# Preparation and Electrocatalytic Characteristics Research of Pd/C Catalyst for Direct Ethanol Fuel Cell

Authors: Qiao Xia Li; Ming Shuang Liu; Qun Jie Xu; Hong Min Mao
Journal: Journal of Chemistry
 (2013)

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## Abstract

Two kinds of carbon-support 20% Pd/C catalysts for use in direct ethanol fuel cell (DEFC) have been prepared by an impregnation reduction method using NaBH4 and NaH2PO2 as reductants, respectively, in this study. The catalysts were characterized by XRD and TEM. The results show that the catalysts had been completely reduced, and the catalysts are spherical and homogeneously dispersed on carbon. The electrocatalytic activity of the catalysts was investigated by electrochemical measurements. The results indicate that the catalysts had an average particle size of 3.3 nm and showed the better catalytic performance, when NaBH4 was used as the reducing agent. The electrochemical active surface area of Pd/C (NaBH4) was 56.4 m2·g−1. The electrochemical activity of the Pd/C (NaBH4) was much higher than that of Pd/C (NaH2PO2).


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## Body

## 1. Introduction

Nowadays, great attention has been paid to direct alcohol fuel cell (DAFC) as portable applications due to some superior advantages over analogous devices fed with hydrogen. Direct ethanol fuel cell (DEFC) has attracted attention, since ethanol has no toxicity comparing to methanol and can be easily produced in great quantities by the fermentation of sugar-containing raw materials [1, 2]. The electroactivity of anodic materials is one of the main factors influencing the practical application of DAFC. Although platinum electrodes present efficient catalytic activity for alcohol oxidation, the widely practical application of Pt electrodes as anodes in DAFC is limited by the high cost of the metal platinum. If DAFC could be operated in an alkaline instead of an acidic electrolyte, it is easy to consider that the kinetics of fuel cells will be significantly improved and Pt-free electrocatalysts can be used. It is reported that Pd is a good electrocatalyst for ethanol oxidation and showed higher activity than that of Pt in alkaline media [3, 4].Recently, nanoparticle palladium has recently received much attention due to some distinguished advantages of it such as significantly large surface areas and high stability. Wen et al. [5] prepared Pd/SnO2-GNS catalysts by a microwave-assisted reduction process. It was found that, compared with Pd/GNS, the Pd/SnO2-GNS catalyst showed superior electrocatalytic activity for ethanol oxidation. The interest in Pd not only is for the purpose to lower the cost of catalysts but pursuits an improved catalytic activity. One method to promote the catalytic activity of Pd is alloying with another metal, such as Ag and Sn [6–9]. Liu et al. [10] synthesized PdNi nanoparticles by a chemical reduction process with formic acid. Zhou et al.  [11] studied the electrooxidation of ethanol on a polycrystalline Pd disk electrode in alkaline media in situ Fourier transform infrared (FTIR) reflection spectroscopy. The selectivity for ethanol oxidation to CO2 (existing as CO32- in alkaline media) was determined as low as 2.5% in the potential region where Pd electrode exhibited considerable electrocatalytic activity (−0.60 to 0.0 V versus SCE). Nevertheless, the ability of Pd for breaking C–C bond in ethanol is still slightly better than that of Pt under the same conditions.In the present work, we prepared two different nanoparticle Pd/C electrocatalysts using NaBH4 and NaH2PO2 as reductants, respectively, to investigate the nanoparticle palladium towards ethanol oxidation reaction (EOR) in alkaline solution. In addition, we have also probed the electrochemical properties of the electrocatalysts to explore their potential applications in DEFC.


## 2. Experimental

### 2.1. Instrumentation

XRD patterns were collected using a Bruker D8-Advance Powder X-ray diffractometer (Cu KR radiation, wavelength 1.5418 Å). Transmission electron microscopy (TEM) images were characterized with a JEM-2100F HR-TEM model using an accelerating voltage of 80 and 200 KV. 10.0 mg catalyst was dissolved in aqua regia (a strong acid mixture with HCl : HNO3 volume ratio of 3 : 1) to form a Pd aqueous solution, and ICP-AES was performed to detect the catalyst metal loading. All electrochemical measurements were performed in a standard three-electrode cell using a CHI 660C Electrochemical Analyzer.


