Synthesis of Highly Efficient Bifunctional Ag/Co3O4 Catalyst for Oxygen Reduction and Oxygen Evolution Reactions in Alkaline Medium

Ag/Co3O4 catalysts using three different modes of solution combustion synthesis were developed and characterized by X-ray diffraction, X-ray photoelectron spectroscopy, scanning electron microscopy, and transmission electron microscopy to identify crystallite size, oxidation state, composition, and morphology. Cyclic voltammetry and linear sweep voltammetry measurements for the oxygen reduction reaction (ORR) and oxygen evolution reaction (OER) confirm the bifunctionality of the electrocatalysts. The electrochemical evaluation indicates that a synergic effect between Ag and Co enhances the activity through the fast breaking of O–O bond in the molecular oxygen to enhance the reduction mechanism. The high content of cobalt (Co) in the catalyst Ag/Co3O4-12, synthesized by second wave combustion, improves the activity for ORR, and the reaction mechanism follows a 3.9 number of electron transfer in overall reaction. The kinetic and limiting current densities of Ag/Co3O4-12 are maximum when compared to those of other Ag/Co3O4 catalysts and are very close to commercial Pt/C. Moreover, the maximum current density of OER for Ag/Co3O4-12 makes it a promising candidate for various bifunctional electrocatalytic applications such as fuel cells and metal–air batteries.


■ INTRODUCTION
Energy conversion electrochemical technologies such as polymer electrolyte fuel cells and metal−air batteries show highly efficient performance based on the oxygen catalyst in the reaction mechanism. 1−5 Platinum (Pt) has been recognized as the most efficient catalyst for anode and cathode of the fuel cells. 6−10 However, its high cost and availability limit its use, and it is an urgent task to find the replacement of Pt with readily available and cheaper ones. Oxygen reduction reaction (ORR) and oxygen evolution reaction (OER) are cathodic and anodic reaction techniques that are applicable for fuel cells, water splitting, and CO 2 reduction and in energy-storage solar fuel synthesis. 11−14 Precious metals such as Pt, Ru, and Ir are well-known OER catalysts with moderate overpotential. 15 It is reported that RuO 2 is thermodynamically unstable, whereas Pt and Ir cause agglomeration in the atomic scale, which prevents them to act as bifunctional catalysts over time. 16,17 It is challenging to introduce a bifunctional oxygen catalyst for both ORR and OER. 17−20 A bimetallic catalyst shows distinct physical and chemical properties that differ from its monometallic catalyst because of the high synergy between the individual metals. 21 The bimetals of transition metals has different applications in the field of catalysis, batteries, and solar energy conversion by the presence of hybrid sites and its concomitant functionalities. 22−28 Bimetallic catalysts have the exciting tuning properties to enhance the reaction pathway. Previous studies have reported on the extensive behavior of bimetals in catalysis, which possess unique properties strongly associated with their intrinsic electronic or geometric structures. 24,29−32 Effective oxygen reduction catalyst with high activity and low cost remains a great challenge. In this work, we demonstrate the synthesis of bifunctional catalysts that are active for ORR and OER suitable to be used in fuel cells and water electrolysisrelated applications.
