Open Access

Ag-Cu nanoalloyed film as a high-performance cathode electrocatalytic material for zinc-air battery

Nanoscale Research Letters201510:197

https://doi.org/10.1186/s11671-015-0900-9

Received: 17 March 2015

Accepted: 10 April 2015

Published: 23 April 2015

Abstract

A novel Ag50Cu50 film electrocatalyst for oxygen reduction reaction (ORR) was prepared by pulsed laser deposition (PLD) method. The electrocatalyst actually is Ag-Cu alloyed nanoparticles embedded in amorphous Cu film, based on transmission electron microscopy (TEM) characterization. The rotating disk electrode (RDE) measurements provide evidence that the ORR proceed via a four-electron pathway on the electrocatalysts in alkaline solution. And it is much more efficient than pure Ag catalyst. The catalytic layer has maximum power density of 67 mW cm−2 and an acceptable cell voltage at 0.863 V when current densities increased up to 100 mA cm−2 in the Ag50Cu50-based primary zinc-air battery. The resulting rechargeable zinc-air battery exhibits low charge-discharge voltage polarization of 1.1 V at 20 mAcm−2 and high durability over 100 cycles in natural air.

Keywords

Pulsed laser deposition Alloyed Ag-Cu Electrocatalyst Zinc-air battery

Background

Metal-air batteries have attracted a lot of attention as a possible energy storage solution for decades [1]. Among various metal-air batteries, zinc-air battery holds the greatest promise for future energy applications [2], owing to its high power density, safety, and economic viability and the abundant zinc reserve in earth [3-5]. The key point for development of zinc-air battery is finding high-performance oxygen reduction reaction (ORR) catalysts. Precious metals, like Pt, are usually used as ORR catalysts [6,7]. In general, Pt-based catalysts can be prepared via various routes, such as electrochemical deposition [8], chemical vapor deposition [9,10], and facile hydrothermal method [11]. Since the catalyst utilization in the fuel cell is determined mainly by the contact surface area of catalyst with electrolyte, the reduction of the thickness of catalytic layer can result in an improvement of the catalyst utilization and reduction of the fuel cell cost [12]. Therefore, pulse laser deposition (PLD) is also used popularly in the field [13-15], because the approach is a feasible way to control the thickness of catalyst layer. Moreover, compared to aforementioned chemical preparations, PLD method also owns high repeatability and stability in process, making it to be a suitable route to obtain electrocatalyst with film state.

Although Pt-based film catalyst has already obtained progress via PLD method [15], it is still expected to further decrease the cost of ORR catalyst. Therefore, the 3d transition metal oxides [16-19], silver [20-27], and its related alloy with transition metals, such as Ag-Co and Ag-Mn [28-31], which consume less cost than Pt were investigated extensively in an alkaline environment. Beyond that, Ag-Cu alloyed materials also might be suitable electrocatalyst for reasons. Theoretical calculations indicate that Ag-Cu alloyed nanoparticles exhibit strong adsorption energies and low activation-energy barriers [32,33]. Meanwhile, Ag and Cu own the same facet-center cubic structure and similar cell parameters. Synthesis of Ag-Cu alloyed catalyst is supposed to be easier than other types of Ag alloy [34]. It is reasonable to believe that Ag-Cu nanoalloy could become a new generation of catalysts. However, successful synthesis of real Ag-Cu alloyed catalysts in nanoscale has seldom been reported aside from some Ag-Cu heterostructures which do not have alloy state [35,36].

Based on the aforementioned background, herein, we expect PLD method can be applied to prepare Ag-Cu alloyed catalyst film, which not only does greatly reduce the catalytic cost but also can obtain effective ORR catalytic activity. In this work, we demonstrate a design of Ag-Cu alloyed film electrocatalyst synthesized via pulsed laser deposition (PLD). The ORR catalytic property of the as-prepared Ag-Cu electrocatalyst has been tested and compared to commercial Pt/C, Ir/C, and Ag film catalysts. Both of the resulting primary and rechargeable zinc-air battery show good performance in natural air.

Methods

Synthesis of Ag50Cu50 film electrocatalyst

Ag-Cu alloyed catalyst was prepared by PLD method in a vacuum chamber with a pressure of 2 × 10−4 Pa. The target of Ag-Cu alloy with atomic ratio of 50:50 was irradiated with a nanosecond Q-switched Nd:YAG laser beam (EKSPLA, Lithuania). The wavelength was set to be 266 nm, and the pulse duration was ranging from 3 to 6 ns. The laser beam diameter was around 1 mm, with an energy density of 200 mJ/pulse. Both target and substrate (nickel foam) rotated at a speed of 5 rpm during deposition, and target was irradiated for 2 min at 10 Hz to clear away the oxide on the surface before deposition. The laser was operated at the frequency of 10 Hz. The deposition time is set as 90 min. The as-prepared product is Ag50Cu50 catalyst.

