Acta Physico-Chimica Sinica  2017, Vol. 33 Issue (3): 573-581   (2746 KB)
 Article Options PDF (2746 KB) Full Text HTML Abstract Figures References History Received: October 24, 2016 Revised: December 12, 2016 Published on Web: December 12, 2016 Service Email this article to a colleague Add to my bookshell Add to citation manager Email Alert Feedback View Feedback Author ZHENG Yan-Gong ZHU Li-Na LI Han-Yu JIAN Jia-Wen DU Hai-Ying
Operating Mechanism of Palladium Oxide as a Potentiometric Sensing Electrode
ZHENG Yan-Gong1,*, ZHU Li-Na1, LI Han-Yu1, JIAN Jia-Wen1,*, DU Hai-Ying2
1 Faculty of Electrical Engineering and Computer Science, Ningbo University, Ningbo 315000, Zhejiang Province, P. R. China;
2 College of Mechanical and Electronic Engineering, Dalian Minzu University, Dalian 116600, Liaoning Province, P. R. China
Abstract: This paper describes the sensing properties of a potentiometric sensor based on a palladium oxide (PdO) electrode. Our investigation of the sensing mechanism is also discussed. We studied carbon monoxide (CO) sensing performance of a PdO electrode doped with Mg, Ni, and La, printed on zirconia. The results indicated that defects on the surface of PdO, which allow adsorption of CO, can effectively enhance the sensitivity of the sensors. To explore the source of the signal, a PdO-based electrode was printed on an alumina disc and a zeolite pellet for CO detection at 450℃. Notably the zeolite coupled with the PdO-based electrode to generate potentiometric responses to changes in CO concentration. According to the resistance and impedance measurements, the response to CO was ascribed to the changing interfacial potential between the PdO electrode and electrolyte. A model based on an electrochemical double layer between the PdO and electrolyte was determined to explain the behavior of the potentiometric sensor. It may be possible to harness these effects at PdO electrodes for the development of electrochemical sensors.
Key words: Palladium oxide     Potentiometric sensor     Doping effect     Carbon monoxide     Electrolyte

1 Introduction

For nearly a century, solid-state potentiometric sensors that employ oxide electrodes have been extensively studied and applied for sensing toxic gases1. Transition metal oxide has been widely used as a sensing electrode for various reasons, including its flexibility of production, simplicity of use, its ability to catalyze a large number of gases, and its thermal and chemical stability2-5. Noble metal oxides are widely used as additives or sensitizers to improve the sensing performance of functional materials6. Few reports consider the unique properties of palladium oxide (PdO) and its performance in gas sensing as a functional element7, 8.

In our previous work8, PdO′s performance as a sensing electrode was explored based on a YSZ (8% (x, molar fraction) Yttriastabilized Zirconia) electrolyte, which was measured via a potentiometry method to detect carbon monoxide (CO). Attractive phenomena were observed. Changes in the electric potential of the sensor in a CO environment are independent of the mobile oxygen in the electrolyte and the thickness of the PdO electrode. A hypothesis is proposed that a potentiometric sensor based on a PdO electrode works in capacitive mode during a sensing process.

The working mechanism of a potentiometric sensor with a PdObased electrode is our focus in this paper. In order to verify the hypothesis, several aspects of the working principle were studied by experimental methods. First, PdO was doped by Ni, La, and Mg. The doping is capable of shrinking the particle size of PdO and creating defects in PdO. The influence on the sensing performance of the sensor was discussed. Second, zirconia was replaced by other materials to test the impact of the electrolyte on the sensing performance. Third, the source of the sensing signal was located by measuring the impedance and resistance. The working model of the sensors with PdO-based electrodes is discussed.

2 Materials and methods
2.1 Materials preparation

Pd (C2H3O2)2, Ni (NO3)2∙6H2O, La (NO3)3∙6H2O and Mg (NO3)2∙ 6H2O were obtained from Sinopharm Chemical Reagent Co. Ltd., China. Y-type zeolite (Na-Y, Si/Al molar ratio=2.5) was pruchased from Alfa Aesar, China. The above chemical reagents were of analytical grade and used without further purification.