Silver (Ag) shows high activity, better tolerance, stability, and longer performance for ORR mechanism. 33,34 The weaker Ag−O 2 interaction results in a stronger O−O bond that causes difficulty in breaking the bond of the electrolyte. Therefore, the Ag−O interaction must be stronger to enhance the electrochemical activity of the catalyst and consequently increases the kinetics of ORR. This can be achieved by incorporating the cheaper metals along with Ag. Cobalt (Co) is a better option because of its low cost, electrical resistance, and corrosion-free nature in basic medium. An active Co 3+ site in Co 3 O 4 shows great performance in ORR. The high interaction of adsorbed oxygen with Ag in the Ag−Co/C particle increases the ORR activity by rupturing the O−O bond. Also, the adsorption of oxygen to Ag from the well-oxidized Co 3 O 4 results in increase in the oxygen transport rate. Lin et al. reported that the presence of Co in Au−Co for ORR changes the electronic structure of the gold. 35 Wang et al. reported on the hydrothermal method of the synthesis of Ag−C, Co 3 O 4 −C, and Ag/Co 3 O 4 −C and compared the monometal and bimetal effect in the catalytic activity. 36 We followed a fast, simple, and single-step solution combustion synthesis (SCS) resulted with the preparation of a wide range of nanoparticles (NPs) of high surface area and porosity in cost-effective way. 37,38 SCS mode is based on the redox reaction between the oxidizing agent (metal nitrate) and the fuel (e.g., urea, glycine, and hydrazine). The fuels mostly used are sources of carbon and hydrogen that are ideally highly water-soluble cyclic and linear organic amines and amino acids with low decomposition temperature. 39 The exothermic reactions between the reactive group (NH 3 ) of fuel and nitric acid (HNO 3 ) from metal nitrate are the primary source of energy to initiate the combustion mode. Hydrogen-rich atmosphere formed during combustion determines the phase of the resulted NPs whether it is pure metal (H 2 rich) or its oxides (H 2 lean), which results in the formation of NPs with a high crystalline structure without any postthermal treatments such as calcination. 40,41 It is possible to synthesize various metals, metal oxides, metal sulfides, and alloys with different properties and dimensions through the precise control of specific fuel and the fuel-to-oxidizer ratio. 42−44 The large amount of gases such as carbon dioxide, nitrogen, and water formed during the combustion causes the significant expansion of gaseous product and reduces the temperature after reduction that would help in the formation of finely dispersed porous nanostructures. 45,46 Manukyan and co-workers studied the mechanism of SCS for the synthesis of nanocrystalline metallic materials using different in situ techniques. 47 They found the effect of fuel-to-oxidizer ratio on the transformation of metal oxides to metals and vice versa. The stoichiometric equation and the mechanism behind the combustion synthesis of NP were reported in our previous work. 48,49 In this work, we first propose a single-step combustion synthesis of Ag/Co 3 O 4 through three different modes, which shows good ORR and OER response in basic medium.
■ RESULTS AND DISCUSSION X-ray diffraction (XRD) patterns indicate the phases of the synthesized Ag/Co 3 O 4 catalysts ( Figure 1). In all the three synthesis modes, Ag is in metallic form, whereas Co is present in the form of its oxides (CoO and Co 3 O 4 36 The formation of CoO in Ag/Co 3 O 4 -12 and Ag/Co 3 O 4 -21 samples could be due to the second wave of combustion where additional fuel is added to synthesize the second phase that could partially reduce Co 3 O 4 to CoO as reported earlier. 49 The absorption spectrum of monometallic Ag NP gave the surface plasmon resonance (SPR) peak at 470 nm ( Figure 2a). Co shows that two SPR peaks centered at lower band (540 nm) are associated with O 2− to Co 2+ and those centered at higher band (800 nm) correspond to O 2− to Co 3+ transition. 