V. Focused Fundamental Research - EERE - U.S. Department of ...
V. Focused Fundamental Research - EERE - U.S. Department of ...
V. Focused Fundamental Research - EERE - U.S. Department of ...
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V.B.7 Role <strong>of</strong> Surface Chemistry on the Cycling and Rate Capability <strong>of</strong> Li Positive Electrode Materials (MIT)<br />
Shao-Horn – MIT<br />
Considering XPS analysis <strong>of</strong> powder LiOH (not shown)<br />
indicated that the surface region <strong>of</strong> LiOH consisted mostly<br />
<strong>of</strong> lithium carbonate, the surface region <strong>of</strong> reference Li 2 O 2<br />
powder observed here more likely consists <strong>of</strong> Li 2 O 2 . The O<br />
1s spectrum <strong>of</strong> Li 2 O reference powder (Figure V - 36, right<br />
panel) consists <strong>of</strong> two components: 1) a major component<br />
at 530.9 eV, which is close to those reported for LiOH; 2)<br />
a minor component (~2%) at 528.4 eV, which is attributed<br />
to O 2- ion in Li 2 O. Based on the major component at 530.9<br />
eV, it is postulated that the surface <strong>of</strong> reference Li 2 O is<br />
largely LiOH in nature as Li 2 O is known to be extremely<br />
moisture-sensitive.<br />
The O 1s regions for the pristine electrodes (Figure V -<br />
36, left panel) display a double peak structure that can be<br />
associated with oxygen bond to CF x groups (i.e., CF-O<br />
CF 2 ) at 535 eV and SO 3 groups at 532 eV in Nafion. After<br />
discharge (Figure V - 36, right panel), the CF-O-CF 2<br />
component at 535 eV from Nafion disappeared, which<br />
indicates the buildup <strong>of</strong> discharge products on the<br />
electrode surface. The majority <strong>of</strong> the oxygen signal for<br />
the discharged electrodes is attributed to the formation <strong>of</strong><br />
Li 2 O 2 at 531.0 eV for all discharge electrodes. However,<br />
the formation <strong>of</strong> LiOH cannot be ruled out. The formation<br />
<strong>of</strong> Li 2 O can be ruled out by the lack <strong>of</strong> an oxygen<br />
component with binding energy in the range <strong>of</strong> 528-529<br />
eV. In addition, a second component was identified at<br />
~533.0 eV for the discharged electrodes, which can be<br />
associated with Li 2 CO 3 and/or O-C=O (532.1 eV) and<br />
oxygen singly bonded with carbon atom in O-C=O (533.5<br />
eV). The formation <strong>of</strong> Li 2 O 2 (majority) and minority<br />
Li 2 CO 3 for all discharge electrodes is also supported by the<br />
Li 1s spectra <strong>of</strong> Figure V - 37.<br />
Electrochemical activity <strong>of</strong> high-energy Li-rich<br />
(Li 2 O) x (MO 2 )y systems. Positive electrodes <strong>of</strong> lithium<br />
peroxide and lithium oxide (Li 2 O x ) were shown to exhibit<br />
higher energy densities compared to LiCoO 2 cells (Bruce<br />
et al., JACS 2006). However, the overpotential required to<br />
charge the Li-Li 2 O x cells is ~1.5 V owing to the slow<br />
reaction rate associated with decomposing Li 2 O x . In order<br />
to efficiently operate the high energy Li-Li 2 O x cells, we<br />
have applied nanoparticles <strong>of</strong> platinum (Pt) and gold (Au)<br />
to facilitate the charging reaction rates where Pt was<br />
shown to have the highest charging activity among Pt, Au<br />
and carbon (Shao-Horn et al. ESSL, 2010). However, the<br />
utilization <strong>of</strong> precious Pt metal is not ideal. Therefore, it is<br />
crucial to identify highly active catalyst with abundant<br />
elements such as Mn, Fe. Co, and Ni for high energy Li<br />
Li 2 O 2 and Li-Li 2 O cells. Here we report the<br />
electrochemical activity for electro-oxidation <strong>of</strong> Li 2 O 2 on<br />
pure carbon, Pt/C, and 40 wt% Co 3 O 4 /C (Co 3 O 4 /C) by<br />
anodic polarization <strong>of</strong> Li 2 O 2 -filled positive electrodes in<br />
1 M LiTFSI DME at 5 mV/s. Co 3 O 4 nanoparticles (NPs)<br />
were synthesized as follows: A solution <strong>of</strong> 10 mL<br />
dichlorobenzene and 10 mL <strong>of</strong> oleylamine was prepared at<br />
room temperature (20°C) in a four-neck flask. The mixture<br />
was heated to 160°C under Ar atmosphere with continuous<br />
stirring. 400mg <strong>of</strong> Co 2 (CO) 8 in 4mL <strong>of</strong> dichlorobenzene<br />
was quickly injected into the above solution and left for 1<br />
hr. The solution was cooled down to room temperature,<br />
and CoO NPs were precipitated by ethanol addition and<br />
collected by centrifugation. The product was re-dispersed<br />
in hexane and separated by ethanol addition and<br />
centrifugation. This procedure was repeated 2 times. The<br />
as-synthesized CoO NPs were transferred to a porcelain<br />
boat and was annealed in a tube furnace at 500°C for 3 hrs<br />
under O 2 which lead to Co 3 O 4 NPs. The heat-treated Co 3 O 4<br />
NPs were loaded onto Vulcan Carbon (Co 3 O 4 : Carbon =<br />
2:3 w/w) yielding 40 wt% Co 3 O 4 /C. The particle<br />
dispersion <strong>of</strong> Co 3 O 4 NPs was uniform with average<br />
particle size 10 nm, as shown in Figure V - 38a.<br />
(a)<br />
(b)<br />
Figure V - 38: (a) TEM image <strong>of</strong> 40 wt% Co3O4/C (b) Li2O2 oxidation curves<br />
<strong>of</strong> pure Carbon, Pt/C, and Co3O4/C in 1 M LiTFSI DME at 5 mV/s<br />
Figure V - 38b shows the net Li 2 O 2 electro-oxidation<br />
currents (carbon-mass normalized), which were obtained<br />
by subtracting carbon-mass normalized currents <strong>of</strong> Li 2 O 2 <br />
free electrodes from those filled with Li 2 O 2 . For C-Li 2 O 2<br />
cells, net currents <strong>of</strong> 200 mA/g carbon were obtained at<br />
4.05V Li , which agrees well with the literature (Bruce et al.,<br />
JACS 2006, JPS 2007, Shao-Horn et al. ESSL, 2010). In<br />
addition, net currents <strong>of</strong> 200 mA/g carbon were obtained at<br />
3.70 V Li for Pt-Li 2 O 2 cells, which is consistent with our<br />
previous study (Shao-Horn et al. ESSL, JACS, 2010). The<br />
application <strong>of</strong> Pt NPs decreases the charge overpotential<br />
by 350 mV compared to that <strong>of</strong> pure Carbon. Furthermore,<br />
Energy Storage R &D 500 FY 2011 Annual Progress Report