# Hydrogen Storage and Release Properties of a Cu-Added Fe/YSZ Redox System

Authors: Hyo-Sub Kim; Dong-Hee Lee; Hong-Soon Kim; Chu-Sik Park; Young-Ho Kim
Journal: Journal of Nanomaterials
 (2013)

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## Abstract

Hydrogen storage and release by the redox reaction of an iron oxide with yttria-stabilized zirconia (YSZ) were investigated. YSZ was introduced to the samples to improve the thermal stability of the iron oxide. The average size of the samples synthesized using urea was 40–50 nm, whereas those synthesized using Na2CO3 as a precipitant were 150–200 nm. The sample prepared via coprecipitation using urea exhibited better stability than the other samples. We prepared the Cu-added Fe/YSZ sample to enhance the low-temperature reactivity. The water-splitting reaction was initiated at approximately 200°C, and the maximum rate of hydrogen evolution was observed at approximately 350°C. In the isothermal redox test over 35 cycles, the degree of hydrogen storage and release was almost maintained over 1.8 wt% based on the total amount of the sample.


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## Body

## 1. Introduction

Hydrogen production, storage, and utilization have been widely studied in an effort to solve the depletion of fossil fuels and environmental problems [1, 2]. Hydrogen can be produced from various processes such as the steam methane reforming, water electrolysis, gasification of coal and biomass, and water splitting by high temperature heat [3]. The hydrogen storage technologies are the physical storage methods, such as compressed gas storage and liquid storage, and the chemical storage methods, such as metal hydrides and chemical hydrides [4, 5]. Among the various methods of hydrogen utilization, the polymer electrolyte membrane fuel cell (PEMFC) is well known to be the most suitable for automobile applications due to high power density and quick start-up. The hydrogen for operating the PEMFC requires the very low tolerance of CO that affects the Pt catalyst by the poisoning. Otsuka et al. [6] proposed a system for the chemical storage and release of hydrogen to supply CO-free hydrogen to the PEMFC. The concept of this system is consistent with the conventional steam-iron process using the redox reaction of iron oxide. The first step in this system involves the reduction of Fe3O4 using hydrogen (1). In the second step, the Fe is oxidized by water vapor (2) as follows:Step 1.
Hydrogen reduction (hydrogen storage)(1)Fe3O4+4H2⟶3Fe+4H2OStep 2.
Water-splitting oxidation (hydrogen release)(2)3Fe+4H2O⟶Fe3O4+4H2The theoretical quantity of stored hydrogen is 4.8 wt% based on 1 g Fe in this system. A high temperature (approximately 400°C) is required for the hydrogen evolution step. The iron oxide exhibits low stability because the particles aggregate during the reactions causing a deactivation. To prevent this deactivation, many researchers have investigated the thermal stability and reactivity by introducing foreign metals or metal oxides. Ostuka et al. [6] reported that Ga, V, Cr, and Mo are favorable additives for accelerating the redox reaction. Takenaka et al. [7] reported that Rh enhances the rate of hydrogen formation for iron oxides and Mo prevents the sintering of the iron particles. In addition, Wang et al. [8] reported that adding Mo to the iron oxide could improve the rate of hydrogen formation.In our previous work [9–12], we investigated the effect of Zr-based mixed oxides (i.e., ZrO2, CeO2, or Ce-ZrO2) as promising supporters or binders for preventing the aggregation of iron oxide during the redox reaction. Yttria-stabilized zirconia (YSZ) is reportedly a promising catalyst or supporting material due to its high thermal stability and its stability under reducing and oxidizing gas conditions [13–15].This work examines the effects of adding YSZ on the redox behavior of iron oxide. We introduced YSZ into the iron oxide to enhance its thermal stability in the redox reaction. The effect of varying the yttria concentration in the iron oxide on the redox reaction behaviors was investigated. The reduction and oxidation studies were carried out via TPR/O (temperature-programmed reduction/oxidation) in a fixed-bed reactor. In addition, we added Cu into the Fe/YSZ sample to improve its low-temperature reactivity for the water-splitting reaction.