Three types of dopants are fabricated based on PdO. Elements used for doping are transition metal (Ni2+), alkaline earth metal (Mg2+), and rare earth metal (La3+). The molar ratios of the palladium and doped elements are 100 : 5, 100 : 10, and 100 : 15, which are denoted by M-PdO-5, M-PdO-10, and M-PdO-15, respectively (where M represents the doped elements, i.e., Ni, Mg, La). The preparation is described in Ref.8: a certain quality of Pd (C2H3O2)2 is dissolved in alcohol by energetic stirring. A corresponding quality of doped element in nitrate is weighed and added to the palladium acetate solution. Hydrolysis is achieved by adding deionized water at 90 ℃ for 2 h. The obtained solution is centrifuged to precipitate the resulting material, and then dried in a box oven at 130 ℃ for 12 h. The resulting sample is calcined at 700 ℃ for 2 h in air.

2.2 Material characterization

X-ray diffraction (XRD, Bruker D8 Focus, Germany) patterns are obtained with Cu Kα radiation (0.1541 nm). Scanning electron microscopy (SEM, Hitachi S-4800, Japan) is performed to obtain images of the samples. The stoichiometric ratio, as well as the quality percentage of the doping element in the samples, is analyzed with an energy dispersive spectrometer (EDS, QUANTAX 400, Germany). The impedance spectroscopy is measured with an Agilent 4284A (USA) at 100 mV in the range of 25 Hz-1 MHz. The electrical resistance of the sensors was measured by a computer-controlled Agilent multimeter (Agilent 34405A, USA).

2.3 Fabrication of the sensor

YSZ and alumina chips (8% (molar fraction) Y2O3 doped zirconia), fabricated by the Shanghai Institute of Ceramics (Chinese Academy of Sciences, China), are used as the electrolyte in the sensor. The YSZ and alumina discs measure 7 mm × 7 mm × 0.5 mm and 7 mm × 7 mm × 0.8 mm, respectively. For the reference electrode, commercial Pt paste (TR27905, Japan Tanaka Precious Metal Industries Ltd.) is applied to one side of the YSZ by screen printing, and then dried at 130 ℃ for 20 min. The Pt reference electrode, which is considered an ideal reversible electrode9, is sintered at a temperature of 1200 ℃ for 2 h. The prepared PdObased samples and α-terpineol are mixed to obtain the sensing electrode paste, which is screen printed on the other side of the YSZ and sintered at 700 ℃ for 2 h. Finally, both electrodes are attached with Pt lead wires. Sensing electrodes with areas of 3 mm × 3 mm (9 mm2), 5 mm × 5 mm (25 mm2), and 7 mm × 7 mm (49 mm2) are created by screen printing. If there are no special instructions, the size of the sensing electrode is 5 mm × 5 mm. The structure and image of the sensors are shown in Fig. 1.

 Fig. 1 (a) Basic schematic of the sensor and (b) photo of the sensors with different areas of sensing electrode

Y-type zeolite is a microporous, crystalline aluminosilicate that has mobile sodium cations inside the framework10. The zeolite pellets are prepared by pressing 200 mg of zeolite powder under 5 t of uniaxial force, and then sintered at 700 ℃ for 2 h. The processes involved in the preparation of the sensor with zeolite are the same as those previously described, with the exception of the sintering temperature for the Pt reference electrode, which is 700 ℃. The framework of zeolite will collapse at a temperature higher than 800 ℃10.

2.4 Sensing apparatus

The sensor is placed in a hermetic quartz tube and heated under different temperatures, which are controlled by a temperature controller and heater in a tubular furnace. The flow rate of different gases is controlled independently by using computercontrolled electronic mass flow controllers (D07-19B, Seven Star Electronics, China). During the test, the total flow rate is maintained at 100 mL∙min-1, and the sensing and reference electrodes are exposed to the same atmosphere. The electric potential (V) between the sensing and reference electrodes is recorded by using a multifunction data acquisition card (USB-6221, National Instruments, USA). The response of the potentiometric sensor is measured as the difference in potential (∆V) between the sensors in the background gas (N2 and 5% (φ, volume fraction) O2 are usually used) and in the targeted gas. The positive terminal is always connected to the PdO-based electrode, and the negative terminal is connected to the Pt electrode.

