# Morphology and Electrochemical Characterization of Electrodeposited Nanocrystalline Ni-Co Electrodes for Methanol Fuel Cells

Authors: R. Abdel-Karim; M. Ramadan; S. M. El-Raghy
Journal: Journal of Nanomaterials
 (2018)

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## Abstract

An electrocatalytic electrode surface was developed for alcoholic fuel cell by electrodeposition of Ni-Co alloy on a 301 stainless steel substrate. Material characterization by EDX and XRD confirmed deposition of Ni-Co alloy on stainless steel surfaces with a cobalt content of 15–35%. SEM showed nodular and/or angular particles with some subparticles embedded within the coarse nodules. Increasing the deposition current density as well as deposition time leads to deposition of Ni-Co alloys characterized by coarse angular morphology with lower cobalt content. The electrocatalytic activity of the coated electrodes was characterized by potentiodynamic polarization test, electrochemical impedance spectroscopy (EIS), and cyclic voltammetry (CV) tests in anodic solution for electrochemical oxidation of methanol. Polarization study showed very much higher current density for the coated electrode compared to bare stainless steel. According to the EIS test in 1 M methyl alcohol acidic solution, it was found that polarization resistance of the coated sample was much lower compared to the bare substrate. The electrical equivalent circuit at the metal solution interface was found to be matching Randle with Warburg resistance. The results of the CV test showed higher peaks for alcohol oxidation and oxygen reduction compared to the bare substrate. The alloy coating with increased effective surface area leads to enhancement in the electrocatalytic activity of the electrodes. The alloys deposited at current densities of 50 and 80 mA/cm2 for 30 minutes (15–16% Co) had higher catalytic activity of the Ni-Co nanocrystalline deposits for methanol oxidation for direct methanol fuel cells, than those under other deposition conditions.


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## Body

## 1. Introduction

Nowadays, a higher demand for energy is observed [1]. Fuel cells can be considered as a main partner in stationary, transporting, and portable energy sectors [2–6]. Extensive researches were directed to study direct methanol fuel cells due to the easy fuel production from the biomass. Synthesizing fuels from the biomass will be useful for clean energy production to meet the global growing demand of pollution-free renewable energy [7, 8]. In direct methanol fuel cells, fuel is converted electrochemically to electricity avoiding the limitation of the Carnot cycle which limits high-efficiency energy conversion [9, 10]. Woody biomass which is generated from agriculture wastes can be converted to ethanol or ethanol by hydrolysis and subsequent fermentation by microorganisms [11–13]. As the fuel in the fuel cells is oxidized at the anode and the output current is delivered at the cathode, the material and the surface properties of the anode are very important. The main problem here is the polarization of the anode and the cathode which leads to minimization of the output current [14, 15]. For the anode materials, this problem can be solved by using a material of higher electrocatalytic behavior with good electrical conductivity, low polarization resistance, strong biocompatibility, chemical stability, corrosion resistance, good strength, and higher toughness. From the beginning of fuel cell production, the carbon and metallic materials are usually used as the anode due to their excellent properties such as chemical stability, higher electrical conductivity, and lower weight.Pt can be considered as an excellent catalyst for dehydrogenation. The main problems of Pt catalysts are the poisoning by halides and CO, which is produced as a by-product of the used alcohol oxidation, and high cost [16]. Much effort was done to promote CO oxidation and increase the electrocatalysis by alloying some metals such as Os, Sn, Au, W, Pd, Ru, Rh, Pb, Ir, and Bi, to Pt. Platinum-based nanomaterial can achieve a higher surface area with higher active site number. An increase in the active site number leads to an increase in the electrocatalytic behavior of the catalyst towards methanol oxidation and hence an increase in the overall performance of fuel cells [17, 18].Nonplatinum electrocatalysts can be used as an excellent alternative for platinum and platinum-based electrocatalysts. This is due to their lower cost and excellent performance. There is limited research on using Ni-based nonplatinum electrocatalysts containing other elements such as Al, Pd, Sn, and Fe. According to Mohamedi et al. [19], a small addition of Al to Ni produces excellent electrodes in molten carbonate fuel cells. Kumar et al. [20] stated that there is a wide range of composition of Ni-Pd electrodes which used as anode material in methanol oxidative fuel cells in the alkaline medium. Some research studies have discussed the electrocatalytic behavior of nanocrystalline Ni-Co electrodeposits [21–24].Electrodeposition has a lot of advantages over other surface modification techniques such as low cost and capability of manufacturing multicomponent nanocrystalline materials for many energy applications [25–28].In this work, attempts have been made to manufacture Ni-Co electrodes for direct methanol fuel cells on stainless steel substrates by electrodeposition. Electrochemical characterization of these electrodes was made by potentiodynamic polarization test, electrochemical impedance spectroscopy (EIS) test, and cyclic voltammetry (CV) test. The surface morphology and the structural characterization of the deposited electrodes were investigated using scanning electron microscopy (SEM) and X-ray diffraction (XRD), respectively. The elemental composition of the deposited electrodes was performed by energy-dispersive X-ray (EDX).


## 2. Experimental Methods

### 2.1. Testing Material and Pretreatment

The substrate used in the electrodeposition process was 301 stainless steel, delivered in the form of 0.4 mm thick polished sheet for having the chemical analysis as shown in Table1. The specimens were machined to be 4 cm long and 1.5 cm wide. Before electrodeposition, all samples were subjected to electrolytic activation pretreatment in a solution of 60% H2SO4 (wt. percent) at a temperature of 80°C. This was followed by rinsing distilled water in order to remove any traces of chemicals.Table 1
The steel substrate chemical composition.
Element
C
N
Si
V
Cr
Mn
Co
Ni
Fe
wt%
0.0471
0.11
0.643
0.142
18.6
1.32
0.173
7.32
Rem.