## 2. Experimental

### 2.1. Sample Preparation

Analytical grade Fe(NO3)3·9H2O (99%, Kanto), Cu(NO3)2·3H2O (99%, Junsei), Y(NO3)3·6H2O (99.9%, Aldrich), and Zr(OCH2CH2CH3)4 (70 wt%, Aldrich) served as sources of the metal precursor of Fe, Cu, Y (yttrium), and Zr, respectively. The concentration of the YSZ in the Fe/YSZ samples was maintained at 40 wt%. We used a urea and Na2CO3 solution as a precipitant and prepared the samples using the coprecipitation and impregnation method.For the coprecipitation method, the samples were prepared as follows. A urea solution was added dropwise to the metal precursor solutions at 90°C over 2 h with stirring. The precipitate was washed three times with deionized water and dried at 100°C for 24 h and then calcined under air at 900°C. For the Na2CO3 solution, the precursor and precipitant solutions were added together dropwise at 2°C under strong stirring.Other samples were prepared via the impregnation method using the as-synthesized YSZ powder. A solution containing the YSZ mixed with the Fe precursor at 60°C was decompressed, and the urea or Na2CO3 solution was added dropwise. The products were washed and dried using the previously described procedure.The prepared samples were denoted as Fe/YSZ-1 (coprecipitation and urea), Fe/YSZ-2 (impregnation method and urea), Fe/YSZ-3 (coprecipitation and Na2CO3), and Fe-YSZ-4 (impregnation method and Na2CO3) depending on the preparation method and type of the precipitant.


### 2.2. Sample Evaluation

We evaluated the redox reactions for the as-prepared samples in a conventional gas-flow system with a fixed-bed quartz reactor. The sample (0.5 g) was charged into the center of the reactor. Hydrogen gas (10% H2, Ar balance) was introduced into the reactor at a flow rate of 40 mL min−1 and heated at 10°C min−1 from room temperature to 550°C for the reduction step. For the subsequent water-splitting oxidation step, water vapor was introduced into the reactor with an Ar carrier gas at a total flow rate of 40 mL min−1; the water vapor partial pressure was approximately 32 kPa, and the heating rate was 10°C min−1 from room temperature to 600°C. The temperature was maintained until no hydrogen peak was detected during both the reduction and oxidation reactions. The hydrogen gas was analyzed using a gas chromatograph (Donam, DS-6200) equipped with a thermal conductivity detector (TCD). Based on the TPR/O profiles, a temperature of 550°C was selected for the hydrogen reduction and 350°C was selected for the water-splitting oxidation in the isothermal cyclic test. The crystallinity of the samples was characterized via X-ray diffraction (XRD, Rigaku Dmax 2500). We also observed the particle size and morphology of the samples via scanning electron microscopy (SEM, Hitachi, S-4700).


## 2.1. Sample Preparation

Analytical grade Fe(NO3)3·9H2O (99%, Kanto), Cu(NO3)2·3H2O (99%, Junsei), Y(NO3)3·6H2O (99.9%, Aldrich), and Zr(OCH2CH2CH3)4 (70 wt%, Aldrich) served as sources of the metal precursor of Fe, Cu, Y (yttrium), and Zr, respectively. The concentration of the YSZ in the Fe/YSZ samples was maintained at 40 wt%. We used a urea and Na2CO3 solution as a precipitant and prepared the samples using the coprecipitation and impregnation method.For the coprecipitation method, the samples were prepared as follows. A urea solution was added dropwise to the metal precursor solutions at 90°C over 2 h with stirring. The precipitate was washed three times with deionized water and dried at 100°C for 24 h and then calcined under air at 900°C. For the Na2CO3 solution, the precursor and precipitant solutions were added together dropwise at 2°C under strong stirring.Other samples were prepared via the impregnation method using the as-synthesized YSZ powder. A solution containing the YSZ mixed with the Fe precursor at 60°C was decompressed, and the urea or Na2CO3 solution was added dropwise. The products were washed and dried using the previously described procedure.The prepared samples were denoted as Fe/YSZ-1 (coprecipitation and urea), Fe/YSZ-2 (impregnation method and urea), Fe/YSZ-3 (coprecipitation and Na2CO3), and Fe-YSZ-4 (impregnation method and Na2CO3) depending on the preparation method and type of the precipitant.