3 Results
3.1 Doping effects on PdO electrode

Since PdO will decompose to metallic Pd at approximately 800 ℃11, PdO-based dopants are prepared at 700 ℃. XRD patterns of pure and doped PdO are shown in Fig. 2 and Fig.S1 (see Supporting Information). All diffraction peaks coincide with the corresponding peaks of PdO given in the standard data file (JCPDS File No. 43-1024). No peaks corresponding to the oxidic dopant are observed, even for the 15% (x, molar fraction) doped samples. This may occur because of the small mass percentage of dopant in the samples. The peaks become broader and weaker when Ni is doped. Peak positions and full width at half maximum (FWHM) are used to determine the cell parameters and crystallite sizes for all palladium oxide12. The lattice parameters for all samples are calculated from the XRD peak positions in Fig. 2 and are listed in Table 1. The cell volume has an initial increase during the incorporation of Ni, and then decreases with the increasing doping concentration.

 Fig. 2 XRD patterns of pure and Ni-doped PdO

Table 1 Measured lattice parameters of Ni-doped PdO

Typical SEM images of pure and Ni-doped PdO are shown in Fig. 3(a-d). The grain becomes smaller as the level of doping increases. The average particle sizes are estimated to be~90, ~72, ~59, and~50 nm for PdO and the dopants Ni-PdO-5, Ni-PdO-10, and Ni-PdO-15, respectively. Agglomerates are clearly observable, and they cause a random spatial distribution. The images of the surfaces of the YSZ disc and the Na-Y pellet are shown in Fig. 3(e, f).

 Fig. 3 SEM images of (a) PdO and dopants with different levels of doping (b) Ni-PdO-5, (c) Ni-PdO-10, and (d) Ni-PdO-15; (e) surface of YSZ disc, and (f) Na-Y pellet

To investigate the relationship between the defects of PdO and the sensing performance of the sensors, an EDS analysis of pure and Ni-doped PdO is carried out to study the impact of the doping. The results in Table 2 indicate that the samples are non-stoichiometric, and the atomic ratio of Pd/Ni increases with the doping level. Moreover, the largest oxygen vacancy is observed on the surface of Ni-PdO-10.

Table 2 Element contents of pure and Ni-doped PdO samples

The role of a dopant is to disrupt the chemical bonds on the surface of the host oxide to ready the doped oxide for chemical interaction13, 14. In the case of Ni-doped PdO, according to XRD patterns and SEM images, the crystals become smaller as the doping content increases. Comparing the relative ionic radius of Pd2+ (0.064 nm) and Ni2+ (0.069 nm), substituting Ni into the Pd positions would increase the unit cell volume. The experimental trend shows an initial increase in unit cell volume, with a decrease that follows the doping content, as shown in Table 1. It is also noticeable that the unit cell volumes of all Ni-doped samples are larger than the undoped volumes. Combining the atomic ratios on the surface obtained by EDS in Table 2, the ratio of Ni increases with the doping level. When the host oxide suffers heavy doping, the dopant tends to be segregated and forms a layer of oxide clusters that heal the oxygen vacancies on the surface13. By contrast, a lower concentration of dopant will solid-dissolve into the crystal of PdO and expand its unit cell volume14-16. At the same time, a solid solution will create more defects by crystal distortion17, 18.

Various sensing electrodes made by PdO-based dopants on YSZ are tested in CO environments. The sensing responses for 100 × 10-6 (volume fraction) CO are given in Fig. 4. A general improvement is observed for the sensors with Ni-and La-doped PdO electrodes in the range of 400-550 ℃. The best working temperature is in the range of 450 to 500 ℃. At temperatures above 500 ℃, the sensors′ responses decay. The doped electrodes, in which Pd and foreign elements are present in a molar ratio of 100 : 5, have the best performance. In particular, the best CO sensor uses Ni-doped PdO at 450 ℃. Hereafter, the sensor made of a NiPdO-5 sensing electrode is used to conduct the study in this paper.

 Fig. 4 Sensing response of potentiometric sensor with doped PdO electrode to CO at (a) 400 ℃, (b) 450 ℃, (c) 500 ℃, and (d) 550 ℃, balanced by N2 and 5% O

For the sensing test in Fig. 4, the Ni-and La-doped PdO behaves better than the undoped version. Despite an increasing response observed for the sensors with Ni-and La-doped PdO electrodes, different active sites are brought into the samples by La, Ni, and Mg. According to the classification of dopant-oxide pairs13, La is a high-valence dopant (HVD), while Mg and Ni are same-valance dopants (SVD). HVD intends to adsorb O2 from a gas phase at the vacant sites, and activates it. Thus, a reducing gas can react with this oxygen and undergo oxidation. In the case of SVD, since MgO is irreducible and the valence of Ni is flexible, it could be predicted that the flexible-valance dopant is favorable for promoting the mobility of oxygen vacancies. The sensing signal of conventional potentiometric sensors can be effectively improved by decreasing the surface area of the grains of the sensing electrode and increasing the contact area of triple phase boundary (TPB)19. However, the response was enhanced by creating oxygen vancancies in the PdO electrode in our study. The oxygen vacancies are the sites for the catalytic oxidation between CO and adsorbed ionic oxygen6.