### 2.2. Reagents and Solutions

All reagents used were of high purity and analytical reagent grade. PdCl2 was purchased from the Shanghai Institute of Fine Chemical Materials (China); Vulcan XC-72 was supplied by Cabot Co. Ltd. (USA); Sodium borohydride (96%, NaBH4), Sodium hypophosphite hydrate (NaH2PO2·H2O), Trisodium citrate dehydrate (C6H5Na3O7·2H2O) ethanol, and ethylene glycol were from Sinopharm Chemical Reagent Co. Ltd. 5% Nafion solution was from DuPont Co. Ltd (USA); all other reagents were of analytical grade and used without further purification. The water utilized in all studies was double distilled and deionized.


### 2.3. Catalyst Preparation

XC-72 carbon was treated in 5 M HNO3 solution with vigorous stirring. 40.0 mg of the prepared carbon and 2 mmol L−1 PdCl2 aqueous solution were added in a mixture of deionized water and ethylene glycol (V/V, 3 : 1). The mixture was stirred for 1 h. After that, the appropriate amount of C6H5Na3O7 ·2H2O was added into the mixture as stabilizing agent and then put into an ultrasonic bath, keeping the temperature at 50°C for 0.5 h in continuous ultrasonic concussion. Subsequently, adjust pH to 11 using 1 M NaOH aqueous solution; excess amounts of 0.01 M NaBH4 (freshly prepared) were added into the mixtures dropwise. After being stirred for 6 h at 50°C, the mixture was filtered and washed several times with deionized water to completely remove all excess reducing agents. The remaining solids were dried in a vacuum oven for 24 h at 80°C. The final catalyst was Pd/C (NaBH4). Pd/C (NaH2PO2) was prepared by the similar method using Sodium hypophosphite hydrate as a reducing agent. The weight percentage of Pd was 20% in both catalysts.


### 2.4. Electrochemical Measurements

Cyclic voltammetry (CV) and chronoamperometry measurements were collected in 1 M KOH + 1 M ethanol solution at a scan rate of 50 mV·s−1. The working electrodes were prepared by dropping 4 μL of the electrocatalyst onto glassy carbon electrode (GCE, 0.07 cm2). The ink was prepared by ultrasonically mixing 5 mg of electrocatalyst sample in a mixture of 1 mL of ethanol and 120 μL of 5% Nafion solution. The counter electrode was large Pt foils, and the reference electrode was saturated calomel electrode (SCE). The CV tests were carried out in the potential range of −0.8 to 0.4 V. Before experiments, pure nitrogen gas (99.99%) was bubbled through the solution at the last 30 min to remove the dissolved oxygen in the solution. CO striping voltammetric measurements were performed as follows: after purging the solution with N2 for 30 min, gaseous CO was bubbled for 30 min to form CO adlayer on catalysts while maintaining potential at −0.6 V. Excess CO in solution was purged with N2 for 2 h and CO stripping voltammetry was recorded in 1 M KOH at 50 mV·s−1. All experiments were carried out at ambient temperature (~25°C).


## 2.1. Instrumentation

XRD patterns were collected using a Bruker D8-Advance Powder X-ray diffractometer (Cu KR radiation, wavelength 1.5418 Å). Transmission electron microscopy (TEM) images were characterized with a JEM-2100F HR-TEM model using an accelerating voltage of 80 and 200 KV. 10.0 mg catalyst was dissolved in aqua regia (a strong acid mixture with HCl : HNO3 volume ratio of 3 : 1) to form a Pd aqueous solution, and ICP-AES was performed to detect the catalyst metal loading. All electrochemical measurements were performed in a standard three-electrode cell using a CHI 660C Electrochemical Analyzer.