## 2.2. Sample Evaluation

We evaluated the redox reactions for the as-prepared samples in a conventional gas-flow system with a fixed-bed quartz reactor. The sample (0.5 g) was charged into the center of the reactor. Hydrogen gas (10% H2, Ar balance) was introduced into the reactor at a flow rate of 40 mL min−1 and heated at 10°C min−1 from room temperature to 550°C for the reduction step. For the subsequent water-splitting oxidation step, water vapor was introduced into the reactor with an Ar carrier gas at a total flow rate of 40 mL min−1; the water vapor partial pressure was approximately 32 kPa, and the heating rate was 10°C min−1 from room temperature to 600°C. The temperature was maintained until no hydrogen peak was detected during both the reduction and oxidation reactions. The hydrogen gas was analyzed using a gas chromatograph (Donam, DS-6200) equipped with a thermal conductivity detector (TCD). Based on the TPR/O profiles, a temperature of 550°C was selected for the hydrogen reduction and 350°C was selected for the water-splitting oxidation in the isothermal cyclic test. The crystallinity of the samples was characterized via X-ray diffraction (XRD, Rigaku Dmax 2500). We also observed the particle size and morphology of the samples via scanning electron microscopy (SEM, Hitachi, S-4700).


## 3. Results and Discussion

### 3.1. Effects of the Preparation Method

Figure1 presents the XRD patterns of the Fe/YSZ samples, all of which demonstrate that the assignable lines originated from the Fe2O3 and cubic-structured YSZ phases. In addition, no mixing of the Fe, Y (yttrium), and Zr was detected. The patterns for pure ZrO2 exhibit tetragonal or monoclinic structures below the calcination temperature of 2,370°C, but a cubic structure was noted in the presence of Y (yttrium) at low temperature. This result indicates that the cubic-structured YSZ was successfully synthesized. Figure 2 provides the SEM images of the as-prepared samples. The particle sizes were approximately 40–50 nm when urea was used as the precipitant but approximately 150–200 nm when Na2CO3 was used. Given this finding, we concluded that the particle size was strongly affected by the precipitant but not by the precipitation method.Figure 1
XRD patterns of the samples after calcination: (a) Fe/YSZ-1, (b) Fe/YSZ-2, (c) Fe/YSZ-3, and (d) Fe/YSZ-4 (●: Fe2O3, ○: YSZ).SEM images of the samples after calcination: (a) Fe/YSZ-1, (b) Fe/YSZ-2, (c) Fe/YSZ-3, and (d) Fe/YSZ-4.
(a)
(b)
(c)
(d)The TPR/O profiles of the as-prepared samples are presented in Figure3. In the first reduction step, TPR profiles typical of Fe2O3 were observed [9]. Although the reduction was initiated at approximately 300°C, the peaks were primarily observed at approximately 350–500°C and 550°C. These peaks were attributed to a reduction of the Fe2O3 to Fe3O4 and subsequently to metallic Fe (see(3) and (4)). To determine the degree of reduction, the ratio of the first and second peaks in the TPR profiles was calculated as 1 : 8 for the complete reduction [16]
(3)3Fe2O3+1H2⟶2Fe3O4+1H2O(4)2Fe3O4+8H2⟶6Fe+8H2OFigure 3
TPR/O profiles of the as-prepared samples during three repeated redox cycles: (a) Fe/YSZ-1, (b) Fe/YSZ-2, (c) Fe/YSZ-3, and (d) Fe/YSZ-4.The ratios of the areas of the first and second peaks were calculated at approximately 11-12% for all samples, which indicates that most of the Fe2O3 was completely reduced to metallic Fe by hydrogen during the first reduction.Although the oxidation reactions were initiated at approximately 250°C, the maximum peaks were observed in the TPO profiles between 520°C and 550°C for all samples. The Fe/YSZ-2 sample exhibits a relatively low peak intensity and longer reaction time, indicating that the reactivity of the Fe/YSZ-2 was low. The quantities of hydrogen consumed and evolved were calculated (Table1). Under the theoretical conditions, 10.36 mmol g−1-sample hydrogen can be consumed during the first reduction step and 9.21 mmol g−1-sample hydrogen can be evolved in the corresponding reaction step. Although approximately 90–95% of the iron oxide participated during the oxidation reaction with the Fe/YSZ-1 and Fe/YSZ-3 samples, only approximately 50–65% of the iron oxide participated in the reaction with the Fe/YSZ-2 and Fe/YSZ-4 samples. The quantity of hydrogen evolved with the Fe/YSZ-2 gradually decreased from 6.41 to 4.65 mmol g−1-sample during the reaction, indicating a substantial deactivation of this sample. It was interesting that the reactivity of Fe/YSZ-2 sample decreased during the reaction, although the XRD patterns and particle sizes of Fe/YSZ-1 and Fe/YSZ-2 were very similar as shown in Figures 1 and 2. It indicates that the coprecipitation method was more effective in inhibiting sintering of the sample than the impregnation method, because the iron oxide and YSZ were well mixed in the crystal growth step via coprecipitation.Table 1
The quantities of hydrogen consumed and evolved in the TPR/O test during three repeated cycles.
Sample
Maxa
1st Redb
1st Oxic
2nd Red
2nd Oxi
3rd Red
3rd Oxi
Fe/YSZ-1
10.36
10.16
8.89
9.07
8.93
10.23
8.84
Fe/YSZ-2
9.51
6.41
8.68
5.62
7.36
4.65
Fe/YSZ-3
9.86
8.46
9.35
8.25
9.23
8.87
Fe/YSZ-4
8.05
6.12
9.23
5.96
7.65
6.97
aQuantity of hydrogen consumed when 1 g of sample was theoretically reduced in the first reduction (mmol g−1-sample).
bQuantity of hydrogen consumed during the reduction step  (mmol g−1-sample).
cQuantity of hydrogen evolved during water-splitting step  (mmol g−1-sample).An isothermal reduction/oxidation was conducted to compare the hydrogen evolution rates of the samples (Table2). Using the results of the TPR/O profiles, the temperature for the reduction and oxidation was fixed at 550°C. Among the as-prepared samples, Fe/YSZ-1 demonstrates the highest hydrogen evolution rate. The rate of hydrogen evolution decreased in the following order: Fe/YSZ-3 > Fe/YSZ-4 > Fe/YSZ-2. We concluded that a preparation method via the coprecipitation using a urea solution was favorable to maintain reactivity.Table 2
The hydrogen evolution rate for the samples during isothermal redox cycles.
Sample
Hydrogen evolution ratea (mmol min−1 g−1-sample)
1st
2nd
3rd
4th
5th
Avg.
Fe/YSZ-1
1.07
0.95
0.92
0.87
0.97
0.96
Fe/YSZ-2
0.19
0.14
0.1
0.12
0.10
0.13
Fe/YSZ-3
0.70
0.63
0.71
0.79
0.75
0.72
Fe/YSZ-4
0.58
0.56
0.44
0.42
0.44
0.49
aQuantity of hydrogen evolved divided by the time required for complete oxidation.


