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Chapter 1. Introduction 6 that make up the electrodes are described in Chapter 3, section 3.2.2.3.2, and the chapters thereafter present studies of these and other electrode materials. Because the solid oxide electrolyte conducts oxide ions, solid oxide cells can oxidize CO and reduce CO2 in addition to H2/H2O, which cannot be done with proton exchange membrane (PEM) cells or alkaline cells because their electrolytes conduct protons (H+) and hydroxide ions (OH–) respectively. The high temperature operation is also advantageous for both thermodynamic and reaction kinetics reasons, increasing energy efficiency and lowering the cost, as discussed further in sections 3.2.2.3 and 3.2.2.3.2. Figure 1-2. A solid oxide cell operated as an electrolysis cell and as a fuel cell. 1.1.1. Thermodynamics The reversible potential of the cell, Erev, which is typically the voltage measured at open circuit (OCV), is defined by the equilibrium gas composition and thermodynamics according to equations (1.1) (the Nernst equation) and (1.2). The Nernst equation is shown with H2/H2O gasses; for CO/CO2 one simply substitutes pCO for pH2 and pCO2 for pH2O. In the case that both types of gas atmospheres are supplied as a mixture (H2/H2O/CO/CO2) then all of the gasPDF Image | Electrolysis of CO2 and H2O
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