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2 Vanadium Redox Flow Battery Review Electrochemical Processes within a VRFB In a VRFB oxidation of π2+ and reduction of π3+ occurs at the negative electrode: π3+ +πβ βπ2+ (πΈ0 = β0.255ππ£π ππ»πΈ) (2.1) The oxidation of ππ2+ and reduction of ππ+ occurs at the positive electrode and is also a one 2 electron transfer reaction: ππ+ +2π»+ +πβ βππ2+ +π» π(πΈ0 = +0.991ππ£π ππ»πΈ) (2.2) 22 Many applications will require higher voltages, thus cells are often connected together by bi- polar plates, mechanically in parallel but electronically in series to create stacks with higher voltages. For the redox couples described in Equations 1 and 2, the reversible cell potential, πΈπππ£ can be found from a modified verison of the Nernst equation. During charging and discharging the state of charge (SOC) of the battery is constantly changing, this influences the reversible cell potential, as the concentration of each vanadium ion depends on the SOC. As two protons participate in the reduction of ππ+, the reversible cell potential is related to the log of the 2 squared proton concentration. Additionally, with the Donnan potential which accounts for differences in the proton concentration across the membrane, between the positive and negative electrolyte [55, 56]: πΈ πππ£ + πππ 2 πππ =πΈ0+π πππ(πΆππ2.πΆπ2+.(πΆπ»+ ).πΆπ»+ ) ππΉ πΆ 2+ .πΆ 3+ .πΆπππ ππ π π»+ (2.3) 14PDF Image | Electron Transfer Kinetics in Redox Flow Batteries
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