pictures of 5.6% MgO 1300 particles both fresh and used after 50 cycles. (a) fresh particles; (b) particles on which 50 cycles of 2 s reduction was performed; (c) particles on which 50 cycles of 14 s reduction was performed.
(a)
(b)
(c)The SEM pictures of fresh and used (after general reactivity test, cooled down in 5% O2) 5.6% MgO 1300 particles are shown in Figure 15. The material maintains good spherical shape after experiments under different conditions. The cracks on some of the particles seen in the pictures were likely caused during the manufacture since they were found on fresh particles and on used ones. No obvious dust formation was noticed during the experiments. On careful examination of the particle surface using energy-dispersive X-ray spectroscopy, it was discovered that there were many small heterogeneous inclusions on the surface which were identified as MgO. Hence, it does not appear that the MgO was included in the perovskite structure, rather the MgO seems to present mainly as a separate phase and in small grains.SEM image of 5.6% MgO 1300 sample. (a) Fresh sample. (b) Used sample (cooled down to room temperature by 5% O2 in N2).
(a)
(b)The crystalline phases of the oxygen carriers are summarized in Table7. Images were taken for fresh samples, used samples which were finished after inert cycle at 1000°C and cooled in 5% O2, and used samples after reduction at 950°C and cooled in pure N2. The phases for the used samples which were cooled in N2 after the temperature stair were difficult to interpret due to low peak intensities of the XRD peaks. The crystalline phases are thus not provided for these samples. In the fresh samples, CaMnO3-δ and MgO were identified in all samples. The multiple phases characterized match the EDX results, where free MgO was identified on the oxygen carrier particle surface. This confirms that MgO was not incorporated into the perovskite structure and hence the oxygen carriers consist of separated CaMnO3-δ and MgO phases. In most cases, the same crystalline phases were identified in fresh particles and particles after tests which were removed after oxidation. This suggests that these CaMnO3-δ materials have a good stability in the CLC process. The minor phase CaMn2O4 identified in used 5.6% MgO 1200 sample was reported as a decomposition product of CaMnO3-δ at lower oxygen deficiency values [32]. Formation of a small amount of CaMn2O4 after the reactivity test could be reasonable considering the sample had been reduced with both methane and syngas. During preparation of the oxygen carrier particles, the molar ratio of calcium and manganese is higher than one. However, CaMnO3-δ is the only XRD detected phase containing Ca and Mn. This means that the oxygen carriers should contain other calcium phases, such as CaO or Ca2MnO4-δ, which were not identified by XRD. The reason could be that the amounts of other calcium phases are too low (<5 wt%) to be detected with the used apparatus; see below for further discussion.Table 7
Crystalline phases identified in investigated samples.
Sample
Sintering temperature
Fresh
Used (cooled in 5%O2)
5.6% MgO
1200°C
CaMnO
2.97, MgO
CaMnO2.98, CaMn2O4, MgO
1300°C
CaMnO
2.95, MgO
CaMnO2.95, MgO
2.7% MgO
1200°C
CaMnO
2.95,  MgO
CaMnO2.95, MgO
1300°C
CaMnO
2.95, MgO
CaMnO2.95, MgO