An O2-dependent experiment is conducted on the sensor at 450 ℃, as shown in Fig. 5. As can be seen, the increasing percentage of O2 in the environment leads to a rise in the baseline of the sensor. The average increase is 12 mV when the O2 concentration doubles. In the meantime, the response of the sensor toward 100 × 10-6 (volume fraction) of CO decreases by approximately 4 mV because of the increase in the O2 concentration. O2 does interfere significantly with the sensing performance.

 Fig. 5 Electric potential change for sensor with Ni-PdO-5 electrode to 100 × 10-6 (volume fraction) CO balanced by 5%, 10%, and 20%(volume fraction) O2 and N2 at 450 ℃

Sensing electrodes with different areas are tested, and the results for CO detection at 450 ℃ are given in Fig. 6. When the responses are plotted versus CO concentrations on a logarithmic scale, the relationship is linear. The responses for all sensors increase as the CO concentration increases. Moreover, the sensitivities of the sensors, which are the slopes of the plots in Fig. 6, are -30.36, -38.21, and -38.77 mV∙decade-1 for sensors with sensing electrodes having areas of 9, 25, and 49 mm2, respectively.The increasing sensing area leads to a higher response.

 Fig. 6 Dependence of ΔV for sensors with different areas of sensing electrode on CO concentrations balanced by 5% O2 and N2 at 450 ℃

Moreover, a potentiometric sensor based on coupling a solid electrolyte with semiconducting oxides is explained by the mixed potential theory20, which assumes a thermodynamic potential independent of the size of the electrode21. However, the potential is typically proportional to the area of the sensing electrode, as shown in Fig. 6. These results lead us to think that the sensing reactions in the sensor with a PdO-based electrode are of the capacitance type.

3.2 Role of electrolyte in gas sensing

In order to address the role of electrolyte in gas sensing, a NiPdO-5 electrode was printed on an alumina disc and zeolite pellet, and tested in a CO environment at 450 ℃. The potentiometric results of the sensor based on the alumina disc are shown in Fig. S2 (see Supporting Information). No potentiometric response is observed for the sensor printed on the alumina disc. Potentiometric responses for the sensor based on zeolite are obtained for 100 × 10-6, 200 × 10-6, and 400 × 10-6 (volume fraction) of CO, as shown in Fig. 7(a). Next, an O2 dependence experiment is conducted. The sensor is tested in 100 × 10-6 (volume fraction) CO under 5%, 10%, and 15% O2, as shown in Fig. 7(b). A depressive response to CO and a rising baseline with increasing O2 are noticed. Moreover, Ni-PdO-5 electrodes on YSZ and Na-Y have sensing profiles similar to those from the oxygen-dependent measurement. Ionic material is essential to generate a potentiometric response to CO. In other words, the changing of the chemical potential gradient in the electrolyte is the source of the sensing signal.

 Fig. 7 Potentiometric response of sensor combined with Ni-PdO-5 sensing electrode and Na-Y electrolyte to (a) 100 × 10-6, 200 × 10-6, and 400 × 10-6 (volume fraction) CO balanced with 5% O2 and N2 and (b) 100 × 10-6 (volume fraction) CO in 5%, 10%, and 15% O2 at 450 ℃

3.3 Source of the sensing signal

A solid-state potentiometric sensor for gas sensing is commonly explained by the mixed potential theory20. When the sensor is exposed to a targeted species, more than one cathodic or anodic reaction between the targeted species and components of the electrolyte occurs at the interface of the electrode/electrolyte, which is the so-called TPB. The resulting electrode potential becomes a mixed potential22. The following pair of reactions (1) and (2) occur at the interface of the sensing electrode/zirconia for gas sensing:

 $\text{Re}\left( \text{g} \right)\text{+}{{\text{O}}^{\text{2-}}}\left( \text{electrolyte} \right)\rightleftharpoons \text{Ox}\left( \text{g} \right)\text{+}n{{\text{e}}^{\text{-}}}\left( \text{electrode} \right)$ (1)

 ${{\text{O}}_{\text{2}}}\text{+}n{{\text{e}}^{\text{-}}}\left( \text{electrode} \right)\rightleftharpoons n{{\text{O}}^{\text{2-}}}\left( \text{electrolyte} \right)$ (2)

where Re (g) and Ox (g) represent a targeted gas in its reduced and oxidized forms, respectively.