Electrochemical measurements

The ORR activities of Ag50Cu50 catalyst were studied at room temperature via measuring rotating disk electrode (RDE) polarization curves. The experiments were performed with a classic three-electrode cell containing a saturated calomel electrode (SCE) as reference electrode, a Pt counter electrode, and Ag-Cu catalyst supported on nickel foam as the working electrode in the CHI660C electrochemical workstation. The electrolyte was 0.1 M KOH aqueous solution. The experiments were performed over the potential range of 0 to −0.8 V at a scanning rate of 10 mV s−1. All potentials reported in this work were converted from the SCE to the RHE scale using E(RHE) = E(SCE) + 0.991 V in 0.1 M KOH. The rotation rates were controlled at 400, 800, 1,200, and 1,600 rpm. The working area for oxygen diffusion in the air electrode was 0.785 cm2.

Performance test of zinc-air battery

The catalyst layer was made by the direct deposition of Ag-Cu alloyed catalyst onto the nickel foam current collector. The air cathode was then assembled by the catalyst layer and the gas diffusion layer prepared by mixing acetylene black and 60% PTFE with a mass ratio of 1:2. A zinc-air battery was then fabricated by the prepared air cathode and pure zinc plate anode and 6 M KOH electrolytes with 0.2 M zinc acetate solution. The cell voltage polarization, power density curves, and specific capacity for the primary zinc-air battery have been tested. The charge and discharge characteristic and the cycle performance of the resulting zinc-air battery were tested by the BTS-9000 battery test system in a homemade metal-air battery model in air where air was introduced from the backside of the gas diffusion layer.

Material characterization on AgCu alloyed catalysts

Ag50Cu50 catalyst was investigated through comprehensive characterization with scanning electron microscope (SEM), transmission electron microscope (TEM), high-resolution TEM, and high-angle annular dark field (HAADF) carried out on a JEM-2200FS TEM (JEOL Ltd., Akishima-shi, Japan). An empty Ni grid was placed in PLD instrument with nickel foam to directly obtain TEM sample for plain viewing observation.

Results and discussion

Characterization on Ag50Cu50 catalyst

Figure 1 shows series of TEM analysis on Ag50Cu50 catalyst. According to Figure 1a, plenty of nanoparticles distribute in a continuous film. The tiny nanoparticles with size under 5 nm dominate the film. Magnifying the blue rectangle area, the obtained HRTEM is shown in Figure 1b. It can be seen that they display two different states: few are amorphous, and the left are with crystallized state.
Figure 1

TEM and HAADF characterization of Ag50Cu50 catalysts. (a) Bright field image, (b) HRTEM, (c) HAADF result, and (d) IFFT image. The scale bar for the inset FFT image in (b) is 5 nm−1.

Fast Fourier transform (FFT) analysis has been performed on particle marked with red rectangle in Figure 1b. Based on the inset FFT image, it is believed that the particle has FCC structure with zone axis of [110]. The corresponding IFFT image is shown in Figure 1d. The d-spacing of (111) and (002) planes are measured to be 0.218 and 0.184 nm, respectively, which show contract upon alloying compared to d-spacing of (111)Ag and (002)Ag. The contracted value is around 7.35% for them. Owing to smaller atomic radius of Cu atom (0.12 nm) than Ag atom (0.1445 nm), only when Cu atoms have solute into Ag cell and form Ag-Cu alloy the shrinkage of d-spacing is reasonable. Here, it is of note that TEM used in this work is well calculated, and the deviation is under 2%. Therefore, interference caused by TEM deviation to the conclusion has been excluded. In addition, HAADF result shown in Figure 1c displays that contrast of the particles is brighter than gap area between particles, demonstrating a higher atomic number Z for nanoparticles. The lower Z corresponding gap area then is attributed from Cu element. This is because Z of Cu (Z = 29) is smaller than Ag (Z = 47). Combining the amorphous state in gap area observed in Figure 1b, we can draw that Ag50Cu50 catalyst actually is Ag-Cu alloyed nanoparticles embedded in amorphous Cu film.