### 2.2. Electrodeposition

The electrodeposition cell was composed of a disc-shaped nickel anode and a rectangular stainless steel cathode which were connected to the positive and negative poles of a Chroma 62000P-100-25-type DC power supply with a Chroma 62000P software. The two electrodes were immersed in an electrolyte containing Ni and Co salts in addition to some additives, as illustrated in Table2. All of the bath parameters such as pH, temperature, deposition current density, and deposition time are indicated in Table 2.Table 2
Chemical analysis of electrolytic bath and controlling parameters for electrodeposition of Ni-Co.
Const. bath components and parameters
Concentration in (g/L)
NiSO4·7H2O
177
NiCL2·7H2O
32
CoSO4·7H2O
11
HCHO
25
HCOOH
23
H3BO3
30
Current density (mA/cm2)
30, 50, 80
Deposition time (min)
15, 20, 30
pH
2.5–3
Temperature
21 ± 1°C


### 2.3. XRD Analysis

The type of phases formed in different electrodeposited samples was determined by XRD. The phases contained in the nanocrystalline Ni-Co alloys were examined by an X-ray diffraction unit (X’Pert PRO PANanalytical) with a copper anode (kα=1.540598Å) and using an applied voltage of 45 kV. Data of XRD were based on Bragg’s equation. The crystalline diameter was estimated by Scherrer’s equation using the peak broadening of the most intense peak.


### 2.4. SEM and EDX

The SEM (model Quanta 250 FEG (field emission gun) attached with EDX unit (energy dispersive X-ray analyses), with accelerating voltage 30 KV, magnification 14x up to 1,000,000x and resolution for Gun.1n, was used to examine the microstructure and presented morphology while EDX was used to identify the chemical composition.


### 2.5. Potentiodynamic Polarization

The solution used to characterize the electrocatalytic activity towards methanol oxidation was 1 M methanol +0.5 M H2SO4. The test was performed at room temperature. Electrochemical measurements were conducted using a VoltaLab 10 potentiostat coupled with PGZ 100 analyst software, controlled by a personal computer in conventional three-electrode-cell systems. The working electrode was the steel substrate or Ni-Co-coated electrode, the auxiliary electrode was the Pt electrode, and the reference electrode was the saturated calomel electrode (SCE). Prior to the potentiodynamic test, the samples were immersed in corrosive medium for 30 min to obtain the open circuit potential “EOCP.” After the stabilization of EOCP, the upper and lower potential limits were fixed to ±300 mV with respect to EOCP, with a scanning rate of 0.33 mV/s. Tafel’s plot obtained from polarization studies was displayed, and the corrosion potential Ecorr and corrosion current density Icorr were deduced from the plot. The Stern-Geary equation [29] is as follows:
(1)Icorr=βa/βc2.303βa+βc⋅1Rp,where βa and βc are Tafel’s constants expressed as V/dec and Rp is the polarization resistance in Ω·cm2, was employed to determine the corrosion current Icorr.


### 2.6. EIS and CV

A Gamry potentiostat instrument coupled with a computer software (Gamry software (Series G 300)) was used to draw the Bode and Nyquist plot. Impedance measurements were conducted in the frequency range of 25 kHz to 10 mHz, and an amplitude of 10 mV was applied in the open circuit potential. The following information is obtained from EIS tests. The values of the solution resistance “Ru”, polarization resistance “Rp”, double-layer capacitance “Cdl”, constant phase element “CPE (Y),” and α are defined from the capacitive impedance equation
(2)Z=1Cjw−α.Capacitors in EIS experiments often do not behave ideally. Instead, they act like a constant phase element (CPE). The exponentα is 1 for the ideal capacitance. For a constant phase element, the exponent α is less than one. The “double-layer capacitor” on real cells often behaves like a CPE instead of like an ideal capacitor [14].The same setup and software were used to obtain the cyclic voltammetry CV curves. The applied range of potential was 0.1 to 1.1 on an Ag/AgCl scale with a scanning rate of 100 mV/s.


## 2.1. Testing Material and Pretreatment

The substrate used in the electrodeposition process was 301 stainless steel, delivered in the form of 0.4 mm thick polished sheet for having the chemical analysis as shown in Table1. The specimens were machined to be 4 cm long and 1.5 cm wide. Before electrodeposition, all samples were subjected to electrolytic activation pretreatment in a solution of 60% H2SO4 (wt. percent) at a temperature of 80°C. This was followed by rinsing distilled water in order to remove any traces of chemicals.Table 1
The steel substrate chemical composition.
Element
C
N
Si
V
Cr
Mn
Co
Ni
Fe
wt%
0.0471
0.11
0.643
0.142
18.6
1.32
0.173
7.32
Rem.


## 2.2. Electrodeposition

The electrodeposition cell was composed of a disc-shaped nickel anode and a rectangular stainless steel cathode which were connected to the positive and negative poles of a Chroma 62000P-100-25-type DC power supply with a Chroma 62000P software. The two electrodes were immersed in an electrolyte containing Ni and Co salts in addition to some additives, as illustrated in Table2. All of the bath parameters such as pH, temperature, deposition current density, and deposition time are indicated in Table 2.Table 2
Chemical analysis of electrolytic bath and controlling parameters for electrodeposition of Ni-Co.
Const. bath components and parameters
Concentration in (g/L)
NiSO4·7H2O
177
NiCL2·7H2O
32
CoSO4·7H2O
11
HCHO
25
HCOOH
23
H3BO3
30
Current density (mA/cm2)
30, 50, 80
Deposition time (min)
15, 20, 30
pH
2.5–3
Temperature
21 ± 1°C


## 2.3. XRD Analysis

The type of phases formed in different electrodeposited samples was determined by XRD. The phases contained in the nanocrystalline Ni-Co alloys were examined by an X-ray diffraction unit (X’Pert PRO PANanalytical) with a copper anode (kα=1.540598Å) and using an applied voltage of 45 kV. Data of XRD were based on Bragg’s equation. The crystalline diameter was estimated by Scherrer’s equation using the peak broadening of the most intense peak.


## 2.4. SEM and EDX

The SEM (model Quanta 250 FEG (field emission gun) attached with EDX unit (energy dispersive X-ray analyses), with accelerating voltage 30 KV, magnification 14x up to 1,000,000x and resolution for Gun.1n, was used to examine the microstructure and presented morphology while EDX was used to identify the chemical composition.


