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The catholyte is the water fed to the cathode compartment and it must be free from hardness ions such as calcium (Ca+2) and magnesium (Mg+2). The pH in the cathode compartment is high enough to precipitate these hardness ions. Therefore, a total hardness concentration of less than 50 ppm is desired. Water produced from a reverse osmosis (RO) system has been normally used in these evaluations. In these test series the RO water will be replaced with KW-city drinking water and the effects on module performance, anode and cathode effluent discharge, and anode effluent chlorine discharge are primary objectives of this evaluation. Table 1 provides a detailed description of the E-CEM’s electrical and flow rate specifications along with the materials used in the cell configuration. The anode and cathode are platinum plated titanium electrodes. These tests determined the flow rate to current ratio required to lower seawater pH to the target level. This information determines electrode performance and operating life. The cell contained a polyethylene extruded cation permeable membrane. Membrane performance was evaluated during these tests, since its performance and operating life is based on current density and level of organic compounds contained in the seawater. 4.2 E-CEM Reactions Figure 1 shows a continuous flow process in which seawater is passed through the center compartment of the E-CEM at a flow rate of 0.5 gal/min. The Na+ in the seawater are exchanged for H+ produced by the stream that is flowing adjacent to two cation-permeable membranes. Direct current (DC) facilitates this exchange. The principle chemical reactions within the E-CEM are simplified as shown in eqs 4 - 8. Anode: 2H2O 4H+ + O2 + 4e- (4) Center Compartment: 2H+ + 2Na+ + 2HCO3- 2H2CO3 + 2Na+ (5) Center Compartment Acidified Seawater Effluent: 2H2CO3 2H2O + 2CO2 (6) Cathode: 4H2O + 4e- 4OH- + 2H2 (7) Overall chemical reaction: 2H2O +2HCO3- 2OH- + O2 + 2H2 + 2CO2 (8) The amount of H+ generated by the anode is proportional to the applied electrical current, which follows Faraday’s law. The anode and cathode reactions used to theoretically determine the amount of H+, OH-, H2, and O2 produced per amp-second of current passed through the electrodes are provided in eqs 9-14 as follows: For the anode reaction, 96,487 A-sec will produce 1⁄4 mole O2 gas and 1 mole H+ and for the cathode reaction, 96,487 A-sec will produce 1⁄2 mole H2 gas and 1 mole OH-. This allows the amount of H+, OH-, H2, and O2 produced per amp/second of current passed through the electrodes to be derived: Anode Reaction 5PDF Image | Extraction CO2 H2 in Seawater Electrolytic Cation Exchange
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