Platinum/carbon black catalysts (Pt/C) entrapped in epichlorohydrin-crosslinked chitosan are used to prepare the cathode electrocatalysts for H2/O2 PEM fuel cells. The effects of the epichlorohydrin content (0–12 g), operating temperatures (40–80 C), and relative humidity (50–100% RH) on performance of the fuel cells are investigated. The optimal epichlorohydrin amount of 4 g (Pt/C–4–Chi) results in the uniform distribution of Pt particles on the carbon black support and the sufficient number of chitosan crosslinks in the catalyst that can both keep the three-phase boundary in place and simultaneously diminish the swelling degree of chitosan chains under humidified conditions. The optimal epichlorohydrin content in combination with the optimal operating conditions of 40 C and 100%RH yield the best fuel cell performance (lowest activation overvoltage and ohmic overvoltage), relative to the unmodified catalyst and the other modified catalysts. Under the optimal operating conditions, the voltage stability of the fuel cell containing Pt/C–4–Chi under continuous operation for 30 h is comparable with that of the cell containing the unmodified catalyst. The performance of the fuel cells is greatly dependent on the relative humidity of the cells which enhances the proton transfer in the cells. 1. Introduction At the cathode, the sluggish electrochemical reaction (i.e. the oxygen reduction reaction) and poor transport of protons and electrons decrease the performance of H2/O2 proton–exchange membrane fuel cells (PEMFCs) by increasing the activation overvoltage, or activation loss [1]. This problem can be overcome by increasing the operating temperature [2], but too high a temperature reduces the membrane humidity, which can increase th... ... middle of paper ... ...ochemistry: application to fuel cells, Ph.D. Thesis, Department of Materials Science and Engineering, Stanford University, USA, 2004. [20] B. Gou, W.K. Na, B. Diong, Fuel Cells: Modeling, Control, and Applications, in: Power Electronics and Applications Series, CRC Press, USA, 2009. [21] X.-Z. Yuan, H. Wang in: J. Zhang (Ed.), PEM Fuel Cell Electrocatalysts and Catalyst Layers: Fundamentals and Applications, Springer, London, 2008. [22] S. Song, G. Wang, W. Zhou, X. Zhao, G. Sun, Q. Xin, S. Kontou, P. Tsiakaras, J. Power Sources 140 (2005) 103−110. [23] I.E. Pacios, M.J. Molina, M.R. Gómez-Antón, I.F. Piérola, J. Appl. Polym. Sci. 103 (2007) 263–269. [24] C. Song, J. Zhang in: J. Zhang (Ed.), PEM Fuel Cell Electrocatalysts and Catalyst Layers: Fundamentals and Applications, Springer, London, 2008. [25] Q. Yan, H. Toghiani, J. Wu, J. Power Sources 158 (2006) 316−325.
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Fuel cells could create new markets for steel, electronics, electrical and control industries and other equipment suppliers. They could provide tens of thousands of high-quality jobs and reduce trade deficits.
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In order to gain strong insight into the surface chemistry of silica we have perform a thorough literature search. Our goal is to identify the pioneer research performed on silica and silica supported catalyst. Particular interest lies in silica-water-cobalt and silica-alcohol-cobalt systems. This study is both on macro and micro level so that a complete theoretical base can be established. From this theoretical knowledge, key areas to look upon will be identified and a design of experiments will be established. The goal is to develop a both efficient and effective product (catalyst) using a novel methodology developed from past research.
Schreuder, Jolanda A. H.; Roelen, Corné A. M.; van Zweeden, Nely F.; Jongsma, Dianne; van der Klink, Jac J. L.; Groothoff, Johan W.
Hydrogen Fuel Cell cars makes water by combining two hydrogen molecules and one oxygen molecule this makes electricity. It works like a regular battery; it stores chemicals inside its cell and converts them into an electric charge. With Fuel Cell, the flow in its cell is steady, so it never dies like a regular battery. Sir William Grove invented Fuel Cell in 1839. It did not become popular because of the success of internal combustion motor.
At the cathode the hydrogen ions gain an electron. They are discharged and are converted into hydrogen gas: 2H (+) + 2e (-) → H2 At the anode, the hydroxide, not the sulphate ions are discharged. Water and oxygen gas are formed: 4OH (-) → 2 H2O + O2 + 4e (-) The hydrogen gas can be collected and measured. The greater the volume of hydrogen gas formed over a set period of time, the faster electrolysis is occurring.
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