## 2.2. Reagents and Solutions

All reagents used were of high purity and analytical reagent grade. PdCl2 was purchased from the Shanghai Institute of Fine Chemical Materials (China); Vulcan XC-72 was supplied by Cabot Co. Ltd. (USA); Sodium borohydride (96%, NaBH4), Sodium hypophosphite hydrate (NaH2PO2·H2O), Trisodium citrate dehydrate (C6H5Na3O7·2H2O) ethanol, and ethylene glycol were from Sinopharm Chemical Reagent Co. Ltd. 5% Nafion solution was from DuPont Co. Ltd (USA); all other reagents were of analytical grade and used without further purification. The water utilized in all studies was double distilled and deionized.


## 2.3. Catalyst Preparation

XC-72 carbon was treated in 5 M HNO3 solution with vigorous stirring. 40.0 mg of the prepared carbon and 2 mmol L−1 PdCl2 aqueous solution were added in a mixture of deionized water and ethylene glycol (V/V, 3 : 1). The mixture was stirred for 1 h. After that, the appropriate amount of C6H5Na3O7 ·2H2O was added into the mixture as stabilizing agent and then put into an ultrasonic bath, keeping the temperature at 50°C for 0.5 h in continuous ultrasonic concussion. Subsequently, adjust pH to 11 using 1 M NaOH aqueous solution; excess amounts of 0.01 M NaBH4 (freshly prepared) were added into the mixtures dropwise. After being stirred for 6 h at 50°C, the mixture was filtered and washed several times with deionized water to completely remove all excess reducing agents. The remaining solids were dried in a vacuum oven for 24 h at 80°C. The final catalyst was Pd/C (NaBH4). Pd/C (NaH2PO2) was prepared by the similar method using Sodium hypophosphite hydrate as a reducing agent. The weight percentage of Pd was 20% in both catalysts.


## 2.4. Electrochemical Measurements

Cyclic voltammetry (CV) and chronoamperometry measurements were collected in 1 M KOH + 1 M ethanol solution at a scan rate of 50 mV·s−1. The working electrodes were prepared by dropping 4 μL of the electrocatalyst onto glassy carbon electrode (GCE, 0.07 cm2). The ink was prepared by ultrasonically mixing 5 mg of electrocatalyst sample in a mixture of 1 mL of ethanol and 120 μL of 5% Nafion solution. The counter electrode was large Pt foils, and the reference electrode was saturated calomel electrode (SCE). The CV tests were carried out in the potential range of −0.8 to 0.4 V. Before experiments, pure nitrogen gas (99.99%) was bubbled through the solution at the last 30 min to remove the dissolved oxygen in the solution. CO striping voltammetric measurements were performed as follows: after purging the solution with N2 for 30 min, gaseous CO was bubbled for 30 min to form CO adlayer on catalysts while maintaining potential at −0.6 V. Excess CO in solution was purged with N2 for 2 h and CO stripping voltammetry was recorded in 1 M KOH at 50 mV·s−1. All experiments were carried out at ambient temperature (~25°C).


## 3. Results and Discussion

### 3.1. TEM

Figure1 shows typical TEM images of the Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts. The catalysts prepared by the reduction method are spherical and homogeneously dispersed on Vulcan XC-72 with no remarkable observation of agglomerations. The average diameters of both catalysts are also summarized in  Table 1. They are 3.3 and 38.0 nm for Pd/C (NaBH4) and Pd/C (NaH2PO2). Obviously, Pd/C (NaBH4) has a smaller particle size than Pd/C (NaH2PO2).Table 1
Summary of physical properties of Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts.
Catalyst
Pd metal loading detected by ICP-AES
Diameter calculated form XRD/nm
Diameter measured by TEM/nm
Pd/C (NaBH4)
21.6%
2.8
3.3
Pd/C (NaH2PO2)
23.8%
3.4
38.0TEM images and particle size distributions of Pd/C (NaBH4) (a) and Pd/C (NaH2PO2) (b).
(a)
(b)