To investigate the ionic motion of the potentiometric sensor during sensing process, impedance is carried out to measure the ionic conductivity of the sensors under variational CO or O2 environment as shown in Fig. 8. Since palladium oxide is a good electrical conductor, the measured impedance belongs to the electrolyte. For the measurements on the sensor with YSZ in Fig. 8 (a, b), the shift of the impedance in different CO concentrations, within experimental error, is negligible.

 Fig. 8 Complex impedance spectra of sensor on YSZ in different (a) CO and (b) oxygen concentrations, and sensor with Na-Y in different (c) CO and (d) oxygen concentrations within frequency range from 1 MHz to 25 Hz at 450 ℃

If the oxygen ions from the electrolyte participate in the electrochemical reactions, the impedance change in the electrolyte can be observed. However, the ionic conductivity decreases when oxygen is enriched in the environment. This occurs because more O2- enters the electrolyte23. This result agrees well with the electric potential increase of the potentiometric sensor, as shown in Fig. 5. No shift of impedance is observed in the CO environment; thus, the number of oxygen ions in the electrolyte and their respective mobility are not disturbed during the electrochemical reactions. For the sensor with zeolite, the impedance is constant under different gaseous environments, as shown in Fig. 8(c, d). The results indicate that sodium ions in zeolite will not be influenced by the gaseous species in the environment.

The mobile ions inside the electrolyte are essential for the generation of a potentiometric response. Since ionic flows from the chemical potential gradient are balanced by the electric field gradient24, the changing resistance across the sensors reflects the change in the chemical potential gradient under CO sensing processes. The electrical resistivity across the sensors decreases for both sensors when CO is introduced (Fig. 9). The resistance of the sensors is a series of Pt reference electrode, electrolyte, PdObased electrode, and their interfacial barrier. To address the source of the change in resistances of the sensors, a resistance of Ni-PdO-5 is measured for 100 × 10-6 (volume fraction) CO at 450 ℃ in Fig. S3 (see Supporting Information). The result indicates that no net electrons transfer between CO and PdO in the equilibrium state. Accordingly, the interfacial barrier between the sensing electrode and electrolyte decreases owing to CO adsorption. Therefore, the interfacial potential increase between the sensing electrode and electrolyte is the source of the potentiometric response.

 Fig. 9 Resistance change across sensors to 100 × 10-6, 200 × 10-6, and 300 × 10-6 (volume fraction) CO balanced by 5% O2 and N2 at 450 ℃ (a) sensor with YSZ electrolyte, (b) sensor with Na-Y electrolyte

4 Discussion

Based on the previous results and discussion, capacitive behaviors were observed for the potentiometric sensor with a PdObased electrode. When PdO is brought into contact with a ionic conductor, an electrochemical double layer appears25. The potential drop across the electrochemical double layer can be interpreted as

 $\Delta \phi =\frac{{{k}_{\text{B}}}T}{q}\ln \left( \frac{{{\rho }_{\text{PdO}}}}{{{\rho }_{\text{electrolyte}}}} \right)$ (3)

where kB is the Boltzmann constant, T is the temperature, q is elementary charge, and ρelectrolyte and ρPdO are the charge densities on the surface of PdO and the electrolyte, respectively.

The capacitance of the electrochemical double-layer is described by

 $C=\left( \frac{A}{d}+L\delta \right)\varepsilon$ (4)

where A is the area of the electrochemical double layer, d is the distance between them, L is the perimeter of the PdO electrode, δ is the edge effect in the capacitor, ε is the permittivity.

The catalytic oxidation of CO over PdO is expressed in equations (5)-(7)26, 27. The reactions could be described as follows27, 28: oxygen and carbon monoxide from the gas phase co-adsorbed at the vacant sites on the surface of the PdO, and interacted to form intermediates (e.g., "carbonate"), which will decompose to form CO2 and heal oxygen vacancies.