Electrochemical performance

A series of electrochemical characterizations have been carried out on Ag50Cu50 catalyst. Figure 2a shows RDE polarization curves of Ag50Cu50 catalyst with rotation rate 1,600 rpm in N2 and O2 saturated 0.1 M KOH solutions. It can be seen that there is reduction current density in O2-saturated KOH solution, while that in N2-saturated solution is flat and the value is close to 0 mA cm−2. The fact indicates that the catalyst indeed works on O2. Figure 2b shows a set of RDE curves with rotation rates of 400, 800, 1,200, and 1,600 rpm. The curves demonstrate that the current density increases with elevating rotation rate. It is because the higher speed of rotating disk electrode, the shorter diffusion distance of oxygen to catalyst surface. The Koutecky-Levich plots were then obtained from the limiting current density, as shown in Figure 2c. The plots show the inverse current density (J −1) as a function of ω–1/2. The detailed Koutecky-Levich equation [37] is expressed as follows:
Figure 2

The electrochemical characterization on Ag50Cu50 catalyst. (a) The RDE curves of Ag50Cu50 catalyst in O2 and N2-saturated 0.1 M KOH solution; (b) the RDE curves at the rotation rates of 400, 800, 1,200, and 1,600 rpm; (c) the Koutecky-Levich plot of Ag50Cu50 catalyst; and (d) the ORR mass activity for Ag, Ag50Cu50, and Pt/C (20 wt%) catalysts.

$$ {J}^{-1}={J}_k^{-1}+{\left(0.62{nFCD}^{\frac{2}{3}}{V}^{-\frac{1}{6}}{\omega}^{\frac{1}{2}}\right)}^{-1} $$
(1)
where J is current density, J k is the kinetic current density of the ORR, n is the number of transferred electrons during ORR, F is the Faraday constant, C is the bulk concentration of O2, D is the diffusion coefficient of O2 in 0.1 M KOH solution, V is the kinetic viscosity of the electrolyte for 0.1 M KOH, and ω is the angular velocity of the disk. After input of these values into Equation 1, n was determined to be 3.76, 3.87, 3.85, and 3.97 when the potential was 0.5, 0.4, 0.3, and 0.2 V, respectively. The result points out that a four-electron pathway occurred, which is a more efficient than the two-electron pathway [38,39].

We also compare the polarization curve of Ag50Cu50 catalyst to commercial Pt/C (20 wt%) and Ag catalysts on a RDE in O2-saturated KOH solution at 1,600 rpm, as shown in Figure 2d. Here, Ag catalyst was obtained through the same PLD process with Ag50Cu50. The limiting current density of Ag catalyst for ORR is only −2 mA mg−1 at 0.2 V. For Ag50Cu50 catalyst, it displays a significant improvement. The onset potential and limiting current density for ORR are 0.81 V and −12.3 mA mg−1 at 0.2 V, respectively. Pt/C catalyst has also been tested and is shown with black curve. Although there is a difference between Pt/C catalyst and Ag50Cu50 catalyst, it is still believed that the catalyst has excellent catalytic activity for ORR. Moreover, the low cost makes it an excellent candidate to substitute precious Pt-based catalysts.

Zinc-air battery performance

Ag50Cu50 catalyst then was used in a cathode catalyst to evaluate its practical application in primary zinc-air battery. The results are shown in Figure 3. The cell voltage polarization and power density curves for the primary zinc-air battery are shown in Figure 3a. The cell voltage decreases with increasing current density, demonstrating that the cell performance shows a strong dependence on the resistance of the battery. The open circuit voltage of the cell is around 1.48 V closing to the theoretical value, and the maximum power density is 67 mW cm−2 at 100 mA cm−2. Figure 3b displays the change of cell voltage with time at a current density of 10, 20, and 30 mA cm−2. The initial discharge voltage for Ag50Cu50 catalyst decreases from 1.12 to 0.97 V when the current density within the range from 10 to 30 mA cm−2. The three curves keep flat after more than 8 h of discharge, indicating a high discharge voltage stability. As shown in Figure 3c, when the current density is 30 mA cm−2, the specific capacity of Ag50Cu50 catalyst-based battery is 598 mAh g−1 as normalized by the mass of consumed Zn anode, corresponding to specific energy density about 610 mWh g−1. When changing the current density to 20 mA cm−2, the specific capacity and specific energy density increase to 678 mAh g−1 and 725.5 mWh g−1, respectively, which is comparable to CoOx/carbon nanotube-based zinc-air battery [40]. The green curve corresponding to 10 mA cm−2 shows a sudden falling. It may result from shedding Zn plate during discharge process. The above results indicate that Ag50Cu50 catalyst prepared via PLD is a highly efficient catalyst in primary zinc-air battery.
Figure 3

The performance of the primary zinc-air battery with Ag50Cu50 catalyst. (a) The cell voltage and power density curves of a primary zinc-air battery. (b) The cell voltage and time curves at different current density of 10, 20, and 30 mA cm−2 in the primary zinc-air battery. (c) The specific capacity curves of the primary zinc-air battery at 10, 20, and 30 mA cm−2. The electrolyte is 6 M KOH solution under natural air atmosphere.