### 3.2. XRD

The X-ray diffraction (XRD) patterns of the Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts are shown in Figure 2. Sharp and well-defined peaks of Pd/C (NaH2PO2) are observed at 2θ values of 40.14°, 46.69°, 68.17°, 82.17°, and 86.69°corresponding to planes of (1 1 1), (2 0 0), (2 2 0), (3 1 1), and (2 2 2), respectively, according to JCPDS No.65-6174. The strong diffraction peaks of Pd/C (NaBH4) are also found in the same angles, but the plane of (2 2 2) disappears. Combined with the TEM images, it is indicated that the crystalline structure of palladium was obtained, respectively, using NaBH4 and NaH2PO2 as reductants.Figure 2
XRD patterns of Pd/C (NaBH4) and Pd/C (NaH2PO2).The average particle size of the nanoparticles (d) was estimated by using Scherrer equation (1) after background subtraction from (1 1 1) peak at 2θ of  ~40° [12]:
(1)d=kλβcosθ,
where k is the coefficient, generally taken as 0.9, λ  is wavelength of X-ray radiation equal to 1.5418 Å, β  is full width at half maximum (FWHM) measured in radians, and θ is the angle measured at the position of platinum peaks. Table 1 shows the crystalline size of the electrocatalysts.


### 3.3. Electrochemical Measurements

Cyclic voltammetry was used to quantify the electrocatalytic activities of the Pd/C as prepared for room temperature. Figure3 shows the CV results of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 C2H5OH + 1 mol·L−1 KOH solution. The scan rate was selected at 50 mV·s−1 in the potential range from −0.8 to 0.4 V. The oxidation peak in the forward scan is corresponding to the oxidation of freshly chemisorbed species coming from ethanol adsorption. At a higher potential, the formation of PdO will block further adsorption of reactive species and lead to a remarkable decrease in current. During the negative-going sweep, the previously formed PdO will be reduced to catalytic active Pd, thus, leading to the recovery of EOR current. Corresponding reactions are shown in (2) and (3) [13]:
(2)Pd+C2H5OH+3OH-⟷Pd-CH3COads+3H2O+3e(3)Pd-CH3COads+Pd-OHads+OH-→2Pd+CH3COO-+H2OFigure 3
Voltammetric curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 C2H5OH + 1 mol·L−1 KOH solution.It is observed from Figure3 that the current density on Pd/C (NaBH4) is obviously higher, compared with that on Pd/C (NaH2PO2). It shows that the Pd/C (NaBH4) catalyst has a better catalytic activity. In the forward scan, the onset potential (Eonset) of Pd/C (NaBH4) is −0.544 V, which have negatively shifts by ~30 mV as compared to that of Pd/C (NaH2PO2) (−0.516 V). The peak current densities are 28.8 and 17.4 mA·cm−2 (the area is the surface area of the electrode) for Pd/C (NaBH4) and Pd/C (NaH2PO2), respectively, while their peak potentials are −0.258 and −0.232 V. The following parameters, including the Eonset, the forward peak potential (Ep), and the forward peak current intensity (jp) expressed in mA·cm−2, are shown in Table 2. At the same time, the peak current density of Pd/C (NaBH4) is higher than that of Pd/C in [7, 14].Table 2
Comparison of activity of ethanol oxidation between Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts.
Catalyst
E
onset
/
V
E
p
/
V
j
p/mA·cm−2
EASA/ m2·g−1
Pd/C (NaBH4)
−0.544
−0.258
28.8
56.4
Pd/C (NaH2PO2)
−0.516
−0.232
17.4
51.2When compared to NaH2PO2 reduction method, the NaBH4 reduction method shows a great advantage in improving the EOR activity. The main reason is that NaBH4 exhibits a higher reduction rate; it is beneficial to maintain high saturation degree during the nucleation stage at the beginning of reaction. On the other hand, the concentrations of BH4- and H2PO2- decide the reduction ability of NaBH4 and NaH2PO2, respectively. In alkaline condition, the hydrolysis of BH4- is inhibited, (4), but the hydrolysis of H2PO2- is promoted, (5):
