# Temperature Dependent Electrical Properties and Catalytic Activities ofLa2O3–CO2–H2O Phase System

Authors: Bahcine Bakiz; Frédéric Guinneton; Madjid Arab; Sylvie Villain; Abdeljalil Benlhachemi; Jean Raymond Gavarri
Journal: Advances in Materials Science and Engineering
 (2009)

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## Abstract

We present a study of electrical properties and catalytic activities of materials belonging to the hydrated carbonated systemLa2O3–CO2–H2O. The polycrystalline hydroxycarbonate, dioxycarbonate, and oxide are prepared via a coprecipitation route followed by heat treatment. The electrical conduction of the phases obtained by thermal decomposition from LaOHCO3, H2O is analyzed by electrical impedance spectroscopy, from 25°C to 950°C, under air. The catalytic properties of LaOHCO3, La2O2CO3 and La2O3 polycrystalline phases are studied by FTIR spectroscopy, in presence of gas mixtures CO-air and CH4-air, at temperatures ranging between 100°C to 525°C. The three materials behave differently in presence of CO or CH4 gases.


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## Body

## 1. Introduction

The general aim of this study is to test the reactivity of materials sensitive to environmental water andCO2, and interacting with  toxic gases (CO, CH4). Presently we deal with the system La2O3–CO2–H2O that presents hydrated and carbonated phases, stable at various temperatures [1–6]; the hydroxycarbonate phase LaOHCO3 stable up to 380°C [7]; the dioxycarbonate phase La2O2CO2 stable up to 700°C, and finally the La2O3 phase stable above this temperature, under air atmosphere. Each phase can be sensitive to partial pressure of H2O or CO2. Consequently, these phases can be used as sensing materials reacting with wet air and CO2. In a first step, we try to determine the evolution of electrical conduction of these phases with increasing temperature; in a second step, we compare the temperature and time dependent catalytic efficiencies of LaOHCO3, La2O2CO3, and La2O3, to convert CH4 and CO present in air-CH4 and air-CO flows.


## 2. Experimental

The samples were prepared by a coprecipitation route described in a recent work [8].  A first step consisted in mixing three aqueous solutions: (1) La(NO3)3·6H2O, (2) urea CO(NH2)2, and (3) polyvinyl-pyrrolydine (PVP) polymer. The initial pH was 3.2. A similar approach was proposed by Li et al. [9]. A second step consisted in heating the solution in a reactor equipped with a vapor condenser, at 80°C. In all experiments, solutions were permanently agitated through a magnet rotating with a fixed rate of 300 rpm. During heating, temperature was fixed, and vapors were condensed through a water-cooled circuit to avoid vanishing of the aqueous solution. A white solid was obtained by precipitation.The thermal decomposition of this solid (the polycrystalline initial hydroxycarbonate phaseLaOHCO3·H2O) was initially studied by thermogravimetry, from room temperature to 1100°C. Then, the same LaOHCO3, H2O phase was compacted in form of cylindrical pellet, and placed in a heating cell, in a Solartron electrical impedance equipment. Platinum circular electrodes were fixed on the two faces of pellet. The electrical analyses that were performed in the temperature range of 25 to 950°C and in the frequency range of 1 to 107 Hz, with a maximal tension of 1 V.  The conductivities were determined from extrapolation of the Nyquist representations delivered by the software of the equipment, and taking into account the dimensions of samples.The catalytic activities were determined using an infrared (FTIR) spectrometer, adapted for analyses of emitted gases. This homemade equipment was described in previous works [10]. Samples are placed in a catalytic cell and a gas flow cross through the powder at various temperatures and various flow rates. The polycrystalline phases LaOHCO3, La2O2CO3, and La2O3 were subjected successively to air-CH4 and air-CO flows, at various temperatures and as a function of time. In all experiments, we used flow rates of 10 sccm and gas concentrations in air of 2500 ppm. The catalytic efficiency is defined as being the intensity of the CO2 vibrational band at 2340–2360 cm-1 resulting from the following transformations:(1)CH4+2O2⇒CO2+2H2O
or(2)CO+12O2⇒CO2.Additional studies by transmission electron microscopy allowed to determine the distributions of sizes and shapes of crystal grains in each sample (not presented here). From these microstructural analyses, we could define calculated grain surfacesSi and grain volumes Vi for each phase noted i (the index i represents La2O3,La2O2CO3, or LaOHCO3). This allowed calculation of specific surfaces Si/Vi. Then, from the mass of each sample used for catalytic analyses, it has been possible to determine an approximate total surface Si for each powdered sample. This surface Si has been used to normalize our FTIR data and allow comparison of catalytic efficiencies. The normalized intensities (I/Si) are calculated by dividing the intensities of CO2 bands by the surfaces Si of samples. The values Si are successively in m2: S(i=La2O3) = 0.61, S(i=La2O2CO3)=2.31, S(i=LaOHCO3)=5.62.