50,51 Ag/Co 3 O 4 showing one absorption peak at the lower band in the region between the resonance peak of monometals Ag and Co clearly indicates the formation of an Ag−Co NP alloy not only a mixture of Ag and Co NPs. In Ag/ Co 3 O 4 -12, the lower resonance peak was observed at 450 nm with a clear blue shift when compared to Ag/Co 3 O 4 -11 and Ag/Co 3 O 4 -21. The blue shift in Ag/Co 3 O 4 -12 could be due to the strong quantum confinement effect that shifts the energy levels of conduction and valence bands with decrease in particle size. 52 The optical band gap for the bimetallic Ag−Co was calculated based on the Tauc equation where h is the Planck constant, ν is the frequency of the vibration, A is the absorption coefficient, E g is the band gap of the semiconductor, and n is a constant, which is 1/2 for a direct transition or 2 for an indirect transition. The Tauc plot (Figure 2b−d) corresponds to two band gap values: the lower band gap value is assigned to d−d spin-allowed transition between Co 3+ and Co 2+ ion and the higher band gap value is originated from p−d charge transfer within Co 3+ and O 2− in Co 3 O 4 . 50,53−55 The dual band gap is the possibility of interband transition in spinel cobalt oxide (Co 3 O 4 ). Ag/ Co 3 O 4 -12 holds a larger band gap value of 1.23 eV possibly because of the quantum particle size confinement that makes the conduction and valence band shifts apart. Fourier transform infrared (FTIR) spectrum shows the absorbance spectrum of monometal and bimetals of Ag−Co ( Figure 3). The vibration in the range of 400−700 cm −1 generally corresponds to metal−oxygen bonding. The vibration spectrum for Ag in this range gets flattened because of the presence of Ag in pure metallic form without any kind of oxygen bonding present in it or because of the possible sintering at higher temperature with increase in fuel ratio. 56,57 In Co spectrum, the two absorption peaks at 652 and 549 cm −1 originate from the stretching vibration of the Co−O bond where Co 2+ (3d 7 ) is tetrahedrally coordinated at 653 cm −1 and Co 3+ (3d 6 ) is octahedrally coordinated at 550 cm −1 confirming the presence of spinel Co 3 O 4 . 58,59 The peak at 1043 cm −1 corresponds to the characteristic vibration of surface bidentate carbonate from the gaseous CO 2 that interacts between the lattice oxygen present in spinel Co 3 O 4 . 60,61

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The weak absorption peak at 835 cm −1 is attributed to the twisting vibrations of unburned carbonyl impurity (O−CO) from the unburned fuel. 62 The absorption band of Ag/Co 3 O 4 -11 is similar to pure Co but with reduced peak intensity, indicating the reduction in the amount of Co on the surface. In Ag/Co 3 O 4 -12, the peak and its intensities are exactly matching with monometallic Co 3 O 4 , which confirms the predominant phase of Co on the surface of the catalyst. The vibration peaks in Ag/Co 3 O 4 -21 tend to merge together, and diminishing the peak intensity could be due to the presence of more metallic Ag. The peaks corresponding to the spinel Co 3 O 4 exist because of the presence of Co with higher molar ratio (1:1.83) in the overall composition.
Scanning electron microscopy (SEM) images display the microstructure of the three synthesized samples ( Figure 4). In all the three cases, a typical structure of SCS-synthesized nanomaterials with porous surface composed of agglomerated NPs is observed. Synthesis conditions tend to affect the particle size and porosity obtained during the SCS process, and a detailed discussion can be found in previously reported articles on the synthesis of Cu−Ni 48

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Article Ag/Co 3 O 4 -21 shows a more uniform size distribution of smaller NPs that agglomerate to form a porous structure ( Figure 4c). At this stage, it is difficult to identify Ag and Co from each other; however, transmission electron microscopy   Figure 6a). This result is expected as in the case of Ag/Co 3 O 4 -12, Co synthesis was carried out on the surface of Ag, leading to a higher content of Co on the surface that reduces the content of surface Ag. Ag spectrum shows the two peaks of Ag 3d 3/2 and Ag 3d 5/2 at 368.1 and 374.1 eV, respectively, with an orbital spin splitting of about 6.1 eV denoting the presence of metallic form of Ag 67 (Figure 6b). There was no apparent shift in the binding energy of Ag in any of the samples, indicating that there is no change in surface Ag oxidation state because of second wave combustion synthesis (SWCS). The XPS spectra for Co 2p do indicate an increase in surface Co present in the Ag/Co 3 O 4 -12 sample (Figure 6c). Surface Co content is anticipated to be higher in the case of Ag/Co 3 O 4 -12 as most of Co will be synthesized on the surface of Ag in SWCS.