(4)BH4-+2H2O=BO2-+4H2↑(5)H2PO2-+OH-=HBO22-+H2↑
The cyclic voltammetry of Pd/C (NaBH4) and Pd/C (NaH2PO2) in the absence of ethanol is shown in Figure 4. It is observed from Figure 4 that they exhibit significantly high anodic and cathodic current densities. The oxidation peak at lower anodic potential during the forward scan is ascribed to the formation of the adsorbed hydroxyl OHads while this at high positive potential is related to the formation of Pd oxides [15, 16]. On the cathodic scan, the palladium oxide layers are reduced, with reduction peaks at −0.512 and −0.431, respectively. The potential region from −1.1 to −0.7 V versus SCE on the CV curve of the catalyst is associated with the hydrogen adsorption/desorption. The electrochemical active surface areas (EASA) of catalysts were measured by integrating the charge on hydrogen adsorption-desorption regions by cyclic voltammetry. These values given in Table 1 can be calculated after the deduction of the double layer region on the CV curves represents the charge passed for the hydrogen desorption. The electrochemical active surface areas (EASA) for Pd/C (NaBH4) and Pd/C (NaH2PO2) were calculated to be 56.4 and 51.2 m2·g−1, respectively (Table 2). Obviously, Pd/C (NaBH4) shows a better electrochemical activity because of higher EASA.Figure 4
Voltammetric curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 KOH solution.In order to evaluate the stability of the catalysts, chronoamperometry was employed and results are shown in Figure5. The present results show that the current densities represent less decay at the applied constant potentials for a long duration (3600 s). It can be observed that the current densities on the Pd/C (NaBH4) and Pd/C (NaH2PO2) after 3600 s are 0.6 and 0.1 mA·cm−2, indicating that the Pd/C (NaBH4) exhibits a better stable electrocatalytic activity towards ethanol oxidation in the alkaline media than Pd/C (NaH2PO2). The results are in accordance with the CV results.Figure 5
Chronoamperometry curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 C2H5OH + 1 mol·L−1 KOH solution at a fixed potential of −300 mV for 3600 s.CO striping voltammetric curves are shown in Figure6. The CO striping measurements are conducted in 1 M KOH. It is observed from Pd/C (NaBH4) (solid line) that an anodic peak with a shoulder an the high potential side appears in the potential from −0.3 to −0.1 V. In contrast to Pd/C (NaBH4), the Pd/C (NaH2PO2) (dash line) possesses a smaller CO stripping peak, indicating that a less amount of CO molecules adsorb on the active surface of Pd/C (NaH2PO2). Moreover, the simple and sharp line profile of the stripping peak observed for the Pd/C (NaBH4) demonstrates that the structure of the sample is relatively homogeneous [17]. After stripping, sharp peaks of two CV curves are disappeared in the 2nd cycle. It indicates that the CO preadsorbed on the surface of electrocatalysts is thoroughly oxidized in the first potential scan and the active sites on the Pd surface recover again.Figure 6
CO striping voltammetric curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 KOH solution.CO has been commonly identified as an intermediate, and the major poisonous species in the alcohol oxidation process, that is prone to adsorb on the surface active sites of electrocatalysts, has been widely used as an effective method to evaluate the active surface area of electrocatalysts [18].