### 3.2. Effects of the Yttria Concentrations

The effects of the yttria concentrations (4, 8, and 12 mol% of the total metal cations in the YSZ) on the redox reactivity were investigated. The samples were prepared via the coprecipitation using urea and were designated as Fe/xYSZ (x=4,8, and 12). Figure 4 presents the TPR/O profiles for the as-prepared Fe/xYSZ samples. Although typical hydrogen reduction profiles were observed for all samples at a similar temperature, the total reaction time increased with increasing yttria concentration. In the TPO profiles, the temperatures at which oxidation was initiated decreased slightly as the yttria concentration increased.Figure 4
TPR/O profiles of the Fe/xYSZ (x=4,8, and 12) samples during three repeated redox cycles: (a) Fe/4YSZ, (b) Fe/8YSZ, and (c) Fe/12YSZ.The isothermal reactions profiles of the oxidation step for each sample over 5 cycles are listed in Table3. The temperatures for the reduction and oxidation were maintained until the hydrogen peaks were no longer observed. The quantities of evolved hydrogen were similar in all samples (approximately 9-10 mmol g−1-sample). As the yttria concentration increased, the total oxidation time and the rate of hydrogen evolution decreased. Therefore, the Fe/12YSZ sample exhibited the highest hydrogen evolution rate.Table 3
Total oxidation time, quantities of evolved hydrogen, and the hydrogen evolution rate with Fe/4YSZ, Fe/8YSZ, and Fe/12YSZ during five repeated isothermal redox cycles.
Sample
1st
2nd
3rd
4th
5th
Avg.
a
Fe/4YSZ
10.00
10.50
11.25
11.00
10.50
10.65
Fe/8YSZ
9.75
10.50
10.50
10.75
9.75
10.25
Fe/12YSZ
7.75
8.75
9.00
9.50
9.50
8.90
b
Fe/4YSZ
10.16
9.95
9.93
10.01
9.93
10.00
Fe/8YSZ
9.61
9.70
9.45
9.85
9.57
9.64
Fe/12YSZ
9.62
9.61
9.93
10.02
9.94
9.82
c
Fe/4YSZ
1.02
0.95
0.88
0.91
0.95
0.94
Fe/8YSZ
0.99
0.92
0.90
0.92
0.98
0.94
Fe/12YSZ
1.24
1.10
1.10
1.05
1.05
1.11
(a) Total oxidation time (min).
(b) Quantity of hydrogen evolved (mmol g−1-sample).
(c) Quantity of hydrogen evolved divided by the time required for complete oxidation (mmol min−1 g−1-sample).


