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The ECFORM Process A schematic diagram of the ECFORM process is shown in Figure 4. It consists of two electrodes, the cathode (negative electrode) and the anode (positive electrode), across which an electrical voltage is applied. The two electrodes are placed in two different chambers, separated from each other by an ion exchange membrane. This prevents bulk mixing of the solutions flowing in each of the chambers, while simultaneously allowing ions to move across the membrane and maintain electrical continuity. A suitable electrolyte is introduced into the cathode chamber along with CO2. The electrolyte comes into contact with the cathode, and the dissolved CO2 is electrochemically reduced to the desired products. This electrical circuit is completed by the complementary oxidation reaction occurring in the anode chamber. In ECFORM, tin or proprietary tin-based alloys are used as the cathodes that convert CO2 to formate salts. Small concentrations of by- products (hydrogen and CO) are also produced at the cathode. An oxygen evolution reaction takes place at the anode. An important metric of the process is the energy consumption, which is determined by the number of electrons (n) involved in reducing 1 molecule of CO2 to products, cell voltage, and the current efficiency, also called Faraday efficiency (FE). The FE denotes the percentage of the total current used for the desired product (i.e., the selectivity). The calculations in Figure 5 include additional energy consumed by auxiliary components, such as pumps. As shown in Figure 5, the reduction of CO2 to formate/ formic acid and to carbon monoxide, respectively, appears to be the best option for practical development for at least two reasons. First, both reactions involve the participation of only two electrons, and therefore the electrical power consumption is the lowest. Secondly, the high FE of CO and formate/formic acid reactions have been achieved on affordable metal cathodes, further minimizing the energy consumption and cost. The next promising reaction may be the production of methanol. Although this involves 6 electrons for each molecule of methanol formed, the low over potentials on the catalysts reduce the cell potential to nearly half of that for other electrochemical processes. Thus, relatively lower specific energy consumption can also be achieved. An economically viable electrochemical technology requires optimization of four key parameters (Figure 6): high current densities, high FE, low specific electricity consumption, and long electrode lifetime. The minimum Figure 4. A schematic representation of the ECFORM process to convert CO2 to formate/formic acid. 8PDF Image | Electrochemical Conversion of CO2
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