## 2.5. Potentiodynamic Polarization

The solution used to characterize the electrocatalytic activity towards methanol oxidation was 1 M methanol +0.5 M H2SO4. The test was performed at room temperature. Electrochemical measurements were conducted using a VoltaLab 10 potentiostat coupled with PGZ 100 analyst software, controlled by a personal computer in conventional three-electrode-cell systems. The working electrode was the steel substrate or Ni-Co-coated electrode, the auxiliary electrode was the Pt electrode, and the reference electrode was the saturated calomel electrode (SCE). Prior to the potentiodynamic test, the samples were immersed in corrosive medium for 30 min to obtain the open circuit potential “EOCP.” After the stabilization of EOCP, the upper and lower potential limits were fixed to ±300 mV with respect to EOCP, with a scanning rate of 0.33 mV/s. Tafel’s plot obtained from polarization studies was displayed, and the corrosion potential Ecorr and corrosion current density Icorr were deduced from the plot. The Stern-Geary equation [29] is as follows:
(1)Icorr=βa/βc2.303βa+βc⋅1Rp,where βa and βc are Tafel’s constants expressed as V/dec and Rp is the polarization resistance in Ω·cm2, was employed to determine the corrosion current Icorr.


## 2.6. EIS and CV

A Gamry potentiostat instrument coupled with a computer software (Gamry software (Series G 300)) was used to draw the Bode and Nyquist plot. Impedance measurements were conducted in the frequency range of 25 kHz to 10 mHz, and an amplitude of 10 mV was applied in the open circuit potential. The following information is obtained from EIS tests. The values of the solution resistance “Ru”, polarization resistance “Rp”, double-layer capacitance “Cdl”, constant phase element “CPE (Y),” and α are defined from the capacitive impedance equation
(2)Z=1Cjw−α.Capacitors in EIS experiments often do not behave ideally. Instead, they act like a constant phase element (CPE). The exponentα is 1 for the ideal capacitance. For a constant phase element, the exponent α is less than one. The “double-layer capacitor” on real cells often behaves like a CPE instead of like an ideal capacitor [14].The same setup and software were used to obtain the cyclic voltammetry CV curves. The applied range of potential was 0.1 to 1.1 on an Ag/AgCl scale with a scanning rate of 100 mV/s.


## 3. Results and Discussions

### 3.1. Morphology of the Deposits

The effect of current density on the surface morphology of Ni-Co layers is presented in Figures1–3. At 30 mA/cm2 (Figure 1), the morphology of the deposited alloys changed with time from nodular to angular as the time increased from 15 minutes to 30 minutes. The particle size increases with increasing deposition time due to the enough time given for particles to grow [30]. Similarly, at 50 mA/cm2 (Figure 2), nodular morphology was observed at deposition time of 15 minutes. At 20 minutes, the morphology turned into a mixture of nodular and angular particles and became fully angular by increasing the deposition time further to 30 minutes. At 80 mA/cm2, the SEM results at 40 KX (Figure 3) illustrated a relatively small particle size embedded within the coarse nodules. An increase in overpotential enhances the rate of nucleation and produces a small particle size [31–37].Figure 1
SEM micrographs of nanocrystalline Ni-Co alloys electrodeposited at 30 mA/cm2: (a) 15 min, (b) 20 min, and (c) 30 min.
(a)
(b)
(c)Figure 2
SEM micrographs of nanocrystalline Ni-Co alloys electrodeposited at 50 mA/cm2: (a) 15 min, (b) 20 min, and (c) 30 min.
(a)
(b)
(c)Figure 3
SEM micrographs of nanocrystalline Ni-Co alloys electrodeposited at 80 mA/cm2: (a) 15 min, (b) 20 min, and (c) 30 min.
(a)
(b)
(c)


### 3.2. EDX Analysis

The chemical composition of nanocrystalline Ni-Co alloys electrodeposited by various applied current densities and deposition time is shown in Table2. At 30 mA/cm2, by increasing the deposition time from 15 minutes to 30 minutes, the cobalt content is decreasing from 37 to 29 wt%. This is due to the depletion of Co2+ in the solution or due to the lower deposition efficiency of Co than that of Ni and hence a decrease in the ratio of Co2+/(Ni2+ + Co2+) [24, 38]. Similarly, at 50 mA/cm2, the cobalt content decreased from 33 to 17.24 wt% as the deposition time increased from 15 to 30 minutes. The same trend was recognized by increasing the current density further to 80 mA/cm2, where the cobalt content dropped down to 15.8 wt%, by increasing the deposition time up to 30 minutes.The effect of the deposition current densities as well as deposition time on the % Co content is also summarized in Table3 and Figure 4. According to Rafailović et al. [39], an increase in the current density leads to an increase in the overpotential which is combined by an increase in the activation of the electrode reaction. This leads to a higher nickel content in the Ni-Co deposits.Table 3
EDX analysis of electrodeposited nanocrystalline Ni-Co layers.
Current density (mA/cm2)
Time (min)
Composition
% Ni
% Co
30
15
63.08
36.92
20
62.22
37.78
30
70.56
29.44
50
15
66.86
33.14
20
73.86
26.23
30
82.93
17.07
80
15
83.16
16.84
20
83.47
16.53
30
84.9
15.1Figure 4
The effect deposition time as well as the current density on the Co content of electrodeposited nanocrystalline Ni-Co alloys.


