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Figure 2.1: The relationship between electrolysis and its reverse reaction, the reaction that occurs in hydrogen fuel cells. Left: Electrolysis of water; Right: Fuel Cell Reaction; Note that the current flows in opposite directions.4 Equation 2.2: ππ2(ππ) + 2π»π»2 (ππ) β 2π»π»2ππ (ππ) At each of the electrodes is a half reaction. At the anode (site of hydrogen consumption/ionization): Equation 2.3: 2π»π»2 (ππ) β 4π»π»+ + 4ππβ The hydrogen ionizes and releases electrons into the wire to create a current (flowing from - to +) and protons (H+) that travel through the electrolyte to the cathode. At the cathode: Equation 2.4: ππ2(ππ) + 4ππβ + 4π»π»+ β 2π»π»2ππ(ππ) Oxygen (usually from filtered ambient air), the electrons, and protons (H+) combine to form water. The electrons flow through the electrical circuit to reach the cathode while the protons travel through the electrolyte. This basic process occurs inside a hydrogen fuel cell. While there are several types of fuel cells, the one examined in this study is the Proton Exchange Membrane FC or PEMFC. 2.1.3. Proton Exchange Membrane Fuel Cells (PEMFCs) PEMFCs are one way to package the theoretical reactions described above into practical power generation devices, minimizing both space and weight. The reactions at the cathode and anode can only take place where the gas, electrode, and electrolyte all meet. To maximize this area, the electrodes are manufactured into thin porous layers and are βsandwichedβ together. PEMFCs have a βsandwichβ of cathode, electrolyte, and anode, which is set between two βbipolarβ plates. See Figure 2.2 for visualization of this structure. 4 βFuel Cell Commercialization Conference of Japan.β Available from: http://fccj.jp/eng/aboutfuelcell.html 20PDF Image | Regenerative Fuel Cell
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