On the basis of the XPS peak, the Co surface atomic concentration in three samples decreases as Ag/Co 3 O 4 -12 > Ag/Co 3 O 4 -21 > Ag/Co 3 O 4 -11, whereas in the case of Ag, the content on surface followed a trend of Ag/Co 3 O 4 -21 ≈ Ag/ Co 3 O 4 -11 > Ag/Co 3 O 4 -12. This trend in Co and Ag surface content can be explained in the light of surface carbon content. The presence of carbon is expected in SCS samples because glycine is used as a fuel, and in many cases, complete combustion and removal of carbon are not observed. A quantitative analysis of surface carbon shows the atomic concentration of 29.98, 17.93, and 16.93% for Ag/Co 3 O 4 -11, Ag/Co 3 O 4 -21, and Ag/Co 3 O 4 -12, respectively. The results indicate that a decrease in carbon content in SWSC could be due to the possibility of further combustion of carbon in the second wave of SWCS and subsequent rearrangement of elements on the surface. A higher content of surface carbon in the Ag/Co 3 O 4 -11 sample indicates a lower total metallic content of (Ag + Co) as compared to that in other two samples. This could be the reason why a similar amount of surface Ag is present in Ag/Co 3 O 4 -21 and Ag/Co 3 O 4 -11, whereas Ag/Co 3 O 4 -21 has a higher amount of Co as compared to the Ag/Co 3has O 4 -11 sample. A detailed study by deconvoluting Co 2p peak to estimate the distribution of oxidation states shows the presence of +3 cations at two peaks of 780.2 eV (2p 3/2 ) and 795.6 eV (2p 1/2 ) with a separation of 15.6 eV between them 68 (Figure 6d). Also, the less dominant satellite peaks at 789.5 and 804.5 eV further confirm the existence of Co 3+ cations. 69 71 respectively, that can be represented as follows: The second pair of redox reaction peaks at A 1 and C 1 at 0.7−0.75 V and around 0.5−0.6 V is attributed to the formation and reduction of Ag 2 O 72 as represented below 2Ag 2OH Ag O H O 2e The redox reactions A 2 and C 2 are same for all the three types of catalysts, whereas A 1 and C 1 are different. A clear shift of C 1 in the cathodic direction is visible toward a negative potential in the order of 0.58, 0.54, and 0.51 V for Ag/Co 3 O 4 -21/C, Ag/Co 3 O 4 -11/C, and Ag/Co 3 O 4 -12/C, respectively, is due to the strong interaction of the absorbed oxygenated species and highest for Ag/Co 3 O 4 -12 when compared to other catalysts could be due to the presence of more Co species over the surface. 73 The extra reduction peak of C 3 in O 2 -saturated 1.0 M KOH electrolyte (Figure 7b) is due to the ORR. The cathodic reaction on Ag/Co 3 O 4 -12/C is positively shifted by 0.208 in comparison with Ag/Co 3 O 4 -11/C and Ag/Co 3 O 4 -21/ C. As reported before, the electrochemical activity has been enhanced through the ligand mechanism of charge transfer between the catalyst metals where the Co particles perturb the active sites of Ag NPs. 74,75 The catalytic activities of all the samples were obtained using the linear sweep voltammetry (LSV) measurement at a speed range of 400−1600 rpm in O 2saturated 1.0 M KOH solution (Figure 8a). The activity of the catalyst was determined by the half-wave potential of the ORR curve. The positive shift on the onset potential is more on Ag/ Co 3 O 4 -12/C in comparison with that on Ag/Co 3 O 4 -11/C and Ag/Co 3 O 4 -21/C, and the calculated limiting current density on Ag/Co 3 O 4 -12/C is greater than that of other two Ag−Co catalysts but lower than that of standard Pt/C. Ag/Co 3 O 4 -12/ C shows comparable kinetics with Pt/C. The limiting diffusion current density in the disk increases with the increase in rotation speed for the Ag/Co 3 O 4 -12/C catalyst (Figure 8b). This expected trend is due to the decrease in diffusion barrier that enables an easy pathway for the passage of electrons at high speed.