### 3.3. X-Ray Diffraction

Figure5 shows an example of the XRD pattern for electrodeposited nanocrystalline Ni-Co alloys. Two sharp peaks for all XRD patterns were detected at 2θ around 44° and 52°. Their main textures are (111) and (200). These high peaks suggest that the Ni-Co alloy deposits are considered crystalline in structure. In agreement with other research [33, 37, 40–42], the obtained peaks indicated the deposition of a one-phase Ni-Co solid solution (α) with a face-centered cubic structure. According to the Ni-Co equilibrium phase diagram, the structure consists of the α phase, which is a substitutional solid solution of Ni and Co and the structure was face-centered cubic (fcc). When the Co content increases to 50%, the fcc phase turns to a mixed crystalline structure of fcc and hcp [43].Figure 5
XRD pattern of electrodeposited layer of nanocrystalline Ni-Co alloys.∗w, >30 mA/cm2; x, >50 mA/cm2; y, >80 mA/cm2; 1, > 15 min; 2, > 20 min; 3, >30 min.From Figure4, Ni-Co coatings with higher cobalt contents were obtained under lower current density and less deposition time conditions. In agreement with Yang and Deng [44], the intensity of the main XRD peaks increases and the peak width is broader, indicating a decrease in grain size with higher Co content.The effect of the current density and deposition time on the crystalline size is illustrated in Figure6. Generally, a crystalline size ranging from 21 nm to 30 nm was obtained. The crystalline size increased slightly with increase in the deposition time at all the deposition current densities due to the presence of enough time for some coarsening of the grains [41]. The effect of the deposition current density on crystalline size is shown in Figure 6. The crystalline size decreased when the deposition current density increased. This is due to the effect of the overpotential. A higher overpotential is needed for a higher current density. An increase in the overpotential leads to an increase in the nucleation rate and hence a reduction in the crystalline size [39, 45].Figure 6
The effect of the deposition time as well as the current density on the crystalline size of the electrodeposited nanocrystalline Ni-Co alloys.


### 3.4. Potentiodynamic Polarization Test

Figure7 displays the polarization of the steel substrate and the deposited nanocrystalline Ni-Co alloys at different current densities and times. From the figure, the anodic branches for all the curves exhibited higher activity or higher current densities than those of the substrate.Figure 7
Potentiodynamic polarization curves for the nanocrystalline Ni-Co deposits in 1 M methyl alcohol acidic solution.
(a)
30 mA/cm2
(b)
50 mA/cm2
(c)
80 mA/cm2The various electrochemical parameters (βa, βc, Ecorr, Icorr, and Rp) estimated from experimental data are illustrated in Table 4. The corrosion potential of stainless steel substrate Ecorr was observed to be −231 mV. It should be mentioned that a positive shift of Ecorr values was observed for coated samples. The shift observed was −52.2 mV for layers containing 15% Co. These layers were deposited at current density 80 mA/cm2 for 30 min.Table 4
Corrosion properties of nanocrystalline electrodeposited Ni-Co alloys and the steel substrate in 1 M methanol + 0.5 M H2SO4.
Time (min)
βa
βc
Ecorr (mV)
Icorr (μA/cm2)
Corrosion rate (μm/y)
Rp (KΩ)
30 mA/cm2
15
40.5
37.5
−205.9
6.64
71.59
1.12
20
47.7
48
−162
5.93
63.95
3.27
30
37.7
33
−156.1
5.04
54.33
1.99
50 mA/cm2
15
24.9
41.6
−188
5.61
60.53
0.999
20
25.9
42.8
−104
4.71
50.78
1.240
30
27.6
36.7
−97.4
3.40
36.73
1.540
80 mA/cm2
15
27.4
40
−116
3.53
38.11
1.95
20
17.1
31.6
−85
2.47
26.73
0. 846
30
10.4
29.2
−52.2
2.37
25.62
1.82
Stainless steel substrate
—
13.58
34.2
−231
1.53
11.73
8.36At 30 mA/cm2, the values of the corrosion current densities were changed. A slight reduction in corrosion current densities, from 6.64 to 5 μA/cm2, with increase in deposition time at constant deposition current density was due to the coarsening of the particle size and hence the small electroactive surface area [43, 46]. The Co content values were 37 and 33% for deposition times 15 and 30 minutes, respectively. In addition, the corrosion resistance of the nanocrystalline Ni-Co alloys can be changed by altering the Co content [47]. Srivastava et al. [48] reported poor corrosion behavior of cobalt-rich coatings by increasing the Co content beyond 20%. At 50 mA/cm2, a further reduction in Icorr from 5.6 to 3.4 μA/cm2 was detected with the increase in deposition time. The Co content and the resulting particle size had their effect as interpreted in the case of 30 mA/cm2. Similarly, at 80 mA/cm2, the corrosion current dropped down to 2.4 μA/cm2. This can be due to the lower Co content obtained at that deposition current density, when compared with the other deposition current densities, for all deposition time periods [49].In agreement with Kharmachi et al [45], the value of Icorr was decreased and a better corrosion resistance was obtained in the case of nickel-rich deposits. For example, the corrosion rate for Ni-Co containing 37% Co was 71.59 μm/y compared to 26 μm/y for a layer containing 16% Co.Paul and Naimuddin [50] stated that the polarization curves for coated materials shift to the right in comparison to a bare stainless steel surface, which indicates that Ni-Co coatings always produce higher current.According to Naimuddin [51], the higher Icorr as well as corrosion rate values for Ni-Co deposits (≅ 72–26 μm/y), compared with that of the substrate (11 μm/y), are due only to the oxidation of methanol and not due to any corrosion of the nanocrystalline Ni-Co alloy surface. Electrodeposition of Ni-Co alloys on stainless steel substrate has been carried out to obtain a high current density electrocatalytic surface with minimum polarization resistance for the anodic oxidation reaction of methyl alcohol. Generally, the nanocrystalline Ni-Co alloys showed lower polarization resistance (1–3.27 KΩ) than that of the steel substrate (8.36 KΩ). This is an evidence for the higher electrochemical activity and ease in charge transfer between the nanocrystalline Ni-Co alloys and the used electrolyte than that of the steel substrate of higher polarization resistance [51].Methanol electrooxidation is a complex reaction occurring in a pattern of parallel reaction pathways [50, 52]. Although detailed reaction mechanisms remain obscure, a number of reaction intermediates and products have been identified. The complete oxidation of methanol yields CO2 and six electrons per methanol molecule as shown in (3). Methanol has a low theoretical oxidation potential (0.02 V) comparable to that of hydrogen (0.0 V), and in principle, it can be an efficient fuel at low temperatures.
(3)CH3OHL+H2Ol→CO2g+6H++6e−.H+ generated during oxidation of methyl alcohol gets diffused into a cathodic chamber through the membrane and supplies H+ ions for the cathodic reduction reaction of O2 to pure water [50].