 ${{\text{O}}_{\text{2}\left( \text{g} \right)}}+n{{\text{e}}^{\text{-}}}\to \left( 1\le n\le 2 \right)$ (5)

 $\text{C}{{\text{O}}_{\left( \text{g} \right)}}+{{\text{e}}^{\text{-}}}\to \text{CO}_{\left( \text{ad} \right)}^{-}$ (6)

 \begin{align} &\text{CO}_{\left( \text{ad} \right)}^{-}+2\text{O}_{\left( \text{ad} \right)}^{n-}\to \left[\text{C}{{\text{O}}_{3}} \right]_{\left( \text{ad} \right)}^{2-}+\left( 2n-1 \right){{\text{e}}^{\text{-}}}\to \\ &\ \ \ \ \ \ \ \ \ \text{C}{{\text{O}}_{2\left( \text{g} \right)}}+\text{O}_{\left( \text{ad} \right)}^{2-}+\left( 2n-1 \right){{\text{e}}^{\text{-}}} \\ \end{align} (7)

During the catalytic oxidation, the ionic species are redistributed on the surface of PdO, the electrons shift between PdO and CO and O2, and mobile positive ions from the volume of electrolyte move toward the PdO-based electrode. If the mobile ions are negative, they will move from the surface into the volume of the electrolyte. During the sensing process, the charge density at the interface and the distribution of potential inside the electrolyte are altered. The degree of the alteration is related to the concentration of CO. Therefore, the potential change at the interface is linearly dependent on the logarithmic concentration of CO according to the equation (3). Moreover, a higher sensitivity of the sensor with larger area of PdO electrode is observed in the Fig. 6. According to the equation (4), the capacitance will increase with the increasing area of PdO electrode because of the edge effect in the capacitance. A higher capacitance is capable to hold more ionic species, which are favorable for the reactions at the interficial of PdO electrode and the electrolyte. Therefore, the charge density (ρPdO) is increased due to the edge effect, then it will lead to a higher sensitivity. A simplistic model uses the sensor with Na-Y as an example, and is shown in Fig. 10.

 Fig. 10 Schematic of mechanism to explain the response of potentiometric sensor constructed by Na-Y and PdO-based electrode under different conditions (a) sensor in background gas, (b) sensor exposed to CO

5 Conclusions

Potentiometric sensors based on noble metal oxide electrodes are an emerging field that is still awaiting consolidation and rationalization. A PdO sensing electrode, printed on YSZ and Na-Y, shows a potentiometric response to changes in CO partial pressure. Doping on PdO could result in a fair improvement in the sensing performance owing to the creation of defects, which would aid in the improvement of the oxidation reaction. The potentiometric response of sensors is ascribed to the interfacial potential between the PdO-based electrode and the electrolyte, e.g., zirconia and zeolite. The most important question is this: What qualities make PdO different from other metal oxides as a sensing electrode? The crystal of PdO has a sub-micro size, thus the PdO electrode has a larger surface area than the oxide electrode used in other literature29, 30. Furthermore, PdO has excellent catalytic activity; thus, gas molecules will be consumed before they reach the TPB. Finally, the relatively weak metal oxygen bonding in PdO could facilitate the transport of oxygen vacancies and the adsorption of charged species. It is advisable to study PdObased electrodes with other electrolytes to explore more applications of solid-state electrochemical sensors.

Supporting Information: available free of charge via the internet at http://www.whxb.pku.edu.cn.