Levich plot shows ( Figure 8c) the electron transfer that occurs in the overall ORR. The number of electrons transferred is independent of the rotation speed, but they are greatly influenced by the catalytic material used and the reaction environment. The number of electron transfer (n) calculated from the Levich line slope of the catalyst by eq 7 is explained earlier. It is observed that Ag/Co 3 O 4 -12/C results in

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Article the transfer of 3.9 electrons, whereas Ag/Co 3 O 4 -11/C and Ag/ Co 3 O 4 -21/C are involved in 3.7 and 3.8 electron exchange, respectively, at a potential of 0.15 V. The inset bar plot shows the kinetic current density in which Ag/Co 3 O 4 -12/C has the value very close to standard Pt/C. The bifunctionality of the Ag−Co catalyst shows the anodic current (OER) and cathodic current (ORR) for the RDE−LSV experiment at 1600 rpm ( Figure 8d). It was observed that all the samples possess a characteristic peak centered between 0.7 and 1 V NHE, which are attributed to the oxidation of lower state Ag species formed during the linear sweep. 76 These metal oxidations provide active centers with higher valences that could help to improve the OER. In OER, Ag/Co 3 O 4 -12/C has higher anodic current than the other two catalysts. This suggests the rapid transfer of electrons between the electrolyte and the catalyst. An increase in the catalytic activity of the electrochemical reaction for Ag/ Co 3 O 4 -12/C is evident from all the above results. The presence of Co 3 O 4 and CoO in the sample is mentioned in the XRD (Figure 1) and TEM ( Figure 5) analyses, respectively. Cobalt oxide network formed over Ag particles increases the binding energy to the oxygen adsorbed and facilitates the O−O bond splitting. 73 Also, the oxygen adsorbed on Co 3 O 4 is transferred to the adjacent Ag particles and gets reduced there. Likewise, if the rate of oxygen transport to the Ag is higher in Ag/Co 3 O 4 -12/C, it will increase the activity in the ORR and OER.
Tafel plot has proved another way to analyze the electrocatalytic activity and reaction mechanism of electrocatalysts. Mass-transfer-corrected Tafel plot is obtained from the log(J K ) versus V, where J K is the kinetic current density calculated from the modified Koutecky−Levich (KL) eq 6 as shown below: where J and J L are the measured current and mass-corrected limiting current, respectively. Two different linear Tafel slopes were noticed at low and higher overpotentials in each catalyst. Lower slope at lower potential and a slope with larger values at higher overpotential corresponding to Temkin isotherm and Langmuir isotherm are preferred for better reduction mechanism. 77 where η is the overpotential, b the Tafel slope, J the current density, and J ex the exchange current density. The exchange current density J ex values for Ag/Co 3 O 4 -11/C, Ag/Co 3 O 4 -12/ C, and Ag/Co 3 O 4 -21/C are 2.7 × 10 −5 A/cm −2 (5.5 × 10 −4 A/ cm −2 ), 1.06 × 10 −4 A/cm −2 (4.2 × 10 −3 A/cm −2 ), and 4.4 × 10 −5 A/cm −2 (1.3 × 10 −3 A/cm −2 ), respectively, for high overpotentials (low overpotential). J ex provides a strong evidence showing that Ag/Co 3 O 4 -12/C is more sensible for the electric current response with the potential and a promising catalyst for the ORR reaction. Tafel plot for OER corresponding to the three Ag−Co catalysts with the smallest slope for Ag/Co 3 O 4 -12/C displays better catalytic perform-

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Article ance for the water electrolysis reaction (OER) to generate oxygen ( Figure 9b). Overall, the Ag/Co 3 O 4 -12/C catalyst shows the best performance for OER and ORR among the three catalysts tested. Bard and co-workers reported the hypothesis for enhancing the ORR in Ag−Co/C as the ability of breaking O−O bond and the adsorbed O atom was migrated to Ag that causes electroreduction. 79 This is more evident from the shifting of Ag oxide reduction peak in CV toward lower potential (Figure 7) for Ag/Co 3 O 4 -12/C compared to other two Ag/Co 3 O 4 catalysts, which is attributed to the stronger interaction of absorbed oxygen with active Ag sites. This high activity could be ascribed to its synergic coupling between the monometals and a fast charge transport in it. The current state-of-the-art of some selected Ag−Comodified electrodes in terms of onset potential and limiting current densities was compared with Ag/Co 3 O 4 combustion synthesis catalyst (Table 1).

