Communication
pubs.acs.org/JACS
Magnesium Antimony Liquid Metal Battery for Stationary
Energy Storage
David J. Bradwell, Hojong Kim,* Aislinn H. C. Sirk, and Donald R. Sadoway*
Department of Materials Science and Engineering, Massachusetts Institute of Technology, 77 Massachusetts Avenue, Cambridge,
Massachusetts 02139-4307, United States
* Supporting Information
S
ABSTRACT: Batteries are an attractive option for grid-
scale energy storage applications because of their small
footprint and flexible siting. A high-temperature (700 C)
magnesium antimony (MgSb) liquid metal battery
comprising a negative electrode of Mg, a molten salt
electrolyte (MgCl2 KCl NaCl), and a positive electrode
of Sb is proposed and characterized. Because of the
immiscibility of the contiguous salt and metal phases, they
stratify by density into three distinct layers. Cells were
cycled at rates ranging from 50 to 200 mA/cm2 and
demonstrated up to 69% DC DC energy efficiency. The
self-segregating nature of the battery components and the
use of low-cost materials results in a promising technology
for stationary energy storage applications.
L arge-scale energy storage is poised to play a critical role in
enhancing the stability, security, and reliability of
tomorrow s electrical power grid, including the support of
intermittent renewable resources.1 Batteries are appealing because Figure 1. Sectioned MgSb liquid metal battery operated at 700 C
showing the three stratified liquid phases upon cooling to room
of their small footprint and flexible siting; however, conventional
temperature. The cell was filled with epoxy prior to sectioning.
battery technologies are unable to meet the demanding low-cost
and long-lifespan requirements of this application.
where R is the gas constant, T is temperature in Kelvins, F is the
A high-temperature (700 C) magnesium antimony (MgSb)
Faraday constant, aMg(in Sb) is the activity of Mg dissolved in Sb,
liquid metal battery comprising a negative electrode of Mg, a
and aMg is the activity of pure Mg.
molten salt electrolyte (MgCl2 KCl NaCl), and a positive
Recent work on self-healing Li Ga electrodes for lithium ion
electrode of Sb is proposed (Figure 1). Because of density batteries has demonstrated the appeal of liquid components.2
differences and immiscibility, the salt and metal phases stratify into While solid electrodes are susceptible to mechanical failure by
mechanisms such as electrode particle cracking,3 these are
three distinct layers. During discharge, at the negative electrode Mg
is oxidized to Mg2+ (Mg Mg2+ + 2e ), which dissolves into the inoperative in liquid electrodes, potentially endowing cells with
unprecedented lifespans. The self-segregating nature of liquid
electrolyte while the electrons are released into the external circuit.
Simultaneously, at the positive electrode Mg2+ ions in the electro- electrodes and electrolytes could also facilitate inexpensive
lyte are reduced to Mg (Mg2+ + 2e MgSb), which is deposited manufacturing of a battery so constructed. However, there do
not appear to be economical materials options that exist as
into the Sb electrode to form a liquid metal alloy (Mg Sb) with
liquids at or near room temperature.
attendant electron consumption from the external circuit (Figure 2).
Previous work with elevated-temperature liquid batteries demon-
The reverse reactions occur when the battery is charged. Charging
strated impressive current density capabilities (>1000 mA/cm2
and discharging of the battery are accompanied by volumetric when discharged at 0 V) with a variety of chemistries.4 7 However,
changes in the liquid electrodes. The difference in the chemical that work generally used prohibitively expensive metalloids (such as
potentials of pure Mg ( Mg) and Mg dissolved in Sb [ Mg(in Sb)] Bi and Te) as the positive electrode. The resulting cells exhibited
self-discharge current densities of 40 mA/cm2, attributed to the
generates a voltage that can be expressed as
solubility of the negative electrode metal (i.e., Na) in the
RT aMg(in Sb)
Ecell = ln Received: October 17, 2011
2F aMg
Published: January 6, 2012
dx.doi.org/10.1021/ja209759s J. Am. Chem.Soc. 2012, 134, 1895 1897
1895
2012 American Chemical Society
Journal of the American Chemical Society Communication
Figure 2. Schematic of a MgSb liquid metal battery comprising three liquid layers that operates at 700 C. During charging, Mg is electrochemically
extracted from the Mg Sb alloy electrode and deposited as liquid Mg on the top (negative) electrode. During discharging, the Mg electrode is
consumed, and Mg is deposited into the Mg Sb liquid bottom (positive) electrode. During charging, the battery consumes energy; upon discharge,
the battery supplies energy.
electrolyte.5 These systems failed to achieve commercial Further electrochemical characterization was performed.
