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Journal of Nanotechnology
Volume 2012 (2012), Article ID 573287, 6 pages
http://dx.doi.org/10.1155/2012/573287
Research Article

Reforming of Ethanol to Produce Hydrogen over PtRuMg/ZrO2 Catalyst

1Department of Chemical and Materials Engineering, Chung Cheng Institute of Technology, National Defense University, Tahsi, Taoyuan 33509, Taiwan
2Fuel Cell Center, Yuan Ze University, Taoyuan 32003, Taiwan
3Department of Mechanical Engineering, Yuan Ze University, Taoyuan 32003, Taiwan
4Graduate School of Renewable Energy and Engineering, Yuan Ze University, Taoyuan 32003, Taiwan

Received 15 March 2012; Accepted 24 April 2012

Academic Editor: Shrikrishna D. Sartale

Copyright © 2012 Josh Y. Z. Chiou et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

A modified PtRu/ZrO2 catalyst with Mg is evaluated for the oxidative steam reforming of ethanol (OSRE) and the steam reforming of ethanol (SRE). In order to understand the variation in the reaction mechanism on OSRE and SRE, further analysis of both fresh and used catalyst is concentrated on for TEM, TG, Raman, and TPR characterization. The results show that the OSRE reaction requires a higher temperature (𝑇𝑅390°C) to achieve 100% ethanol conversion than the SRE reaction (𝑇𝑅2500°C). The distribution of CO is minor for both reactions (< 5% for OSRE, < 1% for SRE). This demonstrates that the water gas shift (WGS) reaction is an important side-reaction in the reforming of ethanol to produce H2 and CO2. A comparison of the temperature of WGS (𝑇WGS) shows it is lower for the SRE reaction (𝑇WGS250°C for SRE, ~340°C for OSRE).

1. Introduction

The prospect of global energy shortages as well as increasingly stringent emission regulations has stimulated interest in renewable energies. Production of hydrogen from renewable sources derived from agricultural or other waste streams offers the possibility of lower or even no net greenhouse gas emissions [1, 2]. Among the candidates for hydrogen production, ethanol produced by the fermentation of biomass offers many advantages, such as low toxicity, high biodegradability, and easy transport [35]; thus, the reforming of ethanol is seen as a promising method for hydrogen production from renewable resource [6, 7]. Hydrogen can be produced from ethanol through different reforming processes, for example, steam reforming of ethanol (SRE), partial oxidation of ethanol (POE), and oxidative steam reforming of ethanol (OSRE). Moreover, a high yield of hydrogen can be obtained from the SRE reaction [414].

The nature of the metal and its support strongly affect both stability and products distribution [5, 15]. In view of the ZrO2-supported system, noble metal catalysts such as Pt and Ru are well known for their high catalytic activities, which have been extensively investigated. The size-selective capability of Pt/ZrO2 catalysts on the catalytic decomposition of alcohol for the production of hydrogen was reported by Cuenya’s group [7, 16]. However, this catalyst deactivated at high temperatures due to carbon deposition. De Lima et al. [17] reported that the side-products of acetaldehyde and ethane were favored on Pt/ZrO2 in the SRE. Relatively low reaction temperatures around 100 to 200°C in the POE and OSRE over a Pt/ZrO2 and PtRu/ZrO2 catalysts were reported by our previous studies [1821], and 300°C was reported by Mattos and Noronha [22] in the POE reaction. The main problem found when using these catalysts is deactivation by sintering and carbon deposition. The use of basic oxides as supports and the addition of metal species (Li, Na, K, and Cu, etc.) have been found to improve catalytic performance and overcome the disadvantages [9, 2325]. Recently, Carrero et al. [26] reported the effect of alkaline earth metals over Cu-Ni/SiO2 catalysts where a high hydrogen selectivity was obtained with Mg, while the incorporation of Ca reduced coke formation.

Therefore, the main objective of this paper is to study PtRuMg/ZrO2 catalyst for the SRE and OSRE reactions to produce hydrogen at a temperature lower than 300°C with higher ethanol conversion (𝑋EtOH), hydrogen yield (𝑌H2), and lower CO distribution. The expectation is that the catalytic activity and stability against the coke deposition of the PtRuMg/ZrO2 catalyst on the reforming of ethanol could be enhanced. The characterization of fresh and used catalysts was analyzed by TEM, TG, Raman, and TPR characterization.

2. Experimental

2.1. Catalyst Preparation

A sol-gel method was used for the preparation of the ZrO2 support using Zr[O(CH2)3CH3]4 (Strem) as the precursor. The PtRuMg/ZrO2 catalyst was prepared by the method of sequent incipient wetness impregnation using H2PtCl6 and RuCl3 as precursors (1.5 wt% for each component) first to disperse on the ZrO2. After drying at 110°C and calcination at 400°C for 4 h, 1.0 wt% of Mg(NO3)2·6H2O was incipient sequentially. After drying at 110°C, the prepared sample was crashed to 6080 mesh and stored as fresh catalyst (labeled as PtRuMg/ZrO2).