### 3.5. EIS Test

Figure8 shows the impedance plots of the nanocrystalline Ni-Co alloys deposited at 30 mA/cm2 and the steel substrate. In agreement with many previous publications [50–53], the substrate had a larger diameter arc in the Nyquist plots (Figure 8(a)) and higher modulus impedance in the Bode plots (Figure 8(b)), with a more positive phase angle (Figure 8(c)) than those of the electrodeposited nanocrystalline Ni-Co electrodes. This means that Ni-Co electrodes had lower impedance to charge transfer than the steel substrate when being subjected to methyl alcohol. The phase angle of the deposited nanocrystalline Ni-Co electrodes was in the range of −10 to −70 degrees compared to a range from 0 to near −90 degrees for the steel substrate. This is due to the fact that when using the steel substrate, the double layer acts as a pure capacitive load for charge transfer. Meanwhile, in case of using the Ni-Co electrodes, the matter is different and lower impedance to charge transfer occurs.Figure 8
EIS plots of the nanocrystalline Ni-Co alloys deposited at 30 mA/cm2 and the steel substrate tested in 1 m methyl alcohol acidic solution.
(a)
Nyquist plot
(b)
Bode plot (impedance modulus versus the frequency)
(c)
Bode plot (phase angle with the frequency)
(d)
Equivalent circuit model of the electrochemical interfaceFrom Table5, it can be concluded that Ni-Co layers showed significantly lower polarization resistance than the stainless steel substrates did. In addition, using a current density of 30 mA/cm2, the polarization resistance did not have a clear trend and was in the range of 1.82 to 3.09 KΩ. At a current density of 50 mA/cm2, the polarization resistance decreased with increasing deposition time and was in the range of 1.71 to 7.99 KΩ, which is lower than that of the steel substrate (103 KΩ). A similar trend was observed using a current density 80 mA/cm2. The polarization resistance was in the range of 1.8 to 8 KΩ, which is also lower than that of the steel substrate [54, 55]. The specimen deposited at 50 mA/cm2 for 30 minutes showed the lowest polarization value (1.71 KΩ), which corresponds to the highest electrocatalytic activity for hydrogen evolution.Table 5
The EIS results of all electrodeposited nanocrystalline Ni-Co alloys tested in 1 M methanol + 0.5 M H2SO4.
Time (min)
Rp (KΩ)
Ru (Ω)
Y (μF/cm2)
α
30 mA/cm2
15
1.82
7.917
63.5
0.88
20
3.09
7.178
63.3
0.86
30
2.39
7.714
35.9
0.86
50 mA/cm2
15
7.99
7.425
15.6
0.85
20
2.64
7.31
18.8
0.86
30
1.71
6.969
22.8
0.89
80 mA/cm2
15
3.6
7.137
51.8
0.843
20
2.27
6.916
27.8
0.845
30
2.53
7.122
37.5
0.814
Stainless steel substrate
—
103
7.271
42. 9
0.89The solution resistance (Ru) was changed in all the specimens by a small degree due to the use of the same methanol electrolyte. There is no uniform behavior in the constant phase element (CPE) values with varying deposition current densities or deposition times. The exponent α was changed in a small range from 0.845 to 0.89. According to Paul and Naimuddin [50], this exponent exists due to the nonideal behavior of the double-phase capacitance. The electric circuit which models the interface is shown in Figure 8(d).


### 3.6. CV Test

Methanol oxidation was examined on nanocrystalline Ni-Co electrodes by CV measurements, and results are shown in Table6 and Figure 9. Methanol electrooxidation on the catalysts electrodes showed two oxidation peaks in the forward and reverse sweeps. In the forward scan, the observed peak is related to the oxidation of freshly chemisorbed species coming from methanol adsorption. In the backward sweep, the oxidation corresponds to removal of the carbonaceous species (CO gas) that have not completely oxidized in the forward scan. The oxidation of intermediate, mainly CO, is shown in [56]
(4)Ni−COads+Co−OHads→CO2+H++e−Table 6
The results obtained from the CV curves performed to nanocrystalline Ni-Co deposits 1 M methanol + 0.5 M H2SO4.
Time (min)
Eonset (mV)
Ep (V)
Jp (mA/cm2)
IfIb
30 mA/cm2
15
−0.445
0.318
3.15
5.03
20
−0.438
0.370
6.20
16.40
30
−0.545
0.358
9.25
26.27
50 mA/cm2
15
−0.348
0.292
16.5
40.24
20
−0.438
0.361
14.27
17.29
30
−0.545
0.31
29.6
64.20
80 mA/cm2
15
−0.445
0.229
5.417
10.74
20
−0.349
0.292
24.38
93.05
30
−0.445
0.468
33.3
59.73118Figure 9
The CV curves for electrodeposited nanocrystalline Ni-Co alloys samples prepared at different current densities, in 1 M methanol acidic solution.
(a)
30 mA/cm2
(b)
50 mA/cm2
(c)
80 mA/cm2At 30 mA/cm2 (Figure 9(a)), the effect of the deposition time on forward peak current densities is very clear. An increase in the deposition time from 15 to 30 min leads to an increase in Jp from 3.15 to 9.25 mA/cm2, due to an increase in the electrochemical active surface area by the presence of subparticles on the relatively larger particles [57]. Longer deposition was also accompanied by reduction in the cobalt content. According to Xu et al. [58], a decrease in Co content leads to an increase in the forward peak current. The broadening of the peaks at 15 and 30 minutes provided a wide a range of potential to achieve the highest current density.Similar trends were observed, at 50 mA/cm2 (Figure 9(b)) and 80 mA/cm 2. The longer the deposition time, the higher the forward-to-backward ratio. This means higher efficiency of the electrodeposited nanocrystalline Ni-Co electrodes for more methanol electrooxidation and excellent oxidation of the strongly adsorbed CO on the surface of the electrode.Figure10 shows the effect of the deposition time as well the deposition current density on the forward peak current density (Jp) of electrodeposited nanocrystalline Ni-Co electrodes. An increase in the deposition time and current density resulted in a higher forward peak current density Jp and thus higher electrocatalytic activity of Ni-Co deposits.Figure 10
The effect of the deposition time as well as the deposition current density on the forward peak current density, obtained from CV curves conducted for nanocrystalline Ni-Co alloys, in 1 M methanol acidic solution.


