By Nobuyuki Imanishi, Alan C. Luntz, Peter Bruce
ISBN-10: 148998061X
ISBN-13: 9781489980618
ISBN-10: 1489980628
ISBN-13: 9781489980625
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5 Capacity / mAh 1 Fig. 7 V versus Li/Li+ in 1 M LiTFSI–DME, previously discharged to 1 mAh under O2 [9]. 6 V versus Li/Li+ [24]. Reprinted (adapted) with permission from [9]. Copyright (2011) American Chemical Society. Reprinted (adapted) with permission from [24]. Copyright (2011) John Wiley and Sons powder XRD [3, 9]. However, although it may be more stable than the longer chain ethers, it still decomposes in a similar manner to that described above. Indeed the data in Fig. 9 are for DME. Overall ether-based electrolytes, including the most widely used tetraglyme and DME, are unstable in the rechargeable Li–O2 cell, which results in significant fading after a few cycles (Fig.
14b) involving formation of HCO2Li, CH3CO2Li and Li2CO3. Li2CO3 is seen to be more difficult to oxidise, as noted above, and is therefore only partly removed and accumulates as the dominant side product on cycling (Fig. 14b) in accord with the observed capacity fading (Fig. 13). 2 Nonaqueous Electrolytes a 1 x 10−6 0 Flux (mol min−1) Fig. 05 mV sÀ1. Note the NO and H2O fluxes are magnified by 103 to make them visible on the same plot. Current decrease during discharge is due to increasing filling of the electrode with product.
B3LYP optimised C–O bond lengths in the transition state are shown. 8 kcal molÀ1. The most plausible pathway for the reaction is a nucleophilic attack at the Cα atom, followed by C–S bond cleavage to give a sulfinate anion [34]. Reprinted with permission from [23]. 2 V), sulfonebased electrolytes, with an anodic (oxidation) stability exceeding 5 V versus Li/Li+, have been explored [87–89]. Recently, sulfones have been considered as the basis of electrolytes for nonaqueous Li–O2 batteries [26, 85].
The Lithium Air Battery: Fundamentals by Nobuyuki Imanishi, Alan C. Luntz, Peter Bruce
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