Figure 4a shows the charge and discharge polarization curve of the resulting rechargeable zinc-air battery with Ag50Cu50 catalyst. The cell voltage rose with a steady trend from 1.4 to 2.7 V when the current density was increasing. When the current density was 20 mA cm−2, the cell voltages for charge and discharge were 1.0 and 2.1 V, respectively. Therefore, the over potential is 1.1 V, which is close to the value of Co3O4 nanodisk catalyst [41]. To well understand the performance of such battery, we also collect the polarization curve from commercial Pt/C and Ir/C catalyst-based zinc-air battery (blue dotted line) in reference [3]. It can be clearly seen that the over potential of Ag50Cu50 is approaching to Pt/C and Ir/C based battery at 20 mA cm−2. Someone may argue that 1.1 V is higher than reported non-precious catalyst-based batteries. The fact is the value was obtained from natural air atmosphere in this work, not the artificial high-density oxygen atmosphere. Therefore, the Ag50Cu50-based battery owns good practicability. The discharge cell voltage still keeps 0.7 V at a high current density of 100 mA cm−2, demonstrating an excellent battery performance. The cycle performance of the rechargeable battery is shown in Figure 4b. It underwent 100 cycles at 20 mA cm−2 with 20 min per cycle. The round-trip efficiency of the first cycle was 52.3%, and the last cycle was 50%. They do as well as that of zinc-air battery assembled with cobalt oxide-based cell [41,42], indicating a good stability for the Ag50Cu50 battery.
Figure 4

The performance of the rechargeable zinc-air battery with Ag50Cu50 catalyst. (a) Charge and discharge polarization curves of the rechargeable zinc-air battery using Ag50Cu50 catalyst compared with the one using Pt/C and Ir/C (blue dotted line). (b) The cycle performance of the rechargeable zinc-air battery with Ag50Cu50 catalyst. The electrolyte is 6 M KOH plus 0.2 M zinc acetate solution under natural air atmosphere.

According to all the above electrochemical characterization and the battery performance, the excellent ORR catalytic activity is believed. It is speculated that these are resulting from the alloying between Ag and Cu. Before we verify the speculation, it is necessary to analyze the formation of AgCu alloyed film firstly. In general, whether a metal forms a continuous film or grows into discrete clusters (or nanoparticles) depends on the relative magnitudes of the adhesion energy (E adh) and the metal/vacuum interfacial free energy (γ v/m). If E adh < 2γ v/m, three-dimensional growth is expected to occur via the Volmer-Weber growth mode [43,44]. As Ag satisfies the criterion [45], Ag nanoparticles have formed at the very beginning of PLD process, and they are showing as tiny amorphous particles at the beginning. In terms of Cu, it is speculated to form as amorphous Cu film using the criterion [46].

There are two possible ways for Cu atom solute into Ag cell. One is some Cu atoms may be surrounded inside the Ag nanoparticles during the PLD ejecting process. The second way is some Cu atoms included in the amorphous Cu film contacting surface of Ag nanoparticles. At this stage, Ag and Cu atoms mixed randomly within the tiny nanoparticles, and they have not formed the alloyed state. In Figure 4b, we can see that the amorphous particles are smaller than the crystallized ones in size. It indicates that they are in this stage.

After the above stage, the following are then the crystallization and growth for the Ag-rich amorphous nanoparticles. The substrate used in PLD is difficult to be definitely clear and pure, which consequently creates preferred sites promoting the nanoparticles to crystallize. In terms of growth, it may occur through coalescence, because of the relatively short diffusion distances [45]. Eventually, Cu atoms have solute into Ag cell via substituting some of Ag atoms and form into silver-rich AgCu solid solution nanoparticles, that is, AgCu alloyed nanoparticles. With increment of deposit time, the alloying degree between Ag and Cu elevates. However, if the deposit time is too long, AgCu alloyed nanoparticles may grow bigger and bigger, like the huge nanoparticles shown in Figure 4a. The ORR activity will get deteriorated, because the bigger the nanoparticles, the smaller the specific surface area.