## 3.1. Morphology of the Deposits

The effect of current density on the surface morphology of Ni-Co layers is presented in Figures1–3. At 30 mA/cm2 (Figure 1), the morphology of the deposited alloys changed with time from nodular to angular as the time increased from 15 minutes to 30 minutes. The particle size increases with increasing deposition time due to the enough time given for particles to grow [30]. Similarly, at 50 mA/cm2 (Figure 2), nodular morphology was observed at deposition time of 15 minutes. At 20 minutes, the morphology turned into a mixture of nodular and angular particles and became fully angular by increasing the deposition time further to 30 minutes. At 80 mA/cm2, the SEM results at 40 KX (Figure 3) illustrated a relatively small particle size embedded within the coarse nodules. An increase in overpotential enhances the rate of nucleation and produces a small particle size [31–37].Figure 1
SEM micrographs of nanocrystalline Ni-Co alloys electrodeposited at 30 mA/cm2: (a) 15 min, (b) 20 min, and (c) 30 min.
(a)
(b)
(c)Figure 2
SEM micrographs of nanocrystalline Ni-Co alloys electrodeposited at 50 mA/cm2: (a) 15 min, (b) 20 min, and (c) 30 min.
(a)
(b)
(c)Figure 3
SEM micrographs of nanocrystalline Ni-Co alloys electrodeposited at 80 mA/cm2: (a) 15 min, (b) 20 min, and (c) 30 min.
(a)
(b)
(c)


## 3.2. EDX Analysis

The chemical composition of nanocrystalline Ni-Co alloys electrodeposited by various applied current densities and deposition time is shown in Table2. At 30 mA/cm2, by increasing the deposition time from 15 minutes to 30 minutes, the cobalt content is decreasing from 37 to 29 wt%. This is due to the depletion of Co2+ in the solution or due to the lower deposition efficiency of Co than that of Ni and hence a decrease in the ratio of Co2+/(Ni2+ + Co2+) [24, 38]. Similarly, at 50 mA/cm2, the cobalt content decreased from 33 to 17.24 wt% as the deposition time increased from 15 to 30 minutes. The same trend was recognized by increasing the current density further to 80 mA/cm2, where the cobalt content dropped down to 15.8 wt%, by increasing the deposition time up to 30 minutes.The effect of the deposition current densities as well as deposition time on the % Co content is also summarized in Table3 and Figure 4. According to Rafailović et al. [39], an increase in the current density leads to an increase in the overpotential which is combined by an increase in the activation of the electrode reaction. This leads to a higher nickel content in the Ni-Co deposits.Table 3
EDX analysis of electrodeposited nanocrystalline Ni-Co layers.
Current density (mA/cm2)
Time (min)
Composition
% Ni
% Co
30
15
63.08
36.92
20
62.22
37.78
30
70.56
29.44
50
15
66.86
33.14
20
73.86
26.23
30
82.93
17.07
80
15
83.16
16.84
20
83.47
16.53
30
84.9
15.1Figure 4
The effect deposition time as well as the current density on the Co content of electrodeposited nanocrystalline Ni-Co alloys.


## 3.3. X-Ray Diffraction

Figure5 shows an example of the XRD pattern for electrodeposited nanocrystalline Ni-Co alloys. Two sharp peaks for all XRD patterns were detected at 2θ around 44° and 52°. Their main textures are (111) and (200). These high peaks suggest that the Ni-Co alloy deposits are considered crystalline in structure. In agreement with other research [33, 37, 40–42], the obtained peaks indicated the deposition of a one-phase Ni-Co solid solution (α) with a face-centered cubic structure. According to the Ni-Co equilibrium phase diagram, the structure consists of the α phase, which is a substitutional solid solution of Ni and Co and the structure was face-centered cubic (fcc). When the Co content increases to 50%, the fcc phase turns to a mixed crystalline structure of fcc and hcp [43].Figure 5
XRD pattern of electrodeposited layer of nanocrystalline Ni-Co alloys.∗w, >30 mA/cm2; x, >50 mA/cm2; y, >80 mA/cm2; 1, > 15 min; 2, > 20 min; 3, >30 min.From Figure4, Ni-Co coatings with higher cobalt contents were obtained under lower current density and less deposition time conditions. In agreement with Yang and Deng [44], the intensity of the main XRD peaks increases and the peak width is broader, indicating a decrease in grain size with higher Co content.The effect of the current density and deposition time on the crystalline size is illustrated in Figure6. Generally, a crystalline size ranging from 21 nm to 30 nm was obtained. The crystalline size increased slightly with increase in the deposition time at all the deposition current densities due to the presence of enough time for some coarsening of the grains [41]. The effect of the deposition current density on crystalline size is shown in Figure 6. The crystalline size decreased when the deposition current density increased. This is due to the effect of the overpotential. A higher overpotential is needed for a higher current density. An increase in the overpotential leads to an increase in the nucleation rate and hence a reduction in the crystalline size [39, 45].Figure 6
The effect of the deposition time as well as the current density on the crystalline size of the electrodeposited nanocrystalline Ni-Co alloys.