### 3.3. Effects of the Cu Additive on the Isothermal Reactivity

In our previous study, mixing the Fe3O4 with Ce-ZrO2 [12] accelerated the water-splitting reaction at low temperatures in the presence of a Cu additive. Although the reactivity was maintained during the test, the temperature for the water splitting with Fe/YSZ was relatively high (>500°C). To improve the low-temperature reactivity of the water-splitting step (<350°C), we introduced a small quantity of Cu into the Fe/YSZ.We prepared the 3 wt% Cu-added Fe/12YSZ sample, designated as Cu/Fe/12YSZ, via the coprecipitation method using urea. The XRD peak for the Cu/Fe/12YSZ (Figure5(a)) corresponding to Fe2O3 (hematite) and cubic-structured YSZ was similar to that in Figure 1(a), indicating that the Cu-added iron oxide existed as CuxFe3-xO4 (x<1) [17]. After the oxidation, metallic Cu and Fe3O4 phases were observed (Figure 5(c)).Figure 5
XRD patterns of the samples (a) before the reaction with Cu/Fe/12YSZ, (b) after the first reduction of (a), and (c) after the first oxidation of (b) (●: Fe2O3, ○: YSZ, ▼: Fe, □: Fe3O4, ◆: Cu).Figure6 provides the TPR/O profiles for the Cu/Fe/12YSZ and Fe/12YSZ samples. The reduction reaction for the Cu/Fe/12YSZ sample was initiated at approximately 200°C, and the main reduction peaks were observed at approximately 300°C and 500°C. We also observed a distinct effect on the oxidation reaction with the addition of Cu. The initiation temperature for the oxidation of Cu/Fe/12YSZ decreased by approximately 200°C with the maximum hydrogen evolution observed at approximately 350°C. The Cu additive improved the low-temperature reduction and oxidation reactivity.Figure 6
TPR/O profiles of the (a) Cu/Fe/12YSZ and (b) Fe/12YSZ.The reduction and oxidation temperatures for the isothermal redox reaction were maintained at 550°C and 350°C depending on the TPR/O results. We performed the isothermal redox tests for 35 cycles to identify the cycle stability of the Cu/Fe/12YSZ sample (Figure7). The results can be divided into two sections: the reactions prior to the 10th cycle and those between the 11th and 30th cycles. For the first section, the hydrogen evolution rate was high and the quantities of evolved hydrogen were over 9 mmol g−1-sample. After the 10th cycle, the hydrogen evolution rate and the quantity of evolved hydrogen decreased and remained stable for the reactions between the 11th and 30th cycles. Approximately 8 mmol g−1-sample hydrogen was evolved in the second section, which indicates a hydrogen storage of 1.8 wt% based on the Cu/Fe/12YSZ sample.Figure 7
Isothermal oxidation profiles of the Cu/Fe/12YSZ during 35 redox cycles.After the 30th cycle, we collected the reacted sample and ground it with a mortar to regenerate the Cu/Fe/12YSZ material. The isothermal redox tests were conducted for 5 cycles by charging the ground sample. The quantity of hydrogen evolved in the regeneration step was maintained at approximately 8 mmol g−1-sample. In addition, the rate of hydrogen evolution was approximately 9 mmol min−1 g−1-sample. These values were similar to those obtained prior to the regeneration step, indicating that the regeneration process restores the sample reactivity.Figure8 provides the SEM images of the Cu/Fe/12YSZ sample both before the reaction and after the 35th redox cycle. The average size of the Cu/Fe/12YSZ was approximately 30–40 nm (Figure 8(a)). After the 35th redox cycle, aggregated Cu/Fe/12YSZ particles were observed (Figure 8(b)). The decrease in the rate of hydrogen evolution and the quantity of hydrogen evolved with Cu/Fe/12YSZ was attributed to the deactivation due to particle aggregation.SEM images of the Cu/Fe/12YSZ sample (a) prior to the reaction and (b) after the 35th redox cycle.
(a)
(b)