According to the formation mechanism of AgCu film, the alloying between Ag and Cu is verified from the aspect of PLD process. In our previous work, it demonstrates that pure Cu material catalyzed ORR barely [8]. Therefore, the enhancement of ORR catalytic activity of Ag50Cu50 film actually is from AgCu alloyed nanoparticles. The synergistic effect between Ag and Cu within the alloyed nanoparticles calculated by simulation is verified through the experiments [47,33]. It is also consistent with the d-bond center theory [48,49]. The theory aims to design a highly active catalyst for ORR via synthesizing a binary or multi-alloy with various metals which have different absorption and desorption energy for oxygen [50]. Ag has the strong oxygen desorption energy, yet the Cu has forceful absorption energy. As a result, when Ag and Cu are formed into AgCu alloy or bimetallic nanomaterials, the product will improve the ORR activity to a great extent owing to the synergistic effect between Ag and Cu atoms.

In addition, the enhancement in ORR activity of Ag50Cu50 over Ag catalyst also can be explained by the ligand effect and strain effect. Regarding the ligand effect, it actually originates from the random Cu atoms solute into (near) surface of structure of various AgCu catalysts. In terms of the strain effect, it could be caused by the shorter Ag-Ag bond length in Ag50Cu50 catalyst than Ag catalyst, given the fact that d-spacing of Ag50Cu50 planes were smaller than the corresponding Ag planes. The two effects both improve the catalytic activity of the catalyst, which can weaken Ag-O binding energies and strengthen the O2 molecular adsorption to the surface of AgCu solid solution [51].

Since the good catalytic activity is attributed to alloyed AgCu nanoparticles, we can illustrate the good recycle stability of Ag50Cu50 catalyst-based zinc-air battery from the perspective of morphology. In Figure 5b, the morphology of Ag50Cu50 catalyst shows as flocculence after recycle test at a macro level, which is not as smooth as its original state shown in Figure 5a. From the inset image in Figure 5b, the particles which were previously embedded in Cu film escape from Cu film. Some particles may shed, while most of the particles expose more surface than before. Therefore, despite slight change of morphology, the retaining of AgCu alloyed nanoparticles and increased specific surface area help keep the good catalytic activity for Ag50Cu50 cell, even if it already underwent long charge and discharge recycles.
Figure 5

The morphology of the Ag50Cu50 catalyst before (a) and after (b) recycle performance test.

Conclusions

We demonstrate a design of Ag-Cu film catalyst via PLD. The obtained Ag50Cu50 film shows excellent ORR catalytic activity. TEM results verify the catalyst actually is AgCu alloyed nanoparticles embedded in amorphous Cu film. The alloying between Ag and Cu from the embedded AgCu nanoparticles synergistically improves the ORR catalytic activity. Using the catalyst to assemble a zinc-air battery, the maximum power density is 67 mW cm−2 in primary zinc-air battery. The resulting rechargeable zinc-air battery shows low charge-discharge voltage polarization of 1.1 V at 20 mA cm−2 and high stability over 100 charge and discharge cycles in natural air.

Declarations

Acknowledgements

This study was supported by the National Natural Science Foundation of China (grant nos. 51271148 and 50971100), the Research Fund of State Key Laboratory of Solidification Processing in China (grant no. 30-TP-2009), the Aeronautic Science Foundation Program of China (grant no. 2012ZF53073), and the Doctoral Fund of Ministry of Education of China (grant no. 20136102110013)

Authors’ Affiliations

(1)
State Key Laboratory of Solidification Processing, Northwestern Polytechnical University
(2)
School of Chemical and Biomolecular Engineering, University of Sydney

