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Chapter 1. Introduction 5 1.1. Electrochemical Energy Conversion and Solid Oxide Cells This section provides a brief introduction to high temperature electrolysis cells with solid oxide electrolytes. Solid oxide cells, as well as most low temperature cellsi, can be operated reversibly, as either a fuel cell or as an electrolyzer. In fuel cell mode, fuel is supplied to one electrode and oxidant (such as air) is supplied to the other, creating a potential difference (voltage) across the cell which drives the electrode reactions and the transport of ions across the electrolyte to complete the electrical circuit, producing electricity and oxidizing the fuel to water and CO2. A variety of fuels can be supplied, such as hydrogen, carbon monoxide, natural gas/methane, and even other hydrocarbons and carbon-rich fuels like coal although they typically need to be gasified first by reforming with steam or CO2. In electrolysis mode, gaseous oxides such as steam and carbon dioxide are supplied to one electrode (and at the other electrode, no reactants are needed but a sweep gas of air or oxygen is often supplied) and a voltage is applied across the cell. This drives the electrolysis of the H2O and/or CO2, splitting these oxides by removal of an oxygen atom, which is transported as an oxide ion across the electrolyte to the other electrode where the oxide ions recombine to produce gaseous oxygen. Fuels such as H2 and CO are thus produced, which can be reformed into other fuels such as methane or liquid hydrocarbons. At the other electrode a valuable stream of pure O2 can be easily obtained if a sweep gas of O2 is used. A diagram of a solid oxide cell in both modes of operation, along with the corresponding electrode reactions, is shown in Figure 1-2. Depicted is a planar-geometry solid oxide cell (as opposed to tubular geometry and other existing geometries). Planar cells are stacked with electrical interconnect plates between the electrodes of adjacent cells to form a cell stack. The electrolyte is a dense thin oxide ion conducting ceramic, usually yttria-stabilized zirconia. The electrolyte layer is sandwiched between the two porous electrodes, which are typically made of a composite of the electrolyte material and an electron conducting material (either a metal or an electronically conductive ceramic) that also provides electrocatalytic activity for the reactions (or sometimes other materials are added to enhance electrocatalytic activity). The typical materials i The ability of an electrochemical cell to operate reversibly as either a fuel cell or an electrolysis cell depends only on the cell geometry, not on any limitation of the electrochemistry. That is, the cell must be constructed such that either type of reactant – the fuel molecules or oxidized molecules – can be supplied to the electrode reaction sites. An example of a cell that is not designed to operate reversibly is a simple aqueous electrolysis cell where the electrodes are immersed in the aqueous electrolyte. Water is split and H2 gas is evolved. There is no easy way to supply H2 to the electrodes and run this type of cell as a fuel cell.PDF Image | Electrolysis of CO2 and H2O
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