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 ...
Create successful ePaper yourself
Turn your PDF publications into a flip-book with our unique Google optimized e-Paper software.
V.B.12 Developing Materials for Lithium-Sulfur Batteries (ORNL)<br />
Liang – ORNL<br />
Capacity (mAh g -1 )<br />
1400<br />
1200<br />
1000<br />
800<br />
600<br />
400<br />
200<br />
Charge, pore volume 2.35<br />
Discharge, pore volume 2.35<br />
Charge, pore volume 1.12<br />
Discharge, pore volume 1.12<br />
Pore volume 2.35<br />
0<br />
5 10 15<br />
0<br />
20<br />
Cycle Number<br />
Figure V - 65: Cycling performance <strong>of</strong> S/C composites with 50% sulfur<br />
loading. Carbon hosts have pore volumes <strong>of</strong> 2.35 and 1.12 cm 3 /g. Surface<br />
areas are ~ 800 m 2 /g for both materials. Capacity is normalized by the sulfur<br />
alone.<br />
Electrolyte Additives. To overcome the corrosion<br />
problem associated with the LiBr additive, a number <strong>of</strong><br />
alternative compounds have been investigated. Organic<br />
alternatives include benzoquinone,<br />
Tetracyanoquinodimethane (TCNQ), and 2,3-Dichloro<br />
5,6-dicyano-1,4-benzoquinone (DDQ). These compounds<br />
have electrochemical redox potentials between 2.5 and 3.9<br />
V. However, the chemical compatibility <strong>of</strong> benzoquinone<br />
and TCNQ with bare lithium anode is a problem. DDQ has<br />
better chemical stability with lithium metal. It was found<br />
that using DDQ as the additive [5% in tetraglyme] reduces<br />
the capacity <strong>of</strong> S by half. The possible reason for this<br />
unexpected capacity loss could be the polymerization <strong>of</strong><br />
DDQ at high concentration. The resulting polymer coats<br />
the carbon electrode surface and compromises the<br />
electrochemical performance <strong>of</strong> the cathode. When the<br />
concentration <strong>of</strong> DDQ was reduced to 1%, the<br />
electrochemical performance was improved comparing<br />
with the 5% DDQ in tetraglyme. Inorganic alternatives to<br />
LiBr were also investigated. Promising results were<br />
obtained when a phosphorous sulfide additive was used in<br />
the cell. As shown in Figure V - 66a, the charge/discharge<br />
curves have plateaus close to the ideal curves. The cell has<br />
a good retention <strong>of</strong> capacity at 0.1 C rate. The cut-<strong>of</strong>f cell<br />
voltage has been set to 1.9 V because the additive can be<br />
reduced at the cathode when the discharge voltage is below<br />
1.9 V. The stability <strong>of</strong> this phosphorous sulfide additive is<br />
still under investigation. The mechanism <strong>of</strong> how the<br />
additive works will be studied in future experiments.<br />
Protection <strong>of</strong> Lithium Anode. To protect lithium<br />
from reacting with the sulfur species, a novel anode made<br />
<strong>of</strong> metal lithium with a pre-formed solid electrolyte<br />
interphase (SEI) on its surface was designed and<br />
implemented in the Li-S batteries. The tenet <strong>of</strong> the design<br />
is to have an ionic conductor covering the surface <strong>of</strong><br />
lithium metal, thereby impeding surface reaction <strong>of</strong> lithium<br />
with polysulfide.<br />
Lithium thiophosphate salts were chosen to form the<br />
100 SEI. Lithium thiophosphates are fast Li ion conductors.<br />
Their ionic conductivity ranges from 10 -6 to 10 -3 S/cm<br />
80<br />
depending on the composition. It was found that Li 2 S x <br />
60<br />
P 2 S 5 can react with lithium metal to form a solid<br />
electrolyte <strong>of</strong> lithium thiophosphate at the surface <strong>of</strong><br />
40 lithium metal. This solid electrolyte conducts lithium ions<br />
while it blocks the access <strong>of</strong> polysulfide to the lithium.<br />
20 Because the polysulfide shuttle phenomenon is more<br />
Coulombic Efficiency (%)<br />
severe at low cycling rates than at high rates, the cell was<br />
intentionally cycled at a low rate <strong>of</strong> 0.1 C to demonstrate<br />
the protection <strong>of</strong> lithium metal through this solid<br />
electrolyte coating. Shown in Figure V - 67a is the voltage<br />
pr<strong>of</strong>ile <strong>of</strong> the first cycle. The discharge curve has two<br />
plateaus at 2.4 and 2.0 V, corresponding to the reduction <strong>of</strong><br />
long chain polysulfides (sulfur atoms greater than 4) and<br />
short chain polysulfides (sulfur atoms less than 4),<br />
respectively. The ratio <strong>of</strong> the first plateau to the second<br />
plateau is exactly 1:3. The same ratio <strong>of</strong> the high to low<br />
plateaus was found in the charging curve. The constant<br />
ratio <strong>of</strong> 1:3 <strong>of</strong> these plateaus at both charging and<br />
discharge cycles proves that the polysulfide shuttle has<br />
been completely blocked by this solid electrolyte coating<br />
on the surface <strong>of</strong> lithium metal. The coulombic efficiency<br />
shown in Figure V - 67b is above 98% for all cycles. The<br />
energy efficiency is about 90% at 0.1 C. Capacity decay<br />
during cycling was still present. It is known that the<br />
capacity decay is caused by the precipitation <strong>of</strong> Li 2 S in the<br />
liquid electrolyte.<br />
Sample Transfer Stage. A new sample transfer stage<br />
has been developed for taking samples from a glove box to<br />
a scanning electron microscope (SEM) without exposure to<br />
air and moisture. The transfer stage operates by the<br />
difference <strong>of</strong> pressure inside and outside the SEM<br />
chamber: when a sample is loaded in a glove box and<br />
exposed to a slight vacuum, the atmospheric pressure<br />
pushes the lid against the o-ring seal. The sample is<br />
protected by the transfer stage as it is moved from the<br />
glove box to the SEM. After the sample stage is loaded<br />
inside the SEM chamber, the higher vacuum causes the lid<br />
to pop open, thus exposing the sample for imaging. This<br />
sample stage enables the analysis <strong>of</strong> lithium anodes after<br />
battery cycling.<br />
Conclusions and Future Directions<br />
Because <strong>of</strong> the poor electronic conductivity <strong>of</strong> sulfur,<br />
the high surface area carbon is the enabler <strong>of</strong> achieving the<br />
maximum utilization <strong>of</strong> sulfur under electrochemical<br />
cycling. The porosity is important for the retention <strong>of</strong><br />
capacity. With the same sulfur loading, excess pore<br />
volume accommodates liquid electrolyte and facilitates the<br />
mass transport <strong>of</strong> lithium ions. Physical adsorption by<br />
porous carbon is insufficient to completely eliminate the<br />
polysulfide shuttle.<br />
Energy Storage R &D 526 FY 2011 Annual Progress Report