2.2. Catalyst Characterization

Transmission electron micrographs (TEMs) were taken on a PHILIPS (CM-200) microscope at an accelerated voltage of 200 kV. Thermal gravimetric analysis was carried out using a Seiko SSC5000 TG system. The rate of heating was maintained at 10°C·min−1. The measurement was carried from RT to 1000°C under air flowing with a rate of 100 mL·min−1. The measurements of the Raman spectroscopy were recorded using a Nicolet Almega XR Dispersive Raman spectrometer. The spectra were collected between 500 and 2000 cm−1, using the beam of a diode laser (780 nm), with the sample exposed to the air under ambient conditions. Reduction behavior was studied by temperature-programmed reduction (TPR). A sample of about 50 mg was introduced a flow of 10% H2/N2 gas mixture at a flow rate of 10 mL·min−1. During TPR, the temperature was increased at 7°C·min−1 from room temperature to 900°C.

2.3. Catalytic Activity Measurement

Catalytic activities of the prepared sample towards the SRE and OSRE reactions were tested in a fixed-bed flow reactor at atmospheric pressure. Catalyst in the amount of 100 mg was placed in a 4 mm i.d. quartz tubular reactor and held by glass-wool plugs. Before the reaction, the catalyst was activated by reduction with hydrogen at 300°C for 3 h. The gas hourly space velocity (GHSV) was maintained at 22,000 h−1, and the H2O/EtOH molar ratio was 13 (H2O : EtOH = 80 : 20 by volume) for the SRE reaction; while the GHSV was maintained at 56,000 h−1, the O2/EtOH molar ratio was 0.26, and the H2O/EtOH molar ratio was 4.86 for the OSRE reaction. A 5 h time-on-stream tests were maintained at each measured temperature. The analysis of the reactants and all reaction products was carried out online by gas chromatography, with columns of Porapak Q and Molecular Sieve 5A for separation. The evaluation of the catalytic activity depended on the conversion, products distribution, and the yield of hydrogen: 𝑋EtOH=𝑛EtOH-in𝑛EtOH-out𝑛EtOH-in𝑌×100%,H2=𝑛H2-out𝑛EtOH-in,𝑆𝑖=𝑛𝑃𝑖𝑛𝑃𝑖×100%,(1) where 𝑋EtOH is the conversion of ethanol, 𝑌H2 is the yield of hydrogen, 𝑆𝑖 is the distribution of different products, 𝑃𝑖 is the different products, and 𝑛 is the amounts of moles.

3. Results and Discussion

3.1. Catalytic Evaluation

Figure 1 illustrates the 𝑋EtOH, products distribution (water excluded), and 𝑌H2 from SRE with an H2O/EtOH molar ratio of 13 over the PtRuMg/ZrO2 catalyst between 175 and 300°C. About 1 h to reach the steady state and the recorded date was 5 h time-on-stream tests at each reaction temperature. The concentration of hydrogen increased progressively with increases in temperature (𝑇𝑅). The detailed proposed pathway was shown in the Scheme 1. Below 200°C, the main product besides hydrogen was acetaldehyde, thus indicating that it behaved as a dehydrogenation of ethanol, and then acetaldehyde decomposition into methane and CO with increasing temperature. This indicated that both platinum and ruthenium had a stronger capacity for breaking the C–C bond in the reforming of ethanol C2H5OHCH3CHO+H2CH3CHOCH4+CO.(2)

573287.sch.001
Scheme 1: Reaction routes of SRE and OSRE over PtRuMg/ZrO2 catalyst.
573287.fig.001
Figure 1: Catalytic performance in the SRE reaction over PtRuMg/ZrO2 catalyst.

At higher temperatures (𝑇𝑅>225C), concentrations of CO2 up to 18% accompanied the decreasing of CO to 0.2%. At the same time, the concentration of methane through the decomposition of acetaldehyde was significant. This indicated that the water-gas shift (WGS) reaction occurred at a lower temperature than that of the cobalt oxide [12] and the PtRu/ZrO2 catalyst [20]. This showed that the addition of magnesium improved the reforming activities and enhanced the WGS reaction at lower temperatures CO+H2OH2+CO2.(3)

When the 𝑇𝑅 increased to 280°C, the amount of CH4 side-product increased slightly to approach 16% and decreased the yield of hydrogen since the reversed water-gas shift reaction (RWGS) occurred. The maximum 𝑌H2 approached 4.0 around 275°C for the SRE reaction CO2+4H2CH4+2H2O.(4)