References

  1. Cheng F, Chen J. Metal–air batteries: from oxygen reduction electrochemistry to cathode catalysts. Chem Soc Rev. 2012;41(6):2172–92.View ArticleGoogle Scholar
  2. Li Y, Dai H. Recent advances in zinc–air batteries. Chem Soc Rev. 2014;43(15):5257–75.View ArticleGoogle Scholar
  3. Li Y, Gong M, Liang Y, Feng J, Kim J-E, Wang H, et al. Advanced zinc-air batteries based on high-performance hybrid electrocatalysts. Nat Commun. 2013;4:1805. http://dx.doi.org/10.1038/ncomms2812.View ArticleGoogle Scholar
  4. Lee JS, Tai Kim S, Cao R, Choi NS, Liu M, Lee KT, et al. Metal–air batteries with high energy density: Li–air versus Zn–air. Adv Energy Mater. 2011;1(1):34–50.View ArticleGoogle Scholar
  5. Oh SH, Black R, Pomerantseva E, Lee J-H, Nazar LF. Synthesis of a metallic mesoporous pyrochlore as a catalyst for lithium–O2 batteries. Nat Chem. 2012;4(12):1004–10.View ArticleGoogle Scholar
  6. Wang J, Yin G, Shao Y, Zhang S, Wang Z, Gao Y. Effect of carbon black support corrosion on the durability of Pt/C catalyst. J Power Sources. 2007;171(2):331–9.View ArticleGoogle Scholar
  7. Jackson A, Viswanathan V, Forman AJ, Larsen AH, Nørskov JK, Jaramillo TF. Climbing the activity volcano: core–shell Ru@ Pt electrocatalysts for oxygen reduction. Chem Electro Chem. 2014;1(1):67–71.Google Scholar
  8. Jin Y, Chen F. Facile preparation of Ag-Cu bifunctional electrocatalysts for zinc-air batteries. Electrochim Acta. 2015;158:437–45.View ArticleGoogle Scholar
  9. Zhu S, Chen Z, Li B, Higgins D, Wang H, Li H, et al. Nitrogen-doped carbon nanotubes as air cathode catalysts in zinc-air battery. Electrochim Acta. 2011;56(14):5080–4.View ArticleGoogle Scholar
  10. Chen Z, Yu A, Higgins D, Li H, Wang H, Chen Z. Highly active and durable core–corona structured bifunctional catalyst for rechargeable metal–air battery application. Nano Lett. 2012;12(4):1946–52.View ArticleGoogle Scholar
  11. Goh FT, Liu Z, Ge X, Zong Y, Du G, Hor TA. Ag nanoparticle-modified MnO 2 nanorods catalyst for use as an air electrode in zinc–air battery. Electrochim Acta. 2013;114:598–604.View ArticleGoogle Scholar
  12. Natarajan SK, Hamelin J. High-performance anode for polymer electrolyte membrane fuel cells by multiple-layer Pt sputter deposition. J Power Sources. 2010;195(22):7574–7.View ArticleGoogle Scholar
  13. Montenegro M, Döbeli M, Lippert T, Müller S, Schnyder B, Weidenkaff A, et al. Pulsed laser deposition of La 0.6 Ca 0.4 CoO 3 (LCCO) films. A promising metal-oxide catalyst for air based batteries. Phys Chem Chem Phys. 2002;4(12):2799–805.View ArticleGoogle Scholar
  14. Montenegro M, Lippert T, Müller S, Weidenkaff A, Willmott P, Wokaun A. Pulsed laser deposition of electrochemically active perovskite films. Appl Surf Sci. 2002;197:505–11.View ArticleGoogle Scholar
  15. Mróz W, Budner B, Tokarz W, Piela P, Korwin-Pawlowski ML. Ultra-low-loading pulsed-laser-deposited platinum catalyst films for polymer electrolyte membrane fuel cells. J Power Sources. 2015;273:885–93.View ArticleGoogle Scholar
  16. Du G, Liu X, Zong Y, Hor TA, Yu A, Liu Z. Co 3 O 4 nanoparticle-modified MnO 2 nanotube bifunctional oxygen cathode catalysts for rechargeable zinc–air batteries. Nanoscale. 2013;5(11):4657–61.View ArticleGoogle Scholar
  17. Lee DU, Kim BJ, Chen Z. One-pot synthesis of a mesoporous NiCo 2 O 4 nanoplatelet and graphene hybrid and its oxygen reduction and evolution activities as an efficient bi-functional electrocatalyst. J Materials Chem A. 2013;1(15):4754–62.View ArticleGoogle Scholar
  18. Prabu M, Ketpang K, Shanmugam S. Hierarchical nanostructured NiCo 2 O 4 as an efficient bifunctional non-precious metal catalyst for rechargeable zinc–air batteries. Nanoscale. 2014;6(6):3173–81.View ArticleGoogle Scholar
  19. Prabu M, Ramakrishnan P, Shanmugam S. CoMn 2 O 4 nanoparticles anchored on nitrogen-doped graphene nanosheets as bifunctional electrocatalyst for rechargeable zinc–air battery. Electrochem Commun. 2014;41:59–63.View ArticleGoogle Scholar
