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Table 7.4.- Electrochemical values of Reaction 1 obtained from the cyclic voltammetry showed on the Top of Figure 7.15 for the initial cycle. Iox / mAg-1 Ired / mAg-1 Electrode Eox /V Ered /V ΔE / V Ired/Iox CF-rGO/Q 1.17 0.57 CF-HT 1.06 0.67 CF-N 1.24 0.51 0.60 8039 0.39 8182 0.73 7976 -6880 0.86 -7024 0.86 -6862 0.86 On the other hand, the minor redox peak (Reaction 2) (initially thought to be a non-reversible side reaction process (Figure 7.16)273) cannot be evaluated at a scan rate of 20 mV/s, as they overlap with the other redox process. In case the scan speed is diminished to 1 mV/s, Figure 7.15, it can be observed the reversibility of the Tiron redox reaction, which continues the same tendency as Reaction 1. However, not only the values for the different electrodes are much closer, almost even. In this case the side redox reaction can be studied separately. Moreover, it also follows the same trend, although reduction/oxidation ratio changes for the different electrodes as: CF-N (1.08) > CF-HT (1.01) < CF-rGO/Q (0.914), the differential of potential between reduction and oxidation follows (mV): CF-HT (67) < CF-rGO/Q (94) < CF-N (107), seen in Table 7.5. Therefore, considering all the three electrode’s electrochemical results, CF-HT has a better electrochemical performance towards reactions 1 and 2 in terms of reversibility comparatively to the other electrodes studied. It s due to the presence of nitrogen groups facilitating the redox reaction, as well as the C=O groups which are more active towards tiron redox reaction. Figure 7.16. - Michael addition of water as plausible side reaction mechanism of Tiron, while oxidizing and reducing. 169PDF Image | Redox Flow Batteries Vanadium to Earth Quinones
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