Stepped-potential experiments indicated low leakage current
success, possibly because of a lack of interest in grid-scale
densities of
storage at that time or the use of high-cost metalloids.
systems. This was attributed to the complexation of Mg2+ by
Sb is less costly ($7/kg average commodity price over the
ligand donors from the supporting electrolyte (NaCl, KCl)13
past 5 years) and more earth-abundant than Bi ($24/kg) and
Te ($150/kg).8 When costs are compared on a per-mole basis and the attendant suppression of metal solubility in its halide
salts.14
(which is more relevant when considering the cost per unit of
Cells cycled at 50 mA/cm2 for a predefined discharge period
energy storage capacity), Sb ($0.74/mol) appears even more
of 10 h to a cutoff charging voltage limit of 0.85 V achieved a
appealing than Bi ($4.40/mol) and Te ($19.19/mol). Interestingly,
round-trip Coulombic efficiency of 97% and a voltage efficiency
the use of Sb had not, until now, been demonstrated in a liquid
of 71%, resulting in an overall energy efficiency of 69% (Figure 3a).
metal battery.
Mg was selected as the negative electrode material on the
basis of its low cost ($5.15/kg, $0.125/mol), high earth
abundance, low electronegativity, and overlapping liquid range
with both Sb and candidate electrolytes. The electrolyte was
MgCl2:NaCl:KCl (50:30:20 mol %), which was selected on the
basis of its sufficiently low melting point (396 C9) and the
greater electrochemical stability of NaCl and KCl in
comparison with MgCl2.10
MgSb single cell batteries were assembled in the fully
charged state in an Ar-filled glovebox, placed inside a sealed test
vessel, and heated in a vertical tube furnace to 700 C. When
the cell was heated above the melting point of the molten salt,
cell open-circuit voltages were found to stabilize at 0.44 V,
consistent with thermodynamic data.11
The cells were electrochemically characterized by cyclic
voltammetry (CV) and electrochemical impedance spectrosco-
py (EIS) using a two-electrode electrochemical setup with the
negative electrode (Mg) as the counter electrode/reference
electrode and the positive electrode (Sb) as the working
electrode. The cells exhibited negligible charge-transfer over-
potentials, as demonstrated by the linearity of the current voltage
relationship in the CV scans and the absence of an obvious
semicircle in the EIS scans. The slope of the CV was consistent
with the area-normalized solution resistance as measured through Figure 3. Electrochemical performance of a MgSb liquid metal
EIS (typically 1.1 cm2), further demonstrating IR voltage loss to battery operated at 700 C. (a) Variation of the cell voltage with the
be the dominant overpotential. state of charge over one cycle. The current was set at 50 mA/cm2. (b)
There were, however, indications of mass-transport limi- Deep discharge results at different current rates. The theoretical cell
EMF was calculated from data in the literature.11
tations under certain conditions. The cells exhibited increased
cell impedance at lower EIS scan frequencies, suggesting that at
At full discharge, the composition of the positive (bottom) liquid
long time periods the reaction rates might be limited by
diffusion.12 Mass-transport limitations could arise from local electrode was estimated to be 12 mol % Mg and 88 mol % Sb.
depletion of Mg2+ ions in the electrolyte at either of the Cells were fully discharged at various rates ranging from 50
electrode electrolyte interfaces or Mg mass-transport limi- to 200 mA/cm2 with 0.05 V as the discharge cutoff limit
tations in the Mg Sb electrode at the Mg Sb electrode (Figure 3b). Operation at higher current density resulted in
electrolyte interface. increased IR voltage loss and decreased capacity, consistent
dx.doi.org/10.1021/ja209759s J. Am. Chem.Soc. 2012, 134, 1895 1897
1896
Journal of the American Chemical Society Communication
with the measured solution resistance and observed mass- Future work will include long-term corrosion testing of solid-state
components, current collector optimization, and investigation of
transport limitations. The operating efficiency could be
alternative sheath materials. While the initial cell performance
improved by reducing the thickness of the electrolyte or
results are promising, exploration of other metal metalloid
operating at lower current density. The cell performance could
couples with still greater cell voltages and lower operating
be optimized by changes in the current collector design and in
temperatures is warranted. If a low-cost, high-voltage system
the electrolyte composition to increase the cell conductivity.
with sufficiently low levels of corrosion were discovered, it would
Cells were cycled more than 30 times for periods of up to 2
find utility in a wide array of stationary storage applications.
weeks and did not exhibit obvious signs of corrosion of the
solid-state cell components (current collectors and walls), as
ASSOCIATED CONTENT
determined through optical imaging and scanning electron
* Supporting Information
S
microscopy (SEM)/energy-dispersive spectroscopy (EDS)
Experimental procedures, cell design details, heating profile,
analysis. Analysis of the positive electrodes of cells that were
materials selection, and additional electrochemical results. This
cooled in a discharged state revealed the presence of Mg
material is available free of charge via the Internet at http://
platelets, consistent with the formation of Mg3Sb2 (Figure 4).
pubs.acs.org.
AUTHOR INFORMATION
Corresponding Author
abqq6g@r.postjobfree.com; abqq6g@r.postjobfree.com
Present Address
Department of Law, University of Victoria, Victoria, BC,
Canada.
ACKNOWLEDGMENTS
Financial support from the Deshpande Center for Technological
Innovation at MIT, the Chesonis Family Foundation at MIT, the
Advanced Research Projects Agency-Energy (U.S. Department of
Energy), and Total, S.A. is gratefully acknowledged.
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dx.doi.org/10.1021/ja209759s J. Am. Chem.Soc. 2012, 134, 1895 1897
1897