## 3.1. TEM

Figure1 shows typical TEM images of the Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts. The catalysts prepared by the reduction method are spherical and homogeneously dispersed on Vulcan XC-72 with no remarkable observation of agglomerations. The average diameters of both catalysts are also summarized in  Table 1. They are 3.3 and 38.0 nm for Pd/C (NaBH4) and Pd/C (NaH2PO2). Obviously, Pd/C (NaBH4) has a smaller particle size than Pd/C (NaH2PO2).Table 1
Summary of physical properties of Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts.
Catalyst
Pd metal loading detected by ICP-AES
Diameter calculated form XRD/nm
Diameter measured by TEM/nm
Pd/C (NaBH4)
21.6%
2.8
3.3
Pd/C (NaH2PO2)
23.8%
3.4
38.0TEM images and particle size distributions of Pd/C (NaBH4) (a) and Pd/C (NaH2PO2) (b).
(a)
(b)


## 3.2. XRD

The X-ray diffraction (XRD) patterns of the Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts are shown in Figure 2. Sharp and well-defined peaks of Pd/C (NaH2PO2) are observed at 2θ values of 40.14°, 46.69°, 68.17°, 82.17°, and 86.69°corresponding to planes of (1 1 1), (2 0 0), (2 2 0), (3 1 1), and (2 2 2), respectively, according to JCPDS No.65-6174. The strong diffraction peaks of Pd/C (NaBH4) are also found in the same angles, but the plane of (2 2 2) disappears. Combined with the TEM images, it is indicated that the crystalline structure of palladium was obtained, respectively, using NaBH4 and NaH2PO2 as reductants.Figure 2
XRD patterns of Pd/C (NaBH4) and Pd/C (NaH2PO2).The average particle size of the nanoparticles (d) was estimated by using Scherrer equation (1) after background subtraction from (1 1 1) peak at 2θ of  ~40° [12]:
(1)d=kλβcosθ,
where k is the coefficient, generally taken as 0.9, λ  is wavelength of X-ray radiation equal to 1.5418 Å, β  is full width at half maximum (FWHM) measured in radians, and θ is the angle measured at the position of platinum peaks. Table 1 shows the crystalline size of the electrocatalysts.