## 5. Discussion

The perovskite CaMnxMg1-xO3-δ studied in this work exhibited promising behavior with respect to parameters important for CLOU, that is, oxygen release, reactivity with methane, and syngas as well as fluidization properties. High reactivity towards methane in the range 93%–100% and full conversion of syngas were achieved at all examined temperatures. The particles have good fluidization properties, neither significant attrition nor agglomeration was observed. Though a slight deactivation was noticed following operation at 1050°C, the materials still worked quite well when the temperature was reduced.Previously, NiO has been the most promising oxygen carrier material for gas application [12, 37, 40]. Nevertheless, there are several problems with utilization of NiO as an oxygen carrier. Besides the high cost and toxicity, there is a thermodynamic limitation of the NiO/Ni system, which restricts methane to be fully converted to CO2 and H2O [11]. Several studies report around 1% CO in the exhausted stream from the fuel reactor when using NiO as an oxygen carrier [13, 14, 37].The studied calcium manganite oxygen carriers were produced from cheap raw materials Mn3O4, Ca(OH)2 and MgO using the commercial available spray-drying manufacturing method. As there are no thermodynamic limitation to convert fuel gas completely to CO2 and H2O, this type of material can clearly be a viable alternative to Ni-based material provided that the reactivity and stability are good. In this work, average methane conversion to CO2 and H2O of above 98% was achieved at temperatures of 950°C and above utilizing 57 kg/MW of CH4; see Figure 10. This is comparable to the reactivity seen at similar conditions using spray-dried Ni-based materials [37]. And unlike NiO, neither unconverted methane at the beginning of fuel injection, at high oxidation levels of the oxygen carrier, nor CO at the end of the reduction period was observed. In the Chalmers 10 kW continuous system, when using the CaMn0.9Mg0.1O3 as oxygen carrier, 100% methane was fully converted to CO2 and H2O above 900°C, and more than 1% O2 was detected in the outlet stream of the fuel reactor [36]. This suggests that gaseous reaction between O2 and CH4 is the main reaction mechanism in the fuel reactor. This is in contrast to NiO, which is a CLC material, meaning that the direct gas-solid reaction is the main mechanism for fuel conversion.The oxygen deficiencyδ in CaMnO3-δ is a function of oxygen partial pressure and temperature. Leonidova et al. [31] and Goldyreva et al. [41] studied the oxygen deficiency under different conditions and provided a phase diagram of CaMnO3-δ where δ was a function of oxygen partial pressure at different temperatures. At a fixed temperature, δ increases with decreasing oxygen partial pressure meaning that more oxygen is released under lower oxygen partial pressure environment. Conversely, at a constant partial pressure of oxygen, δ increases with temperature. This indicates that CaMnO3-δ oxygen carriers may not be oxidized to the same level at higher temperatures as it would be at lower temperatures. Despite this fact, the amount of oxygen that is available for CLOU depends on the δ difference between the oxidized and reduced form of CaMnO3-δ. Though oxidized CaMnO3-δ has less oxygen at higher temperature, it may be reduced further at low partial pressures of O2, as would be existing in the fuel reactor of a chemical-looping unit [31, 41]. For instance, for an oxygen partial pressure change, from 0.05 atm to 0.005 atm, the oxygen carrier CaMnO3-δ should release approximately the same amount of oxygen at higher and lower temperature cases employed in this work. This matches the experimental results well, where the oxygen carriers’ oxygen capacity seemed to be similar independent of temperature. On the other hand, the growth of oxygen carrier reactivity towards CH4 with temperature may due to an increase of oxygen release rate as a function of temperature.The level of oxygen deficiency of CaMnO3-δ cannot grow infinitely, and seems to be limited by the decomposition of CaMnO3-δ to CaMn2O4 and Ca2MnO4-δ [32]. The reported boundary 3-δ value was within the range of 2.863 to 2.83 for temperature interval 950°C to 1050°C. Beyond the boundary level, further removing of oxygen triggered the decomposition of CaMnO3-δ. However, this decomposition process was reversible and very slow even at 1000°C [32]. For CaMnO3-δ oxygen carriers applied in a CLC process where typical solid conversion changes could be around 1 wt%; this leads to the 3-δ value above 2.86, assuming fully oxidized sample from the air reactor. Hence, in order to avoid decomposition products and fully utilize the perovskites uncoupling properties, it may be a good idea to avoid deep reduction of the oxygen carrier in a real system and to keep the change in the mass based conversion level below 1% if possible. This could be