## 3.1. Effects of the Preparation Method

Figure1 presents the XRD patterns of the Fe/YSZ samples, all of which demonstrate that the assignable lines originated from the Fe2O3 and cubic-structured YSZ phases. In addition, no mixing of the Fe, Y (yttrium), and Zr was detected. The patterns for pure ZrO2 exhibit tetragonal or monoclinic structures below the calcination temperature of 2,370°C, but a cubic structure was noted in the presence of Y (yttrium) at low temperature. This result indicates that the cubic-structured YSZ was successfully synthesized. Figure 2 provides the SEM images of the as-prepared samples. The particle sizes were approximately 40–50 nm when urea was used as the precipitant but approximately 150–200 nm when Na2CO3 was used. Given this finding, we concluded that the particle size was strongly affected by the precipitant but not by the precipitation method.Figure 1
XRD patterns of the samples after calcination: (a) Fe/YSZ-1, (b) Fe/YSZ-2, (c) Fe/YSZ-3, and (d) Fe/YSZ-4 (●: Fe2O3, ○: YSZ).SEM images of the samples after calcination: (a) Fe/YSZ-1, (b) Fe/YSZ-2, (c) Fe/YSZ-3, and (d) Fe/YSZ-4.
(a)
(b)
(c)
(d)The TPR/O profiles of the as-prepared samples are presented in Figure3. In the first reduction step, TPR profiles typical of Fe2O3 were observed [9]. Although the reduction was initiated at approximately 300°C, the peaks were primarily observed at approximately 350–500°C and 550°C. These peaks were attributed to a reduction of the Fe2O3 to Fe3O4 and subsequently to metallic Fe (see(3) and (4)). To determine the degree of reduction, the ratio of the first and second peaks in the TPR profiles was calculated as 1 : 8 for the complete reduction [16]
(3)3Fe2O3+1H2⟶2Fe3O4+1H2O(4)2Fe3O4+8H2⟶6Fe+8H2OFigure 3
TPR/O profiles of the as-prepared samples during three repeated redox cycles: (a) Fe/YSZ-1, (b) Fe/YSZ-2, (c) Fe/YSZ-3, and (d) Fe/YSZ-4.The ratios of the areas of the first and second peaks were calculated at approximately 11-12% for all samples, which indicates that most of the Fe2O3 was completely reduced to metallic Fe by hydrogen during the first reduction.Although the oxidation reactions were initiated at approximately 250°C, the maximum peaks were observed in the TPO profiles between 520°C and 550°C for all samples. The Fe/YSZ-2 sample exhibits a relatively low peak intensity and longer reaction time, indicating that the reactivity of the Fe/YSZ-2 was low. The quantities of hydrogen consumed and evolved were calculated (Table1). Under the theoretical conditions, 10.36 mmol g−1-sample hydrogen can be consumed during the first reduction step and 9.21 mmol g−1-sample hydrogen can be evolved in the corresponding reaction step. Although approximately 90–95% of the iron oxide participated during the oxidation reaction with the Fe/YSZ-1 and Fe/YSZ-3 samples, only approximately 50–65% of the iron oxide participated in the reaction with the Fe/YSZ-2 and Fe/YSZ-4 samples. The quantity of hydrogen evolved with the Fe/YSZ-2 gradually decreased from 6.41 to 4.65 mmol g−1-sample during the reaction, indicating a substantial deactivation of this sample. It was interesting that the reactivity of Fe/YSZ-2 sample decreased during the reaction, although the XRD patterns and particle sizes of Fe/YSZ-1 and Fe/YSZ-2 were very similar as shown in Figures 1 and 2. It indicates that the coprecipitation method was more effective in inhibiting sintering of the sample than the impregnation method, because the iron oxide and YSZ were well mixed in the crystal growth step via coprecipitation.Table 1
The quantities of hydrogen consumed and evolved in the TPR/O test during three repeated cycles.
Sample
Maxa
1st Redb
1st Oxic
2nd Red
2nd Oxi
3rd Red
3rd Oxi
Fe/YSZ-1
10.36
10.16
8.89
9.07
8.93
10.23
8.84
Fe/YSZ-2
9.51
6.41
8.68
5.62
7.36
4.65
Fe/YSZ-3
9.86
8.46
9.35
8.25
9.23
8.87
Fe/YSZ-4
8.05
6.12
9.23
5.96
7.65
6.97
aQuantity of hydrogen consumed when 1 g of sample was theoretically reduced in the first reduction (mmol g−1-sample).
bQuantity of hydrogen consumed during the reduction step  (mmol g−1-sample).
cQuantity of hydrogen evolved during water-splitting step  (mmol g−1-sample).An isothermal reduction/oxidation was conducted to compare the hydrogen evolution rates of the samples (Table2). Using the results of the TPR/O profiles, the temperature for the reduction and oxidation was fixed at 550°C. Among the as-prepared samples, Fe/YSZ-1 demonstrates the highest hydrogen evolution rate. The rate of hydrogen evolution decreased in the following order: Fe/YSZ-3 > Fe/YSZ-4 > Fe/YSZ-2. We concluded that a preparation method via the coprecipitation using a urea solution was favorable to maintain reactivity.Table 2
The hydrogen evolution rate for the samples during isothermal redox cycles.
Sample
Hydrogen evolution ratea (mmol min−1 g−1-sample)
1st
2nd
3rd
4th
5th
Avg.
Fe/YSZ-1
1.07
0.95
0.92
0.87
0.97
0.96
Fe/YSZ-2
0.19
0.14
0.1
0.12
0.10
0.13
Fe/YSZ-3
0.70
0.63
0.71
0.79
0.75
0.72
Fe/YSZ-4
0.58
0.56
0.44
0.42
0.44
0.49
aQuantity of hydrogen evolved divided by the time required for complete oxidation.