## 3. Results and Discussion

### 3.1. Thermal Analyses and Electrical Responses

Using first classical TG-TDA analysis of the hydrated hydroxycarbonate sample, we have determined the various temperature ranges of phase stabilities. These preliminary results were useful to better interpret our electrical measurements. Figure1(a) gives the conventional thermal analysis using thermogravimetry data coupled with differential thermal analysis (TG-DTA). The various mass losses versus temperature in °C are clearly visible with a first lattice water departure, then the change of hydroxycarbonate into La2O2CO3 and, finally, the final formation of La2O3.(a) Thermal decomposition analysis (DTA-TG) of hydrated hydroxycarbonate: successive phasesLaOHCO3 (LHC), La2O2CO3 (LOC), and La2O3 (L), (b) Electrical impedance analysis of hydrated hydroxycarbonate: variation of lnσ versus 1000/T. Existence of electrical changes corresponding to chemical decomposition.
(a)(b)Figure1(b) gives the corresponding thermal evolution of the logarithm of conductivitylnσ as a function of 1000/T (T being in K) of the initial hydrated hydroxycarbonate phase; as temperature increases, the electrical modifications due to thermal decomposition are observed through undulations on the curve lnσ versus 1000/T. In Figure 1(b), as 1000/T decreases, several domains are observed as follows(a)
At low temperature (25–300°C), an increasing low conductivity is observed, with weak activation energy; this is typically relative to extrinsic conduction linked to surface water and proton (OH-) mobility;(b)
Between 350 and 700°C, if we extrapolate the previous lower temperature results, we can observe an abnormal variation of conductivity; it is due to the OH- and CO2 species departure, involving defect formation in hydroxycarbonate and formation of dioxycarbonate La2O2CO3;(c)
Between 700°C and 800°C, a very weak abnormal evolution is observed (undulation), probably due to the lastCO2 departure from the oxycarbonate, with transformation into oxide La2O3 (phase with higher activation energy).Taking into account the logarithmic scale of the graph, we observe a relatively strong variation of the electrical signal between 300 and 600°C; this domain, in which the OH- and one of the CO32- species are unstable in the lattice, should be highly sensitive to water and CO2 exchanges. This might be used to detect water and CO2 molecules in a gas sensor.


### 3.2. Catalytic Studies

Figures2(a), 2(b) give the normalized catalytic efficiencies (intensities of CO2 vibrational frequency band) of La2O2CO3 and La2O3 subjected to CH4-air flow (2500 ppm CH4) at different temperatures. Because of thermal decomposition occurring at a temperature greater than 350°C, no experiment was possible for LaOHCO3. Figure 3(a) reports the results for the LaOHCO3 phase at various temperatures. The maximum catalytic efficiency of each material interacting with CO is obtained at a relatively low temperature (275°C).The catalysis of CH4 is obtained at higher temperatures (above 450°C). Figure 3(b) gives the normalized catalytic efficiencies of the three phases in presence of air-CO flows at a given temperature of 275°C. It is clearly evidenced that the catalytic efficiency of La2O3 (per surface unit) is greater than that of the two other compounds.(a) catalytic conversion ofCH4 interacting with La2O2CO3 as a function of time and temperature, (b) catalytic conversion of CH4 interacting with La2O3 as a function of time and temperature. The normalized efficiencies are expressed in arbitrary units (a.u.).
(a)
La2O2CO3(b)
La2O3(a) catalytic efficiencies of LaOHCO3 in presence of air-CO flows at various temperatures, (b) compared catalytic efficiencies of La2O3,La2O2CO3 and LaOHCO3 in presence of air-CO flows, at a fixed temperature of 275°C; the normalized efficiencies are expressed in a.u.
(a)(b)