achieved by employing high circulation of particles between the reactors. Another option to extract more oxygen from the material is to employ a lower temperature in the air reactor compared to the fuel reactor, something which should be feasible considering that the overall reactions should be exothermic in the fuel reactor [29]. The small amount of detected CaMn2O4 in the used 5.6% MgO 1200°C sample is likely due to the described decomposition process. It should be noted, however, that the identified phase had a very low intensity and is thus likely present in rather small amounts. Further, it is possible that also the other used samples contained this phase, but in undetectable quantities. Even in well controlled solid state chemistry synthesis processes, small amount of CaMn2O4 was also discovered as a secondary phase together with the CaMnO3-δ [42–44].The perovskite CaMnO3-δ can exist as different structures, depending upon temperature and partial pressure of oxygen. When heating in air, stoichiometry CaMnO3 with orthorhombic structure at room temperature lost oxygen forming the nonstoichiometric CaMnO3-δ and transforms to tetragonal and subsequently to cubic symmetry structure at 869°C and 913°C [31, 45–47]. This transition would happen at lower temperatures in our experiment since the particles were heated in 5% O2 in N2 under a much lower oxygen partial pressure compared to air. Such structure transitions involve changes of crystalline lattice parameters, although the compounds have the same chemical stoichiometry. During isothermal cycling in the fuel reactor at temperatures above 900°C, the cubic structure should be the most stable. However, it is possible that phase changes can occur during heating and cooling of the particles. In the current experiment, no degradation of particles was seen; so although there could have been certain structure transformations, as described above, these do not seem to have affected the physical integrity of the particles to any appreciable extent. In addition, the long-term testing in continuous operation of this type of particles without major attrition also suggests that possible degradation due to phase transformations should not be a major issue [36].For the investigated particles the moles of Ca is greater than the moles of Mn. However, only CaMnO3-δ and MgO were identified, meaning that Ca should be present in additional phases. The highly possible phases which contain Ca could be CaO or Ca2MnO4-δ. Horowitz and Longo suggested that CaO and CaMnO3 were the phases in Ca-Mn-O system at temperature below 1300°C when the Ca to Mn molar ratio was above 1, and the oxygen partial pressure 0.2 atm [48]. On the other hand, several research groups identified small amount of CaMn2O4 which coexited with CaMnO3-δ during synthesis of CaMnO3-δ when using stoichiometric molar amount of Ca and Mn during production. Since CaMn2O4 and Ca2MnO4-δ are the decomposition products of CaMnO3-δ [32], Ca2MnO4-δ may be present in the oxygen carrier particles as well, but in amounts too small to be detected by the present XRD unit. From characterization, it is clear that Mg is not incorporated into the perovskite structure, and this is likely due to the low ionic radii of Mg [49]. This is unlike the cations Fe and Ti, which can substitute Mn in the perovskite structure [50, 51]. Still, in a prior investigation, Hallberg et al. [35] clearly showed that the calcium manganite with Mg addition had better behavior with respect to CLOU than material doped with Fe and Ti. This suggests that MgO may be an active component in the oxidation reaction with methane; for instance, it may have a role as a reforming catalyst on the particle exterior. To clarify the role of MgO and CaMnO3-δ in methane conversion reaction, further investigation of the mechanism is apparently needed. On the other hand, considering the encouraging results reported here, by Hallberg et al. and Källén et al. in both batch and 10 kWth gas-fired CLC unit on the same type of material [35, 36], it is quite clear that this oxygen carrier is a valid alternative to NiO.


## 6. Conclusion

Cheap and environmentally friendly Ca-Mn combined oxide particles with general formulaCaMnxMg1-xO3 were produced using the spray-drying method. The active compound in the oxygen carriers was likely the perovskite material CaMnO3-δ, and it showed highly promising results with respect to reactivity and stability. Generally, the methane and syngas conversion was high, and the particles exhibited oxygen uncoupling at all investigated temperatures in the range 900–1050°C. There was some deactivation of the particles, especially prominent after exposure to fuel at high temperature, 1050°C. CaMn0.8Mg0.2O3 sintered at 1300°C showed good stability in 50 cycles’ tests, and even a small increase in reactivity was noted.



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*Source: 679560-2013-09-30.xml*