## 3.3. Electrochemical Measurements

Cyclic voltammetry was used to quantify the electrocatalytic activities of the Pd/C as prepared for room temperature. Figure3 shows the CV results of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 C2H5OH + 1 mol·L−1 KOH solution. The scan rate was selected at 50 mV·s−1 in the potential range from −0.8 to 0.4 V. The oxidation peak in the forward scan is corresponding to the oxidation of freshly chemisorbed species coming from ethanol adsorption. At a higher potential, the formation of PdO will block further adsorption of reactive species and lead to a remarkable decrease in current. During the negative-going sweep, the previously formed PdO will be reduced to catalytic active Pd, thus, leading to the recovery of EOR current. Corresponding reactions are shown in (2) and (3) [13]:
(2)Pd+C2H5OH+3OH-⟷Pd-CH3COads+3H2O+3e(3)Pd-CH3COads+Pd-OHads+OH-→2Pd+CH3COO-+H2OFigure 3
Voltammetric curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 C2H5OH + 1 mol·L−1 KOH solution.It is observed from Figure3 that the current density on Pd/C (NaBH4) is obviously higher, compared with that on Pd/C (NaH2PO2). It shows that the Pd/C (NaBH4) catalyst has a better catalytic activity. In the forward scan, the onset potential (Eonset) of Pd/C (NaBH4) is −0.544 V, which have negatively shifts by ~30 mV as compared to that of Pd/C (NaH2PO2) (−0.516 V). The peak current densities are 28.8 and 17.4 mA·cm−2 (the area is the surface area of the electrode) for Pd/C (NaBH4) and Pd/C (NaH2PO2), respectively, while their peak potentials are −0.258 and −0.232 V. The following parameters, including the Eonset, the forward peak potential (Ep), and the forward peak current intensity (jp) expressed in mA·cm−2, are shown in Table 2. At the same time, the peak current density of Pd/C (NaBH4) is higher than that of Pd/C in [7, 14].Table 2
Comparison of activity of ethanol oxidation between Pd/C (NaBH4) and Pd/C (NaH2PO2) catalysts.
Catalyst
E
onset
/
V
E
p
/
V
j
p/mA·cm−2
EASA/ m2·g−1
Pd/C (NaBH4)
−0.544
−0.258
28.8
56.4
Pd/C (NaH2PO2)
−0.516
−0.232
17.4
51.2When compared to NaH2PO2 reduction method, the NaBH4 reduction method shows a great advantage in improving the EOR activity. The main reason is that NaBH4 exhibits a higher reduction rate; it is beneficial to maintain high saturation degree during the nucleation stage at the beginning of reaction. On the other hand, the concentrations of BH4- and H2PO2- decide the reduction ability of NaBH4 and NaH2PO2, respectively. In alkaline condition, the hydrolysis of BH4- is inhibited, (4), but the hydrolysis of H2PO2- is promoted, (5):
(4)BH4-+2H2O=BO2-+4H2↑(5)H2PO2-+OH-=HBO22-+H2↑
The cyclic voltammetry of Pd/C (NaBH4) and Pd/C (NaH2PO2) in the absence of ethanol is shown in Figure 4. It is observed from Figure 4 that they exhibit significantly high anodic and cathodic current densities. The oxidation peak at lower anodic potential during the forward scan is ascribed to the formation of the adsorbed hydroxyl OHads while this at high positive potential is related to the formation of Pd oxides [15, 16]. On the cathodic scan, the palladium oxide layers are reduced, with reduction peaks at −0.512 and −0.431, respectively. The potential region from −1.1 to −0.7 V versus SCE on the CV curve of the catalyst is associated with the hydrogen adsorption/desorption. The electrochemical active surface areas (EASA) of catalysts were measured by integrating the charge on hydrogen adsorption-desorption regions by cyclic voltammetry. These values given in Table 1 can be calculated after the deduction of the double layer region on the CV curves represents the charge passed for the hydrogen desorption. The electrochemical active surface areas (EASA) for Pd/C (NaBH4) and Pd/C (NaH2PO2) were calculated to be 56.4 and 51.2 m2·g−1, respectively (Table 2). Obviously, Pd/C (NaBH4) shows a better electrochemical activity because of higher EASA.Figure 4
Voltammetric curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 KOH solution.In order to evaluate the stability of the catalysts, chronoamperometry was employed and results are shown in Figure5. The present results show that the current densities represent less decay at the applied constant potentials for a long duration (3600 s). It can be observed that the current densities on the Pd/C (NaBH4) and Pd/C (NaH2PO2) after 3600 s are 0.6 and 0.1 mA·cm−2, indicating that the Pd/C (NaBH4) exhibits a better stable electrocatalytic activity towards ethanol oxidation in the alkaline media than Pd/C (NaH2PO2). The results are in accordance with the CV results.Figure 5
Chronoamperometry curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 C2H5OH + 1 mol·L−1 KOH solution at a fixed potential of −300 mV for 3600 s.CO striping voltammetric curves are shown in Figure6. The CO striping measurements are conducted in 1 M KOH. It is observed from Pd/C (NaBH4) (solid line) that an anodic peak with a shoulder an the high potential side appears in the potential from −0.3 to −0.1 V. In contrast to Pd/C (NaBH4), the Pd/C (NaH2PO2) (dash line) possesses a smaller CO stripping peak, indicating that a less amount of CO molecules adsorb on the active surface of Pd/C (NaH2PO2). Moreover, the simple and sharp line profile of the stripping peak observed for the Pd/C (NaBH4) demonstrates that the structure of the sample is relatively homogeneous [17]. After stripping, sharp peaks of two CV curves are disappeared in the 2nd cycle. It indicates that the CO preadsorbed on the surface of electrocatalysts is thoroughly oxidized in the first potential scan and the active sites on the Pd surface recover again.Figure 6
CO striping voltammetric curves of Pd/C (NaBH4) and Pd/C (NaH2PO2) in 1 mol·L−1 KOH solution.CO has been commonly identified as an intermediate, and the major poisonous species in the alcohol oxidation process, that is prone to adsorb on the surface active sites of electrocatalysts, has been widely used as an effective method to evaluate the active surface area of electrocatalysts [18].


## 4. Conclusions

In summary, two different 20 wt% nanoparticle Pd/C electrocatalysts were prepared with NaBH4 and NaH2PO2 as reductants, respectively. Pd/C (NaBH4) catalysts have small average diameter (3.3 nm) and large electrochemical surface areas (56.4 m2·g−1). Therefore, Pd/C (NaBH4) exhibits higher reactivity toward EOR in alkaline electrolyte, compared to Pd/C (NaH2PO2). The CV tests show that the Eonset on Pd/C (NaBH4) is more negative than that of Pd/C (NaH2PO2); the peak current densities of Pd/C (NaBH4) (28.8 mA·cm−2) are higher than those of Pd/C (NaH2PO2) (17.4 mA·cm−2). After a 3600 s chronoamperometry test at −0.3 V, Pd/C (NaBH4) exhibits a better stable electrocatalytic activity towards ethanol oxidation in the alkaline media than Pd/C (NaH2PO2).



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*Source: 250760-2013-02-24.xml*