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Figure 1. 3. A schematic of the fundamental operation of RFBs. Positive and negative electrolytes are pumped into the battery. Electrolytes passing through the electrodes trade electrons via an external circuit, alongside trading ions through the IEM. All-vanadium redox flow batteries (VRFBs) are aqueous RFBs, which utilize four different states of vanadium ions for operation. VRFBs are the most studied RFBs, due to the simplicity of using various ions of one metal, instead of two or more base chemical compounds, as anode and cathode. Additionally, anions and cations are dissolved in the same solvent. Hence, the cell is stabilized by omitting the crossover of electrolytes; a problem occurring when employing different anolytes and catholytes. [2,5,9] The common solvent is diluted aqueous sulfuric acid for VRFBs. However, the dissolution of vanadium salt is limited to 1.7 M in this solvent, limiting the energy density of VRFBs. A couple of studies have suggested various additives for improving the solubility of vanadium up to 3 M, which leads to more energy-dense VRFBs. [3,10] The electrochemical reactions of VRFBs are presented in Equations 1.1 and 1.2 for positive and negative electrodes. As deduced from these equations, the open circuit potential is 1.26V. Positive:VO+ +2H+ +e− ↔VO2+ +H O,E0 =1.0Vvs.SHE (1.1) 22 Negative: V3+ + e− ↔ V2+, E0 = −0.26 V vs. SHE (1.2) VO2+ ions are oxidized to VO2+ ions in the positive half-cell reaction, and V3+ ions are reduced to V2+ ions in the negative half-cell reaction during the charging cycle. In other words, these ions transform into their more unstable states with higher energy differences by storing energy or being “charged”. The unstable ions VO2+ and V2+ take their more stable forms, VO2+ and V3+, respectively, during the discharging cycle. during this process, energy stored in the ions is released or the cell is “discharged”. 5PDF Image | Analysis of Fluid Flow in Redox Flow Batteries
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