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3. Results and Discussion To screen the impact of electrolyte purification on the electrolytes, we performed cyclic voltammograms (CVs) in a three-electrode cell at 50 °C; electrolyte concentration and composition were chosen in accordance with full cell experiments (i.e., mixed electrolyte with 1.0 M FeCl2 and 1.0 M CrCl3 in 3.0 M HCl). The Cr redox reaction is known to be sluggish at room temperatures [38], thus requiring elevated temperatures to proceed at acceptable rates. However, hydrogen (H2) readily evolves at the Cr redox potential, reducing access to catalyst sites due to bubble formation, and lower efficiencies; these side effects are exacerbated by the elevated temperatures needed to facilitate the Cr reaction. Figure V-2 - Cyclic voltammograms of electrochemically purified (blue) and unpurified (red) electrolytes at a scan rate of 50 mV s–1. The purified electrolyte was harvested from the negative electrolyte after a purification. The electrolyte composition was 1.0 M FeCl2 / 1.0 M CrCl3 in 3.0 M HCl, at a temperature of 50 °C. The working, counter, and reference electrodes used were a glassy carbon disk, a Pt coil, and Ag/AgCl in 3 M NaCl. Figure V-2 shows CVs for electrochemically purified (“ePurified,” blue) and unpurified (red) electrolyte conducted at a scan rate of 50 mV s–1. The solid and dashed lines show the directions of oxidative and reductive sweeps, respectively. The relatively facile and reversible Fe2+/3+ redox 94PDF Image | Bringing Redox Flow Batteries to the Grid
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