## 3.4. Potentiodynamic Polarization Test

Figure7 displays the polarization of the steel substrate and the deposited nanocrystalline Ni-Co alloys at different current densities and times. From the figure, the anodic branches for all the curves exhibited higher activity or higher current densities than those of the substrate.Figure 7
Potentiodynamic polarization curves for the nanocrystalline Ni-Co deposits in 1 M methyl alcohol acidic solution.
(a)
30 mA/cm2
(b)
50 mA/cm2
(c)
80 mA/cm2The various electrochemical parameters (βa, βc, Ecorr, Icorr, and Rp) estimated from experimental data are illustrated in Table 4. The corrosion potential of stainless steel substrate Ecorr was observed to be −231 mV. It should be mentioned that a positive shift of Ecorr values was observed for coated samples. The shift observed was −52.2 mV for layers containing 15% Co. These layers were deposited at current density 80 mA/cm2 for 30 min.Table 4
Corrosion properties of nanocrystalline electrodeposited Ni-Co alloys and the steel substrate in 1 M methanol + 0.5 M H2SO4.
Time (min)
βa
βc
Ecorr (mV)
Icorr (μA/cm2)
Corrosion rate (μm/y)
Rp (KΩ)
30 mA/cm2
15
40.5
37.5
−205.9
6.64
71.59
1.12
20
47.7
48
−162
5.93
63.95
3.27
30
37.7
33
−156.1
5.04
54.33
1.99
50 mA/cm2
15
24.9
41.6
−188
5.61
60.53
0.999
20
25.9
42.8
−104
4.71
50.78
1.240
30
27.6
36.7
−97.4
3.40
36.73
1.540
80 mA/cm2
15
27.4
40
−116
3.53
38.11
1.95
20
17.1
31.6
−85
2.47
26.73
0. 846
30
10.4
29.2
−52.2
2.37
25.62
1.82
Stainless steel substrate
—
13.58
34.2
−231
1.53
11.73
8.36At 30 mA/cm2, the values of the corrosion current densities were changed. A slight reduction in corrosion current densities, from 6.64 to 5 μA/cm2, with increase in deposition time at constant deposition current density was due to the coarsening of the particle size and hence the small electroactive surface area [43, 46]. The Co content values were 37 and 33% for deposition times 15 and 30 minutes, respectively. In addition, the corrosion resistance of the nanocrystalline Ni-Co alloys can be changed by altering the Co content [47]. Srivastava et al. [48] reported poor corrosion behavior of cobalt-rich coatings by increasing the Co content beyond 20%. At 50 mA/cm2, a further reduction in Icorr from 5.6 to 3.4 μA/cm2 was detected with the increase in deposition time. The Co content and the resulting particle size had their effect as interpreted in the case of 30 mA/cm2. Similarly, at 80 mA/cm2, the corrosion current dropped down to 2.4 μA/cm2. This can be due to the lower Co content obtained at that deposition current density, when compared with the other deposition current densities, for all deposition time periods [49].In agreement with Kharmachi et al [45], the value of Icorr was decreased and a better corrosion resistance was obtained in the case of nickel-rich deposits. For example, the corrosion rate for Ni-Co containing 37% Co was 71.59 μm/y compared to 26 μm/y for a layer containing 16% Co.Paul and Naimuddin [50] stated that the polarization curves for coated materials shift to the right in comparison to a bare stainless steel surface, which indicates that Ni-Co coatings always produce higher current.According to Naimuddin [51], the higher Icorr as well as corrosion rate values for Ni-Co deposits (≅ 72–26 μm/y), compared with that of the substrate (11 μm/y), are due only to the oxidation of methanol and not due to any corrosion of the nanocrystalline Ni-Co alloy surface. Electrodeposition of Ni-Co alloys on stainless steel substrate has been carried out to obtain a high current density electrocatalytic surface with minimum polarization resistance for the anodic oxidation reaction of methyl alcohol. Generally, the nanocrystalline Ni-Co alloys showed lower polarization resistance (1–3.27 KΩ) than that of the steel substrate (8.36 KΩ). This is an evidence for the higher electrochemical activity and ease in charge transfer between the nanocrystalline Ni-Co alloys and the used electrolyte than that of the steel substrate of higher polarization resistance [51].Methanol electrooxidation is a complex reaction occurring in a pattern of parallel reaction pathways [50, 52]. Although detailed reaction mechanisms remain obscure, a number of reaction intermediates and products have been identified. The complete oxidation of methanol yields CO2 and six electrons per methanol molecule as shown in (3). Methanol has a low theoretical oxidation potential (0.02 V) comparable to that of hydrogen (0.0 V), and in principle, it can be an efficient fuel at low temperatures.
(3)CH3OHL+H2Ol→CO2g+6H++6e−.H+ generated during oxidation of methyl alcohol gets diffused into a cathodic chamber through the membrane and supplies H+ ions for the cathodic reduction reaction of O2 to pure water [50].


