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4. Discussion 4.1. Influence of Current Density MembrCanuesr2r0e2n0t, 1d0e, n19s8ity effects can be observed in experiments 1, 2 and 3 (see Table 3). The results11shofo2w1 that current density influences cell voltage, specific electrical consumption, current efficiency and LiOH production rate. 2 At the same temperature, an increase in current density from 1200 to 2400 A/m At the same temperature, an increase in current density from 1200 to 2400 A/m2 produced a cell cell voltage increase of 24%. This caused an increase in LiOH production rate of 120% at the cost of voltage increase of 24%. This caused an increase in LiOH production rate of 120% at the cost of increasing specific electrical consumption by 14%. On the other hand, a current density increment increasing specific electrical consumption by 14%. On the other hand, a current density increment from 2400 to 3600 A/m2 produced a 56% increase in cell voltage. This effect allows a LiOH production from 2400 to 3600 A/m2 produced a 56% increase in cell voltage. This effect allows a LiOH production rate increase of 66% at the cost of increasing specific electrical consumption by 41%. This difference rate increase of 66% at the cost of increasing specific electrical consumption by 41%. This difference suggests that increasing current density above 2400 A/m2 reduces process energy efficiency. The results suggests that increasing current density above 2400 A/m2 reduces process energy efficiency. The follow [18], where energy consumption increases with higher voltages and current densities. results follow [18], where energy consumption increases with higher voltages and current densities. In this work, values of standard reduction potentials at different concentrations, temperatures and In this work, values of standard reduction potentials at different concentrations, temperatures pH variations were determined, according to the Nernst equation. The standard reduction potential and pH variations were determined, according to the Nernst equation. The standard reduction for cathodic and anodic reactions at 25 ◦C was −0.827 V and 1.358 V, respectively. At 75 ◦C and 85 ◦C, potential for cathodic and anodic reactions at 25 °C was −0.827 V and 1.358 V, respectively. At 75 °C the equilibrium potential for the cathodic half-reaction resulted between −0.844 V and −0.870 V. On the and 85 °C, the equilibrium potential for the cathodic half-reaction resulted between −0.844 V and other hand, anodic half-reaction values varied from 1.324 V to 1.336 V. The average difference between −0.870 V. On the other hand, anodic half-reaction values varied from 1.324 V to 1.336 V. The average equilibrium potentials (∆Ee) during experiments was between 2.17 V and 2.19 V. Variations of difference difference between equilibrium potentials (∆Ee) during experiments was between 2.17 V and 2.19 V. between equilibrium potentials can be attributed to concentration variation of electrolytes and pH Variations of difference between equilibrium potentials can be attributed to concentration variation changes during the electrodialysis process. Figure 6 was intended as a simplified Evans diagram of electrolytes and pH changes during the electrodialysis process. Figure 6 was intended as a showing experimental results and fitted curves for potentiodynamic sweeps. Cathodic reaction was simplified Evans diagram showing experimental results and fitted curves for potentiodynamic characterized on nickel and sheet of stainless steel 316, and anodic reaction on graphite at 75 ◦C and sweeps. Cathodic reaction was characterized on nickel and sheet of stainless steel 316, and anodic 85 ◦C. Cathode and anode current densities (ic, ia) were determined by a quotient of current (I) and the reaction on graphite at 75 °C and 85 °C. Cathode and anode current densities (ic, ia) were determined corresponding effective area. by a quotient of current (I) and the corresponding effective area. produced a Figure 6. Kinetics of oxidation (Cl−/Cl and H O/O ) and reduction kinetics (H O/H ) using nickel, −222 22 Figure 6. Kinetics of oxidation (Cl /Cl2 and H2O/O2) and reduction kinetics (H2O/H2) using nickel, stainless steel 316 and graphite at 75 ◦C and 85 ◦C. stainless steel 316 and graphite at 75 °C and 85 °C. According to the results of potentiodynamic sweeps, it was determined that cathodic reactions were According to the results of potentiodynamic sweeps, it was determined that cathodic reactions carried out under mixed control and mass transfer control when nickel and stainless steel 316 cathodes were carried out under mixed control and mass transfer control when nickel and stainless steel 316 were used, respectively. The cathodic reaction on stainless steel 316 exhibited a lower exchange current density and a greater overpotential than the nickel one, therefore nickel as cathodic material offers performance with respect to cell voltage in the membrane electrodialysis cell. Futhermore, potentiodynamic tests in Figure 6 show that by using a nickel cathode, higher current densities could be reached. Regarding anodic reaction, a requirement to increase graphite anode area at least twice inPDF Image | Battery Grade Li Hydroxide by Membrane Electrodialysis
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