  20. Spendelow JS, Wieckowski A. Electrocatalysis of oxygen reduction and small alcohol oxidation in alkaline media. Phys Chem Chem Phys. 2007;9(21):2654–75. doi:10.1039/B703315J.View ArticleGoogle Scholar
  21. Lemke AJ, O’Toole AW, Phillips RS, Eisenbraun ET. The effect of high anionomer loading with silver nanowire catalysts on the oxygen reduction reaction in alkaline environment. J Power Sources. 2014;256:319–23. doi:10.1016/j.jpowsour.2014.12.141.View ArticleGoogle Scholar
  22. Neumann CCM, Laborda E, Tschulik K, Ward KR, Compton RG. Performance of silver nanoparticles in the catalysis of the oxygen reduction reaction in neutral media: efficiency limitation due to hydrogen peroxide escape. Nano Res. 2013;6(7):511–24. doi:10.1007/s12274-013-0328-4.View ArticleGoogle Scholar
  23. Sharifi N, Tajabadi F, Taghavinia N. Nanostructured silver fibers: facile synthesis based on natural cellulose and application to graphite composite electrode for oxygen reduction. Int J Hydrog Energy. 2010;35(8):3258–62. doi:10.1016/j.ijhydene.2010.01.147.View ArticleGoogle Scholar
  24. Xu XH, Tan C, Liu HJ, Wang F, Li ZL, Liu JJ, et al. Carbon black supported ultra-high loading silver nanoparticle catalyst and its enhanced electrocatalytic activity towards oxygen reduction reaction in alkaline medium. J Electroanal Chem. 2013;696:9–14. doi:10.1016/j.jelechem.2013.02.018.View ArticleGoogle Scholar
  25. Chatenet M, Genies-Bultel L, Aurousseau M, Durand R, Andolfatto F. Oxygen reduction on silver catalysts in solutions containing various concentrations of sodium hydroxide—comparison with platinum. J Appl Electrochem. 2002;32(10):1131–40. doi:10.1023/a:1021231503922.View ArticleGoogle Scholar
  26. Lu YZ, Chen W. Size effect of silver nanoclusters on their catalytic activity for oxygen electro-reduction. J Power Sources. 2012;197(0):107–10. http://dx.doi.org/10.1016/j.jpowsour.2011.09.033.View ArticleGoogle Scholar
  27. Singh P, Buttry DA. Comparison of oxygen reduction reaction at silver nanoparticles and polycrystalline silver electrodes in alkaline solution. J Phys Chem C. 2012;116(19):10656–63. doi:10.1021/jp301676n.View ArticleGoogle Scholar
  28. Beer SZ, Sandler YL. Oxygen reduction at silver and silver-based alloy electrodes. J Electrochem Soc. 1965;112(11):1133–6. doi:10.1149/1.2423379.View ArticleGoogle Scholar
  29. Arul Raj I, Vasu KI. Electrochemical and oxygen reduction behaviour of solid silver-bismuth/antimony electrodes in KOH solutions. J Appl Electrochem. 1993;23(7):728–34. doi:10.1007/BF00243342.View ArticleGoogle Scholar
  30. Lima FHB, de Castro JFR, Ticianelli EA. Silver-cobalt bimetallic particles for oxygen reduction in alkaline media. J Power Sources. 2006;161(2):806–12. http://dx.doi.org/10.1016/j.jpowsour.2006.06.029.View ArticleGoogle Scholar
  31. Kostowskyj MA, Kirk DW, Thorpe SJ. Ag and Ag–Mn nanowire catalysts for alkaline fuel cells. International. J Hydrogen Ener. 2010;35(11):5666–72. http://dx.doi.org/10.1016/j.ijhydene.2010.02.125.View ArticleGoogle Scholar
  32. Shin K, Kim DH, Yeo SC, Lee HM. Structural stability of AgCu bimetallic nanoparticles and their application as a catalyst: a DFT study. Catal Today. 2012;185(1):94–8. http://dx.doi.org/10.1016/j.cattod.2011.09.022.View ArticleGoogle Scholar
  33. Shin K, Kim DH, Lee HM. Catalytic characteristics of AgCu bimetallic nanoparticles in the oxygen reduction reaction. ChemSusChem. 2013;6(6):1044–9. doi:10.1002/cssc.201201001.View ArticleGoogle Scholar
  34. Lei Y, Chen F, Huang B, Liu Z. Synthesis and characterization of L12 ordered silver-copper alloy nanodendrites. Materials Res Express. 2014;1(1):015031.View ArticleGoogle Scholar
  35. Han M, Liu S, Zhang L, Zhang C, Tu W, Dai Z, et al. Synthesis of octopus-tentacle-like Cu nanowire-Ag nanocrystals heterostructures and their enhanced electrocatalytic performance for oxygen reduction reaction. ACS Appl Mater Interfaces. 2012;4(12):6654–60. doi:10.1021/am301814y.View ArticleGoogle Scholar