## 3.5. EIS Test

Figure8 shows the impedance plots of the nanocrystalline Ni-Co alloys deposited at 30 mA/cm2 and the steel substrate. In agreement with many previous publications [50–53], the substrate had a larger diameter arc in the Nyquist plots (Figure 8(a)) and higher modulus impedance in the Bode plots (Figure 8(b)), with a more positive phase angle (Figure 8(c)) than those of the electrodeposited nanocrystalline Ni-Co electrodes. This means that Ni-Co electrodes had lower impedance to charge transfer than the steel substrate when being subjected to methyl alcohol. The phase angle of the deposited nanocrystalline Ni-Co electrodes was in the range of −10 to −70 degrees compared to a range from 0 to near −90 degrees for the steel substrate. This is due to the fact that when using the steel substrate, the double layer acts as a pure capacitive load for charge transfer. Meanwhile, in case of using the Ni-Co electrodes, the matter is different and lower impedance to charge transfer occurs.Figure 8
EIS plots of the nanocrystalline Ni-Co alloys deposited at 30 mA/cm2 and the steel substrate tested in 1 m methyl alcohol acidic solution.
(a)
Nyquist plot
(b)
Bode plot (impedance modulus versus the frequency)
(c)
Bode plot (phase angle with the frequency)
(d)
Equivalent circuit model of the electrochemical interfaceFrom Table5, it can be concluded that Ni-Co layers showed significantly lower polarization resistance than the stainless steel substrates did. In addition, using a current density of 30 mA/cm2, the polarization resistance did not have a clear trend and was in the range of 1.82 to 3.09 KΩ. At a current density of 50 mA/cm2, the polarization resistance decreased with increasing deposition time and was in the range of 1.71 to 7.99 KΩ, which is lower than that of the steel substrate (103 KΩ). A similar trend was observed using a current density 80 mA/cm2. The polarization resistance was in the range of 1.8 to 8 KΩ, which is also lower than that of the steel substrate [54, 55]. The specimen deposited at 50 mA/cm2 for 30 minutes showed the lowest polarization value (1.71 KΩ), which corresponds to the highest electrocatalytic activity for hydrogen evolution.Table 5
The EIS results of all electrodeposited nanocrystalline Ni-Co alloys tested in 1 M methanol + 0.5 M H2SO4.
Time (min)
Rp (KΩ)
Ru (Ω)
Y (μF/cm2)
α
30 mA/cm2
15
1.82
7.917
63.5
0.88
20
3.09
7.178
63.3
0.86
30
2.39
7.714
35.9
0.86
50 mA/cm2
15
7.99
7.425
15.6
0.85
20
2.64
7.31
18.8
0.86
30
1.71
6.969
22.8
0.89
80 mA/cm2
15
3.6
7.137
51.8
0.843
20
2.27
6.916
27.8
0.845
30
2.53
7.122
37.5
0.814
Stainless steel substrate
—
103
7.271
42. 9
0.89The solution resistance (Ru) was changed in all the specimens by a small degree due to the use of the same methanol electrolyte. There is no uniform behavior in the constant phase element (CPE) values with varying deposition current densities or deposition times. The exponent α was changed in a small range from 0.845 to 0.89. According to Paul and Naimuddin [50], this exponent exists due to the nonideal behavior of the double-phase capacitance. The electric circuit which models the interface is shown in Figure 8(d).


## 3.6. CV Test

Methanol oxidation was examined on nanocrystalline Ni-Co electrodes by CV measurements, and results are shown in Table6 and Figure 9. Methanol electrooxidation on the catalysts electrodes showed two oxidation peaks in the forward and reverse sweeps. In the forward scan, the observed peak is related to the oxidation of freshly chemisorbed species coming from methanol adsorption. In the backward sweep, the oxidation corresponds to removal of the carbonaceous species (CO gas) that have not completely oxidized in the forward scan. The oxidation of intermediate, mainly CO, is shown in [56]
(4)Ni−COads+Co−OHads→CO2+H++e−Table 6
The results obtained from the CV curves performed to nanocrystalline Ni-Co deposits 1 M methanol + 0.5 M H2SO4.
Time (min)
Eonset (mV)
Ep (V)
Jp (mA/cm2)
IfIb
30 mA/cm2
15
−0.445
0.318
3.15
5.03
20
−0.438
0.370
6.20
16.40
30
−0.545
0.358
9.25
26.27
50 mA/cm2
15
−0.348
0.292
16.5
40.24
20
−0.438
0.361
14.27
17.29
30
−0.545
0.31
29.6
64.20
80 mA/cm2
15
−0.445
0.229
5.417
10.74
20
−0.349
0.292
24.38
93.05
30
−0.445
0.468
33.3
59.73118Figure 9
The CV curves for electrodeposited nanocrystalline Ni-Co alloys samples prepared at different current densities, in 1 M methanol acidic solution.
(a)
30 mA/cm2
(b)
50 mA/cm2
(c)
80 mA/cm2At 30 mA/cm2 (Figure 9(a)), the effect of the deposition time on forward peak current densities is very clear. An increase in the deposition time from 15 to 30 min leads to an increase in Jp from 3.15 to 9.25 mA/cm2, due to an increase in the electrochemical active surface area by the presence of subparticles on the relatively larger particles [57]. Longer deposition was also accompanied by reduction in the cobalt content. According to Xu et al. [58], a decrease in Co content leads to an increase in the forward peak current. The broadening of the peaks at 15 and 30 minutes provided a wide a range of potential to achieve the highest current density.Similar trends were observed, at 50 mA/cm2 (Figure 9(b)) and 80 mA/cm 2. The longer the deposition time, the higher the forward-to-backward ratio. This means higher efficiency of the electrodeposited nanocrystalline Ni-Co electrodes for more methanol electrooxidation and excellent oxidation of the strongly adsorbed CO on the surface of the electrode.Figure10 shows the effect of the deposition time as well the deposition current density on the forward peak current density (Jp) of electrodeposited nanocrystalline Ni-Co electrodes. An increase in the deposition time and current density resulted in a higher forward peak current density Jp and thus higher electrocatalytic activity of Ni-Co deposits.Figure 10
The effect of the deposition time as well as the deposition current density on the forward peak current density, obtained from CV curves conducted for nanocrystalline Ni-Co alloys, in 1 M methanol acidic solution.


## 4. Conclusion

An increase in the deposition current density as well as deposition time leads to deposition of Ni-Co alloys characterized by a coarse angular morphology with lower cobalt content. Generally, a crystalline size ranging from 21 nm to 30 nm was obtained. The crystal size increased slightly with the increase in the deposition time at all the deposition current densities. The obtained XRD peaks indicated the deposition of a one-phase Ni-Co solid solution (α) with a face-centered cubic structure. The corrosion resistance of the nanocrystalline Ni-Co alloys has been changed by altering the Co content. The higher Icorr values for Ni-Co deposits, compared with those of the substrate, are due only to oxidation of methanol and not due to any corrosion of the nanocrystalline Ni-Co alloy surface. According to the EIS test, the deposited nanocrystalline Ni-Co alloy had less impedance to charge transfer through the interface. The appearance of the forward and backward peaks in the CV test means high activity to methanol oxidation and higher resistance to CO poisoning. The longer the deposition time, the higher the forward-to-backward ratio and hence the higher the efficiency of the electrodeposited nanocrystalline Ni-Co electrodes for more methanol electrooxidation and excellent oxidation of the strongly adsorbed CO on the surface of the electrode. An increase in the deposition time as well as the current density resulted in a higher forward peak current density Jp and thus higher electrocatalytic activity of Ni-Co deposits.



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*Source: 9870732-2018-08-07.xml*