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Study of redox flow battery systems for residential applications The reactions that occur on the positive half-cell during charging and discharging steps are [19, 24]: VO2+ + 2H+ + e- Discharge VO2+ + H2O Charge and the reactions that occur on the negative half-cell during charge and discharge can describe as [19, 24]: V3+ + e- Thus, the overall reaction is [20]: VO2+ + V3+ + H2O 2.1.1 Standard potential Charge V2+ Discharge Charge VO2+ + V2+ + 2H+ Discharge The standard potential, Eo, is the reaction potential of the battery when it is operating at standard conditions: 1 M concentration for vanadium species and a temperature of 25 oC. The standard potential can either be determined from the combination of the standard reduction potentials of redox reactions that occur on each half-cell with Equation 2.1 (Figure 2.2): 𝐸° = 𝐸°+ − 𝐸°− = 1.000 − (−0.255) = 1.255 V (2.1) where Eo+ and Eo- are the standard reduction potential for the redox reactions that occur on the positive and negative half-cell, respectively, in V. Figure 2.2 – Potential diagram for vanadium species in strong acidic solutions (values are in V)[19]. or from thermodynamics considering the change in Gibbs free energy (Equation 2.2) [19, 20, 23]. 𝐸° = − ∆𝐺° (2.2) 𝑛𝐹 where, ∆Go is the standard Gibbs free energy (kJ mol-1), n is the number of electrons (n = 1 for VRFB) involved in the reaction and F is the faraday constant (96 487 C mol-1) [23]. To calculate the standard Gibbs free energy, the standard enthalpy of reaction, ∆Hro, and the standard entropy of reaction, ∆Sro, should be calculated in first place (Equation 2.3): ∆𝐺°= ∆𝐻𝑟°−𝑇∆𝑆𝑟° (2.3) Chapter 2: Vanadium redox flow battery 7PDF Image | Tubular Vanadium Air Redox‐flow battery
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