  36. Kang YR, Chen FY. Preparation of Ag–Cu bimetallic dendritic nanostructures and their hydrogen peroxide electroreduction property. J Appl Electrochem. 2013;43(7):667–77. doi:10.1007/s10800-013-0563-0.View ArticleGoogle Scholar
  37. Liu ZW, Peng F, Wang HJ, Yu H, Zheng WX, Yang J. Phosphorus‐doped graphite layers with high electrocatalytic activity for the O2 reduction in an alkaline medium. Angew Chem. 2011;123(14):3315–9.View ArticleGoogle Scholar
  38. Wang Y, Liu Y, Lu X, Li Z, Zhang H, Cui X, et al. Silver-molybdate electrocatalysts for oxygen reduction reaction in alkaline media. Electrochem Commun. 2012;20:171–4.View ArticleGoogle Scholar
  39. Garcia AC, Gasparotto LH, Gomes JF, Tremiliosi-Filho G. Straightforward synthesis of carbon-supported Ag nanoparticles and their application for the oxygen reduction reaction. Electrocatalysis. 2012;3(2):147–52.View ArticleGoogle Scholar
  40. Li Y, Gong M, Liang Y, Feng J, Kim J-E, Wang H, et al. Advanced zinc-air batteries based on high-performance hybrid electrocatalysts. Nat Commun. 2013;4:1805. doi:10.1038/ncomms2812.View ArticleGoogle Scholar
  41. Lee DU, Scott J, Park HW, Abureden S, Choi J-Y, Chen Z. Morphologically controlled Co 3 O 4 nanodisks as practical bi-functional catalyst for rechargeable zinc–air battery applications. Electrochem Commun. 2014;43:109–12.View ArticleGoogle Scholar
  42. Lee DU, Choi JY, Feng K, Park HW, Chen Z. Advanced extremely durable 3D bifunctional air electrodes for rechargeable zinc-air batteries. Adv Energy Mater. 2014;4(6):1301389.Google Scholar
  43. Campbell CT. Ultrathin metal films and particles on oxide surfaces: structural, electronic and chemisorptive properties. Surf Sci Rep. 1997;27(1):1–111.View ArticleGoogle Scholar
  44. Alonso J, Diamant R, Castillo P, Acosta–García M, Batina N. Thin films of silver nanoparticles deposited in vacuum by pulsed laser ablation using a YAG. Nd laser Appl Surface Sci. 2009;255(9):4933–7.View ArticleGoogle Scholar
  45. Barnes J, Petford-Long A, Doole R, Serna R, Gonzalo J, Suarez-Garcia A, et al. Structural studies of Ag nanocrystals embedded in amorphous Al2O3 grown by pulsed laser deposition. Nanotechnology. 2002;13(4):465.View ArticleGoogle Scholar
  46. Kriese M, Moody N, Gerberich W. Effects of annealing and interlayers on the adhesion energy of copper thin films to SiO2/Si substrates. Acta Mater. 1998;46(18):6623–30.View ArticleGoogle Scholar
  47. Ma W, Chen F, Zhang N, Wu X. Oxygen reduction reaction on Cu-doped Ag cluster for fuel-cell cathode. J Mol Model. 2014;20(10):1–8. doi:10.1007/s00894-014-2454-7.View ArticleGoogle Scholar
  48. Lima FHB, Zhang J, Shao MH, Sasaki K, Vukmirovic MB, Ticianelli EA, et al. Catalytic activity–d-band center correlation for the O2 reduction reaction on platinum in alkaline solutions. J Phys Chem C. 2006;111(1):404–10. doi:10.1021/jp065181r.View ArticleGoogle Scholar
  49. Nørskov JK, Rossmeisl J, Logadottir A, Lindqvist L, Kitchin JR, Bligaard T, et al. Origin of the overpotential for oxygen reduction at a fuel-cell cathode. J Phys Chem B. 2004;108(46):17886–92. doi:10.1021/jp047349j.View ArticleGoogle Scholar
  50. Jackson A, Viswanathan V, Forman AJ, Larsen AH, Nørskov JK, Jaramillo TF. Climbing the activity volcano: core–shell Ru@Pt electrocatalysts for oxygen reduction. Chem Electro Chem. 2014;1(1):67–71. doi:10.1002/celc.201300117.Google Scholar
  51. Holewinski A, Idrobo J-C, Linic S. High-performance Ag–Co alloy catalysts for electrochemical oxygen reduction. Nat Chem. 2014;6(9):828–34.View ArticleGoogle Scholar

Copyright

© Lei et al.; licensee Springer. 2015

This is an Open Access article distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/4.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly credited.