Figure 2 displays the 𝑋EtOH, products distribution (water excluded), and 𝑌H2 from OSRE with an EtOH/H2O/O2 at a molar ratio of 1 : 4.86 : 0.26 over a PtRuMg/ZrO2 catalyst between 250 and 420°C. As compared with the SRE reaction, there were significant differences in the different reactions. The SRE reaction preceded complete conversion of the ethanol at 250°C, while there was only 75% conversion at this temperature and full ethanol conversion exceeded 390°C for the OSRE reaction. The temperature for the decomposition of acetaldehyde (𝐷𝑇) showed that the easy cracking promoted the formation of hydrogen. The 𝐷𝑇 on the SRE reaction approached 200°C, and above 250°C for the OSRE reaction. The acetaldehyde disappeared at 275°C for the SRE reaction, and at 420°C for the OSRE reaction. A comparison of the temperature of WGS (𝑇WGS) showed that it was lower for the SRE reaction (𝑇WGS~ 250°C for SRE, ~340°C for OSRE). The distribution of CO was minor for both reactions (<5% for OSRE, <0.5% for SRE). Besides the main products of H2 and CO2, the decreasing of acetaldehyde accompanied with the trace amounts of acetone was produced through the condensation of acetaldehyde (showed in the Scheme 1) at 𝑇𝑅>340C. At a further temperature increase, the acetone was still detected. This clearly influenced the yield of hydrogen and also, possibly, the coke deposition. The maximum 𝑌H2 only approached 2.8 around 420°C for the OSRE reaction.

573287.fig.002
Figure 2: Catalytic performances in the OSRE reaction over PtRuMg/ZrO2 catalyst.
3.2. Characterization of Used Catalyst

The design of a stable and applicable catalyst is one of the most important issues in the production of hydrogen from ethanol. The significant deactivation reported for hydrogen production from ethanol reforming is usually attributed to carbon formation and sintering of active metals, which is strongly influenced by the nature of the support, catalyst, and reaction conditions (especially temperature and H2O/EtOH/O2 ratio) [9, 2729]. In order to obtain more information about the behavior of the used catalyst, TEM, TG, Raman, and TPR characterizations were pursued for the samples after the SRE and OSRE catalytic tests.

Figure 3 shows the TEM micrographs of both fresh and used catalysts. A comparison with the fresh sample (see Figure 3(a)) showed an apparent deposition of coke on the used catalyst after the OSRE reaction (see Figure 3(b)). There was no obvious coke formation observed after the SRE reaction (see Figure 3(c)). The specific weight loss of combustion of adsorbed C1 species (200~300°C) and coke (400~600°C) on the catalyst surface was obtained from the TG results (see Figure 4). Since the addition of magnesium modified the catalyst becomes slightly base which may be adsorbed C1 species after the reforming reaction. It was apparent that only after the OSRE reaction was the combustion of coke observed. Furthermore, the Raman spectra (see Figure 5) of the used catalyst after the SRE reaction differed from the OSRE reaction. There were two bands centered at 1320 (D-band) and 1590 (G-band) cm−1, characteristic of poorly ordered carbon deposition [30], observed after the OSRE reaction but not after the SRE reaction. This result indicated that the coke formed through the OSRE reaction. Also, the evidence of coke formation can be demonstrated by the TPR analysis. Figure 6 shows the TPR profiles of the used catalyst after the SRE and OSRE reactions. Two reduction regions can be distinguished: one region for the adsorbed C1 species (around 298°C) and the other region for coke (around 584°C), with the broad signal coming from the methanation of deposited carbon [8] C+2H2CH4.(5)

fig3
Figure 3: TEM images of fresh and used catalysts: (a) fresh, (b) after OSRE reaction, and (c) after SRE reaction.
573287.fig.004
Figure 4: TG curves of used catalyst after SRE and OSRE reaction.
573287.fig.005
Figure 5: Raman spectra of used catalyst after SRE and OSRE reaction.
573287.fig.006
Figure 6: TPR profiles of used catalyst after SRE and OSRE reaction.

From the characterization of the used catalyst, we observed a more pronounced coke formation in the OSRE reaction and confirmed that the designed PtRuMg/ZrO2 catalyst was a suitable application on the SRE reaction.

4. Conclusions

A novel and high performance PtRuMg/ZrO2 catalyst had been designed and applied on the SRE and OSRE reaction to produce hydrogen at low temperature. The results showed that the distribution of CO was minor for both reactions (<5% for OSRE, <1% for SRE). The OSRE reaction required a higher temperature (𝑇𝑅390C) to achieve 100% ethanol conversion than the SRE reaction (𝑇𝑅250C). Also the temperature of WGS accompanying the OSRE reaction was higher (𝑇WGS340C) than that of the SRE reaction (𝑇WGS250C). A more pronounced coke formation was observed in the OSRE reaction. In considering the catalytic stability against the coke deposition, application of PtRuMg/ZrO2 catalyst on the SRE reaction is suitable.

Acknowledgment

The authors are pleased to acknowledge the financial support for this study by the National Science Council of the Republic of China under contract nos. of NSC 99-2113-M-606-001-MY3, and NSC 101-2623-E-155-001-ET.

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