## 3.2. Effects of the Yttria Concentrations

The effects of the yttria concentrations (4, 8, and 12 mol% of the total metal cations in the YSZ) on the redox reactivity were investigated. The samples were prepared via the coprecipitation using urea and were designated as Fe/xYSZ (x=4,8, and 12). Figure 4 presents the TPR/O profiles for the as-prepared Fe/xYSZ samples. Although typical hydrogen reduction profiles were observed for all samples at a similar temperature, the total reaction time increased with increasing yttria concentration. In the TPO profiles, the temperatures at which oxidation was initiated decreased slightly as the yttria concentration increased.Figure 4
TPR/O profiles of the Fe/xYSZ (x=4,8, and 12) samples during three repeated redox cycles: (a) Fe/4YSZ, (b) Fe/8YSZ, and (c) Fe/12YSZ.The isothermal reactions profiles of the oxidation step for each sample over 5 cycles are listed in Table3. The temperatures for the reduction and oxidation were maintained until the hydrogen peaks were no longer observed. The quantities of evolved hydrogen were similar in all samples (approximately 9-10 mmol g−1-sample). As the yttria concentration increased, the total oxidation time and the rate of hydrogen evolution decreased. Therefore, the Fe/12YSZ sample exhibited the highest hydrogen evolution rate.Table 3
Total oxidation time, quantities of evolved hydrogen, and the hydrogen evolution rate with Fe/4YSZ, Fe/8YSZ, and Fe/12YSZ during five repeated isothermal redox cycles.
Sample
1st
2nd
3rd
4th
5th
Avg.
a
Fe/4YSZ
10.00
10.50
11.25
11.00
10.50
10.65
Fe/8YSZ
9.75
10.50
10.50
10.75
9.75
10.25
Fe/12YSZ
7.75
8.75
9.00
9.50
9.50
8.90
b
Fe/4YSZ
10.16
9.95
9.93
10.01
9.93
10.00
Fe/8YSZ
9.61
9.70
9.45
9.85
9.57
9.64
Fe/12YSZ
9.62
9.61
9.93
10.02
9.94
9.82
c
Fe/4YSZ
1.02
0.95
0.88
0.91
0.95
0.94
Fe/8YSZ
0.99
0.92
0.90
0.92
0.98
0.94
Fe/12YSZ
1.24
1.10
1.10
1.05
1.05
1.11
(a) Total oxidation time (min).
(b) Quantity of hydrogen evolved (mmol g−1-sample).
(c) Quantity of hydrogen evolved divided by the time required for complete oxidation (mmol min−1 g−1-sample).


