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phase formation. The explanation could be linked to a different mechanism of Li2S formation with some delay in this low voltage plateau at high C-rate. In parallel, β-S8 was detected at the end of both charges. This proves that α-sulfur is present in the electrode only at the initial state of the Li/S battery, i.e. before cycling. Once it gets reduced into soluble lithium polysulfides, all further recrystallization/reduction steps involve β-sulfur form, as illustrated on the schematic graph below (Figure 5-21). Figure 5-21. Schematic graph illustrating changes of the active material solid forms upon cycling. 5.6.2. Quantitative interpretation In this part, we mostly focused on Li2S formation/disappearance processes, and on the effect of current density on the kinetic of this reactions. Figure 5-22 presents the evolution of (111) peak intensity as a function of capacity. We can clearly observe the slight hysteresis between formation and re-oxidation of Li2S, even if less pronounced than at lower C-rate. We can also distinguish two steps for both Li2S formation/consumption. However, the difference in the slope is not as remarkable as it was in the case of C/20. It can be also noticed that the presence of Li2S on the electrode surface is much longer during its oxidation, as compared with the moment of the creation. Further detailed interpretation of the possible mechanism based on these observations was not the scope of this manuscript. Chapter 5: In situ and operando XRD 188PDF Image | Accumulateur Lithium Soufre
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