Lithium-ion battery research reaches for higher voltages
For years, small rechargeable lithium-ion batteries have reliably supplied billions of portable devices with energy. But manufacturers of high-energy applications such as electric cars and power storage systems are seeking out new electrode materials and electrolytes.
Michael Metzger, researcher at the Technical University of Munich (TUM), has developed a new battery test cell to investigate anionic and cationic reactions separately. The researcher was honored recently with a significant research prize for his work.
A new battery test cell setup allows anionic and cationic reactions to be investigated separately. [Photo: Monika Weiner/TUM]
Energy storage systems are in demand as never before. Billions of mobile telephones and tablets need electricity to operate. Add to this a growing number of electric cars. But high-performance batteries can also store renewable energy produced by wind turbines and solar cells so that it can be fed into the grid on cloudy and windless days.
"Manufacturers of rechargeable batteries are building on the proven lithium-ion technology, which has been deployed in mobile devices like laptops and cell phones for many years," says TUM researcher Michael Metzger. "However, the challenge of adapting this technology to the demands of electromobility and stationary electric power storage is not trivial."
Standard rechargeable batteries are only marginally suited for high performance. "To raise the energy density, you need to increase the voltage or the capacity, and that is where traditional electrode materials and electrolytic fluids reach their limits," explains the physicist.
Research is running at full gallop around the world. For example, engineers are experimenting with special electrode materials that can provide a voltage of nearly 5 V, instead of the current maximum of 4.2 V to 4.3 V.
But this "battery doping" also has side effects. Changes in the chemical composition of the electrodes and electrolytes can lead to battery performance drops after only a few charging cycles or the formation of gasses at the electrodes that cause the batteries to balloon.
"The future of lithium-ion batteries hinges on getting a grip on these undesirable reactions," says Metzger. He has already fulfilled one prerequisite to this end: The chemical processes that transpire during charging and discharging can be investigated in detail using the new battery test cell he developed with his team.
A test cell for the batteries of the future
The researchers spent three years working on their apparatus. "Normally, electrolytic fluids and electrodes -- the positive cathode and negative anode -- are in a permanent electrochemical exchange," says Metzger. "Thus far, it has not been possible to investigate the reactions at the anode and cathode independently of each other. We are the first to manage this successfully."
The key: The battery test cell, which, like every lithium-ion battery, comprises an anode, a cathode, and electrolytes, is not completely sealed, but rather is fitted with a fine capillary. This allows gasses that are released during charging and discharging to be sampled and investigated using a mass spectrometer.
Metzger was recently honored with the Evonik Research Prize for the development of the battery test cell, which, for the first time, allows mass spectroscopy investigations and an independent analysis of the processes at each electrode. The chemical group Evonik awards the prize annually to an exceptional next-generation scientist.
Water is poison for a battery
Using their test cell, the researchers were, for the first time, able to explain precisely what transpires inside a high-voltage battery. The results demonstrate that the stability of electrodes and electrolytes depends on several factors, for example, charging voltage, operating temperature, and even the tiniest chemical impurities:
- The higher the applied voltage and temperature, the faster the electrolytic fluid decomposes. The gasses released in the process, mainly carbon monoxide and carbon dioxide, can cause the battery enclosure to balloon.
- Even the smallest traces of water that intrude into the cell release hydrogen at the anode and act as an oxidizing agent on the carbon in the cathode. This impairs the conductivity of the electrode.
- The chemical reactions that take place at the anode and cathode lead to interactions. This crosstalk, which has hardly been investigated to date, reduces the overall cell performance.
Measurement in practice
"For industrial end-users, the new measurement methodology is extremely interesting," says Prof. Hubert Gasteiger, who chairs the Department of Technical Electrochemistry. "In our investigations, we were able to show that the development of gasses in batteries can be reduced by adding the right admixtures to the electrolytic fluid or by inhibiting crosstalk between the electrodes."
One research result, in particular, bears a direct consequence in practice: The higher the desired voltage, the less residual moisture the materials may contain. Manufacturers could extend the lifetime of future cells by replacing the electrolyte ethylene carbonate with more stable solution components.
But here, too, the devil is in the details. A small amount of ethylene carbonate is required in current systems to pacify the anode. The new cell allows processes at the anode and the cathode to be observed independently, possibly leading to the discovery of entirely novel solutions.
M. Metzger, P. Walke, B. Strehle, S. Solchenbach, and H. A. Gasteiger: "Anodic Oxidation of Carbon and Electrolyte with Different Conducting Salts in High-Voltage Lithium-Ion Batteries Studied By Online Electrochemical Mass Spectrometry"; Pacific Rim Meeting on Electrochemical and Solid-State Science, 5. Oct. 2016
M. Metzger, B. Strehle, S. Solchenbach, and H. A. Gasteiger: "Hydrolysis of Ethylene Carbonate with Water and Hydroxide under Battery Operating Conditions," J. Electrochem. Soc., 163 (7), A1219-A1225 (2016), DOI: 10.1149/2.0411607jes
M. Metzger, B. Strehle, S. Solchenbach, and H. A. Gasteiger, "Origin of H2-Evolution in LIBs: H2O Reduction vs. Electrolyte Oxidation," J. Electrochem. Soc., 163 (5), A798-A809 (2016), DOI: 10.1149/2.1151605jes
Source: Technical University of Munich
Published February 2017
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