Reference
 (1) Park C. O.; Fergus J. W.; Miura N.; Park J.; Choi A. Ionics 2009, 15, 261. doi: 10.1007/s11581-008-0300-6 (2) Di Bartolomeo E.; Grilli M. L.; Traversa E. J. Electrochem. Soc. 2004, 151, H133. doi: 10.1149/1.1695387 (3) Di Bartolomeo E.; Grilli M. L.; Yoon J. W.; Traversa E.J. Am. Chem. Soc. 2004, 87, 1883. doi: 10.1111/j.1151-2916.2004.tb06335.x (4) Tang W.; Wang J.; Yao P. J.; Du H. Y.; Sun Y. H. ActaPhys. -Chim. Sin. 2014, 30, (4), 781. [唐伟, 王兢, 姚朋军, 杜海英, 孙炎辉. 物理化学学报, 2014, 30, (4), 781.] doi: 10.3866/PKU.WHXB201402191 (5) Feng Q. X.; Yu P.; Wang J.; Li X. G. Acta Phys. -Chim. Sin. 2015, 31, (12), 2405. [冯秋霞, 于鹏, 王兢, 李晓干. 物理化学学报, 2015, 31, (12), 2405.] doi: 10.3866/PKU.WHXB201510261 (6) Korotcenkov G. Mat. Sci. Eng. B-Solid 2007, 139, 1. doi: 10.1016/j.mseb.2007.01.044 (7) Chiang Y. J.; Pan F. M. J. Phys. Chem. C. 2013, 117, 15593. doi: 10.1021/jp402074w (8) Zhu L.; Zheng Y.; Jian J. Ionics 2015, 21, 2919. doi: 10.1007/s11581-015-1487-y (9) Zhang W. F.; Schmidt-Zhang P.; Guth U. Solid State Ionics 2004, 169, 121. doi: 10.1016/j.ssi.2003.10.004 (10) Auerbach S. M.; Carrado K. A.; Dutta P. K. Handbook ofZeolite Science and Technology; Marcel Dekker Inc.: New York 2003 (11) Zheng Y.; Qiao Q.; Wang J.; Li X.; Jian J. Sens. Actuator BChem. 2015, 212, 256. doi: 10.1016/j.snb.2015.02.035 (12) Bukhari S. M.; Giorgi J. B. Solid State Ionics 2010, 181, 392. doi: 10.1016/j.ssi.2010.01.017 (13) McFarland E. W.; Metiu H. Chem. Rev. 2013, 113, 4391. doi: 10.1021/cr300323w (14) Zheng Y.; Wang J.; Yao P. Sens. Actuator B-Chem. 2011, 156, 723. doi: 10.1016/j.snb.2011.02.026 (15) Gurlo A. Nanoscale 2011, 3, 154. doi: 10.1039/c0nr00560f (16) Burbano M.; Norberg S. T.; Hull S.; Eriksson S. G.; Marrocchelli D.; Madden P. A.; Watson G. W. Chem. Mater. 2011, 24, 222. doi: 10.1021/cm2031152 (17) Zhang J.; Xie K.; Wei H.; Qin Q.; Qi W.; Yang L.; Ruan C.; Wu Y. Sci. Rep. 2014, 4, 7082. doi: 10.1038/srep07082 (18) Kim Y. M.; He J.; Biegalski M. D.; Ambaye H.; Lauter V.; Christen H. M.; Pantelides S. T.; Pennycook S. J.; Kalinin S.V.; Borisevich A. Y. Nat. Mater. 2012, 11, 888. doi: 10.1038/NMAT3393 (19) Elumalai P.; Wang J.; Zhuiykov S.; Terada D.; Hasei M.; Miura N. J. Electrochem. Soc. 2005, 152, H95. doi: 10.1149/1.1923707 (20) Mukundan R.; Brosha E. L.; Brown D. R.; Garzon F. H.J. Electrochem. Soc. 2000, 147, 1583. doi: 10.1149/1.1393398 (21) Stetter J. R.; Li J. Chem. Rev. 2008, 108, 352. doi: 10.1021/cr0681039 (22) Garzon F. H.; Mukundan R.; Brosha E. L. Solid-State MixedPotential Gas Sensors: Theory, Experiments and Challenges; Elsevier: Kidlington, Royaume-Uni 2000 (23) Sridhar S.; Stancovski V.; Pal U. B. Solid State Ionics 1997, 100, 17. doi: 10.1016/S0167-2738(97)00322-6 (24) Lim D. K.; Im H. N.; Song S. J. Sci. Rep. 2016, 6, 18804. doi: 10.1038/srep18804 (25) Simon P.; Gogotsi Y. Nat. Mater. 2008, 7, 845. doi: 10.1038/nmat2297 (26) Gong X. Q.; Hu P.; Raval R. J. Chem. Phys. 2003, 119, 6324. doi: 10.1063/1.1602053 (27) Gabasch H.; Knop-Gericke A.; Schlogl R.; Borasio M.; Weilach C.; Rupprechter G.; Penner S.; Jenewein B.; Hayek K.; Klotzer B. Phys. Chem. Chem. Phys. 2007, 9, 533. doi: 10.1039/b610719b (28) Weaver J. F. Chem. Rev. 2013, 113, 4164. doi: 10.1021/cr300323wl (29) Macam E. R.; Blackburn B. M.; Wachsman E. D. Sens.Actuator B-Chem. 2011, 157, 353. doi: 10.1016/j.snb.2011.05.014 (30) Miura N.; Raisen T.; Lu G.; Yamazoe N. J. Electrochem. Soc. 1997, 144, L198. doi: 10.1149/1.1344558