## 3.1. Thermal Analyses and Electrical Responses

Using first classical TG-TDA analysis of the hydrated hydroxycarbonate sample, we have determined the various temperature ranges of phase stabilities. These preliminary results were useful to better interpret our electrical measurements. Figure1(a) gives the conventional thermal analysis using thermogravimetry data coupled with differential thermal analysis (TG-DTA). The various mass losses versus temperature in °C are clearly visible with a first lattice water departure, then the change of hydroxycarbonate into La2O2CO3 and, finally, the final formation of La2O3.(a) Thermal decomposition analysis (DTA-TG) of hydrated hydroxycarbonate: successive phasesLaOHCO3 (LHC), La2O2CO3 (LOC), and La2O3 (L), (b) Electrical impedance analysis of hydrated hydroxycarbonate: variation of lnσ versus 1000/T. Existence of electrical changes corresponding to chemical decomposition.
(a)(b)Figure1(b) gives the corresponding thermal evolution of the logarithm of conductivitylnσ as a function of 1000/T (T being in K) of the initial hydrated hydroxycarbonate phase; as temperature increases, the electrical modifications due to thermal decomposition are observed through undulations on the curve lnσ versus 1000/T. In Figure 1(b), as 1000/T decreases, several domains are observed as follows(a)
At low temperature (25–300°C), an increasing low conductivity is observed, with weak activation energy; this is typically relative to extrinsic conduction linked to surface water and proton (OH-) mobility;(b)
Between 350 and 700°C, if we extrapolate the previous lower temperature results, we can observe an abnormal variation of conductivity; it is due to the OH- and CO2 species departure, involving defect formation in hydroxycarbonate and formation of dioxycarbonate La2O2CO3;(c)
Between 700°C and 800°C, a very weak abnormal evolution is observed (undulation), probably due to the lastCO2 departure from the oxycarbonate, with transformation into oxide La2O3 (phase with higher activation energy).Taking into account the logarithmic scale of the graph, we observe a relatively strong variation of the electrical signal between 300 and 600°C; this domain, in which the OH- and one of the CO32- species are unstable in the lattice, should be highly sensitive to water and CO2 exchanges. This might be used to detect water and CO2 molecules in a gas sensor.


## 3.2. Catalytic Studies

Figures2(a), 2(b) give the normalized catalytic efficiencies (intensities of CO2 vibrational frequency band) of La2O2CO3 and La2O3 subjected to CH4-air flow (2500 ppm CH4) at different temperatures. Because of thermal decomposition occurring at a temperature greater than 350°C, no experiment was possible for LaOHCO3. Figure 3(a) reports the results for the LaOHCO3 phase at various temperatures. The maximum catalytic efficiency of each material interacting with CO is obtained at a relatively low temperature (275°C).The catalysis of CH4 is obtained at higher temperatures (above 450°C). Figure 3(b) gives the normalized catalytic efficiencies of the three phases in presence of air-CO flows at a given temperature of 275°C. It is clearly evidenced that the catalytic efficiency of La2O3 (per surface unit) is greater than that of the two other compounds.(a) catalytic conversion ofCH4 interacting with La2O2CO3 as a function of time and temperature, (b) catalytic conversion of CH4 interacting with La2O3 as a function of time and temperature. The normalized efficiencies are expressed in arbitrary units (a.u.).
(a)
La2O2CO3(b)
La2O3(a) catalytic efficiencies of LaOHCO3 in presence of air-CO flows at various temperatures, (b) compared catalytic efficiencies of La2O3,La2O2CO3 and LaOHCO3 in presence of air-CO flows, at a fixed temperature of 275°C; the normalized efficiencies are expressed in a.u.
(a)(b)


## 4. Conclusion

In this study, we have developed an electrical approach allowing determining the electrical responses of a phase change involvingH2O and CO2 molecules elimination, from electrical impedance analyses. The departure of the couple H2O+CO2 can be linked to an increase of conductivity (the slope of the ln(σ) curve increases in the range of 400–600°C) followed by a stabilization of the conductivity (in the range of 600 to 700°C) associated with last carbonate phase formation. The increase of conductivity might be ascribed to the high mobility of unstable chemical specie, mainly protons that can jump easily from oxygen to oxygen or OH- species that can migrate from vacancies to vacancies as soon as they are formed. In this temperature range, the variation of conductivity should be sufficiently significant to be used to detect presence of CO2. Specific experiments involving action of CO2 on La2O3 are in progress and will be published elsewhere. In the range of 700 to 800°C, the observed smooth undulation might be due to a last CO2 departure and formation of final stable oxide. From the analyses of catalytic interactions, it should be noted that LaOHCO3 and La2O2CO3 can be good catalysts for CO in air-CO mixtures. These phases might have some interest in selectivity of gas sensors interacting with environmental gas mixtures (CO+CO2+H2O); they might be stable in presence of CO2 and could interact with CO. At low temperature, they might only interact with environmental CO2 or H2O. At higher temperature, they might only interact with CO, not with these environmental gases.



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*Source: 612130-2009-12-28.xml*