## 3.3. Effects of the Cu Additive on the Isothermal Reactivity

In our previous study, mixing the Fe3O4 with Ce-ZrO2 [12] accelerated the water-splitting reaction at low temperatures in the presence of a Cu additive. Although the reactivity was maintained during the test, the temperature for the water splitting with Fe/YSZ was relatively high (>500°C). To improve the low-temperature reactivity of the water-splitting step (<350°C), we introduced a small quantity of Cu into the Fe/YSZ.We prepared the 3 wt% Cu-added Fe/12YSZ sample, designated as Cu/Fe/12YSZ, via the coprecipitation method using urea. The XRD peak for the Cu/Fe/12YSZ (Figure5(a)) corresponding to Fe2O3 (hematite) and cubic-structured YSZ was similar to that in Figure 1(a), indicating that the Cu-added iron oxide existed as CuxFe3-xO4 (x<1) [17]. After the oxidation, metallic Cu and Fe3O4 phases were observed (Figure 5(c)).Figure 5
XRD patterns of the samples (a) before the reaction with Cu/Fe/12YSZ, (b) after the first reduction of (a), and (c) after the first oxidation of (b) (●: Fe2O3, ○: YSZ, ▼: Fe, □: Fe3O4, ◆: Cu).Figure6 provides the TPR/O profiles for the Cu/Fe/12YSZ and Fe/12YSZ samples. The reduction reaction for the Cu/Fe/12YSZ sample was initiated at approximately 200°C, and the main reduction peaks were observed at approximately 300°C and 500°C. We also observed a distinct effect on the oxidation reaction with the addition of Cu. The initiation temperature for the oxidation of Cu/Fe/12YSZ decreased by approximately 200°C with the maximum hydrogen evolution observed at approximately 350°C. The Cu additive improved the low-temperature reduction and oxidation reactivity.Figure 6
TPR/O profiles of the (a) Cu/Fe/12YSZ and (b) Fe/12YSZ.The reduction and oxidation temperatures for the isothermal redox reaction were maintained at 550°C and 350°C depending on the TPR/O results. We performed the isothermal redox tests for 35 cycles to identify the cycle stability of the Cu/Fe/12YSZ sample (Figure7). The results can be divided into two sections: the reactions prior to the 10th cycle and those between the 11th and 30th cycles. For the first section, the hydrogen evolution rate was high and the quantities of evolved hydrogen were over 9 mmol g−1-sample. After the 10th cycle, the hydrogen evolution rate and the quantity of evolved hydrogen decreased and remained stable for the reactions between the 11th and 30th cycles. Approximately 8 mmol g−1-sample hydrogen was evolved in the second section, which indicates a hydrogen storage of 1.8 wt% based on the Cu/Fe/12YSZ sample.Figure 7
Isothermal oxidation profiles of the Cu/Fe/12YSZ during 35 redox cycles.After the 30th cycle, we collected the reacted sample and ground it with a mortar to regenerate the Cu/Fe/12YSZ material. The isothermal redox tests were conducted for 5 cycles by charging the ground sample. The quantity of hydrogen evolved in the regeneration step was maintained at approximately 8 mmol g−1-sample. In addition, the rate of hydrogen evolution was approximately 9 mmol min−1 g−1-sample. These values were similar to those obtained prior to the regeneration step, indicating that the regeneration process restores the sample reactivity.Figure8 provides the SEM images of the Cu/Fe/12YSZ sample both before the reaction and after the 35th redox cycle. The average size of the Cu/Fe/12YSZ was approximately 30–40 nm (Figure 8(a)). After the 35th redox cycle, aggregated Cu/Fe/12YSZ particles were observed (Figure 8(b)). The decrease in the rate of hydrogen evolution and the quantity of hydrogen evolved with Cu/Fe/12YSZ was attributed to the deactivation due to particle aggregation.SEM images of the Cu/Fe/12YSZ sample (a) prior to the reaction and (b) after the 35th redox cycle.
(a)
(b)


## 4. Conclusions

We investigated the hydrogen storage and release characteristics of a YSZ-supported iron oxide sample using TPR/O and isothermal redox tests. Preparation via coprecipitation using urea was effective in maintaining the sample reactivity. Increasing the yttria concentration in the Fe/YSZ decreased the total oxidation time and the rate of hydrogen evolution. The introduction of a small quantity of Cu into the Fe/YSZ enhanced the low-temperature reduction and oxidation reactivity. The isothermal redox tests yielded the hydrogen storage of 1.8 wt% based on the Cu/Fe/12YSZ sample. In addition, the regeneration of the sample restores its reactivity.



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*Source: 695258-2013-12-15.xml*