■ CONCLUSIONS
Ag−Co catalysts with three different compositions were synthesized by combustion-based techniques. These NPs were applied for ORR and OER in alkaline medium. Among the three catalysts, the catalyst with high content of Co in Ag/ Co 3 O 4 -12/C displayed better performance for electrocatalytic ORR and OER. In general, the presence of Co oxide on the surface of the Ag/Co 3 O 4 -12/C catalyst is anticipated to enhance the adsorption and transport of oxygen involved in ORR. The Ag atoms in the catalyst activate the O−O bond splitting and increase the reaction kinetics of ORR. High performance for OER can be achieved because of the presence of more active centers with high valence that was generated through the metal oxidation of Ag. All the three catalysts were found to follow the four-electron transfer mechanism for ORR. The catalytic activity of Ag/Co 3 O 4 -12/C for ORR was confirmed with low Tafel slope and lower exchange current density at high potential and high exchange density and larger Tafel slope at lower potentials. Therefore, it can be concluded that Ag/Co 3 O 4 -12/C is a promising catalyst for the application of fuel cell and water electrolysis owing to the presence of more Co atoms on the surface that promote the transfer of oxygen to Ag where it is reduced by releasing electrons.

■ EXPERIMENTAL SECTION
Catalyst Synthesis. All the catalysts in this work were synthesized using the SCS technique. The detailed synthesis procedure is outlined in our previous reports, 48,49,87 explaining the effect of synthesis conditions on the nanomaterials' properties. The bimetallic Ag−Co catalysts were synthesized in three modes as described below using the following metallic ratio: 1.5 g Ag and 1.5 g Co = 1:1 weight ratio and molar ratio of (Ag/Co = 1:1.83).
Mode 1Silver−Cobalt (Ag/Co 3 O 4 -11). Bimetallic Ag− Co was prepared from an aqueous solution of Ag nitrate (AgNO 3 ), Co nitrate (Co(NO 3 ) 2 ·6H 2 O), and glycine (C 2 H 5 NO 2 ) with a fuel ratio (φ) of 1.75. 48 The quantity of metal nitrates and glycine was adjusted to obtain 1.5 g of the solid product (with Ag/Co atomic ratio of 1:1.83) by using the stoichiometric equation reported elsewhere. 40,41,48,88 In the first mode of synthesis, the metal nitrates of Ag and Co along with glycine in desired quantities were dissolved in 25 mL of deionized water (DIW) and kept aside for 1 h to achieve a homogeneous solution. The beaker containing reactive solution was placed on a hotplate heater at 250°C. After sometime, the water evaporates and the reactive mixture temperature increases to reach the self-ignition temperature, where combustion starts and converts the precursor mixture into Ag−Co bimetallic nanopowder in a single step.
Mode 2Silver First Cobalt Second (Ag/Co 3 O 4 -12). In the second mode of synthesis, a two-step SWCS 89 process was utilized. Ag nanopowder was synthesized in the first step by following the procedure of mode 1 using silver nitrate and glycine with a fuel ratio of φ = 1.75. In the second step, the synthesized Ag nanopowder was placed in the solution containing cobalt nitrate and glycine. This mixture, when combusted, is expected to give Co NPs on the surface of Ag NPs. This mode of combustion, termed as SWCS, is illustrated in Scheme 1. SWCS consists of two combustion steps to maximize the surface dispersion of Co on Ag NPs.

Mode 3Cobalt First Silver Second (Ag/Co 3 O 4 -21).
The third mode of synthesis is similar to mode 2 except that Co was synthesized first and Ag later. In this case, Ag content on the surface is expected to be more as compared to other two modes. In all the three cases, the synthesized nanopowder was collected, ground using mortar−pestle, and sieved to get a uniform size of <75 μm agglomerated particles that were used for electrocatalytic testing. These materials were dispersed on carbon black to increase the electrical conductivity to be used on the cathode side of the electrochemical system. A 30 mg of Ag−Co was mixed with 3.5 mL of DIW and sonicated for 1 h; thereafter, 70 mg of carbon black was slowly added in the mixture that was further sonicated for 3 h at 60°C. The wellmixed sample was dried at 110°C until all the water evaporates and the sample becomes dry. The dried sample was further ground to get uniform size.
Material Characterization. The crystalline structure of Ag/Co 3 O 4 was identified using a Rigaku MiniFlexII Desktop X-ray powder diffractometer with a wavelength of Cu Kα radiation and 10−80°scan range. Optical properties of the synthesized catalysts were studied using Thermo Scientific Evolution 300 UV−visible spectroscopy. FTIR spectroscopy (Thermo Nicolet FTIR 6700) spectra of the as-synthesized samples were recorded in the range of 400−1800 cm −1 to understand the chemical bonding on the surface of the catalyst. Morphology of the particles synthesized was analyzed with SEM (Nova Nano 450, FEI). A high-resolution transmission

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Article electron microscope (Tecnai G 2 , F20, FEI) has been used to identify the presence of NPs and its size distribution. XPS (Kratos AXIS Ultra DLD) was used to analyze the elemental composition and the bonding configuration on the surface of bimetallic NPs.
Electrochemical Measurement. Electrochemical activities were measured in a standard three-cell PINE instrument bipotentiostat (WaveDriver 20) with 1 M KOH aqueous electrolyte at the room temperature. A 5 mm diameter glassy electrode was used as the working electrode and Hg/Hg 2 SO 4 single junction electrode and platinum wire were used as reference electrode and counter electrode, respectively. All the potentials are reported relative to the NHE by adding a +0.64 V to the potential versus Hg/Hg 2 SO 4. The working electrode was prepared by dispersing 10 mg of the Ag−Co/C sample in 2.5 mL of water and sonicating it for 1 h. A 20 μL of the dispersed solution was added dropwise on the glassy carbon attached to the Teflon RDE housing (Pine Instruments) that can be connected to the rotator. Once dried, a 20 μL of Nafion (0.125 wt %) solution was dropped on the surface to bind the catalyst over the electrode.
The working electrode was pretreated electrochemically with a scan rate of 500 mV s −1 for 100 cycles in the potential range of −0.8 to 0.2 V before conducting CV experiments. The electrolyte solution was purged by bubbling high-purity N 2 gas for 1 h before conducting CV experiments. CV data were recorded from −0.8 to 0.8 V at a scan rate of 50 mV s −1 . Oxygen reduction and evolution studies were conducted after purging the electrolyte solution with O 2 for 1 h. LSV data were collected at 5 mV s −1 scan rate with a rotation speed ranging from 400 to 1600 rpm. KL plot was analyzed for each sample, and the number of electron transferred (n) was calculated from the slope of the best linear fit based on the KL equation. 90 where J, J L , and J K are measured current densities, diffusionlimited current densities owing to transport, and kinetic current densities related to charge transfer, respectively. Also, ω is the electrode angular rotation velocities, n is the overall electron transfer, F is the Faraday constant (96 485 C mol −1 ), C 0 is the bulk concentration of O 2 dissolved in the electrolyte (7.8 × 10 −7 mol cm −3 for 1 M KOH), v is the kinematic velocity of the electrolyte (0.01 cm 2 s −1 ), D 0 is the O 2 diffusion coefficient (1.9 × 10 −5 cm 2 s −1 ), and k is the electron-