Lithium-oxygen batteries boast energy density levels comparable to fossil fuels and are thus seen as a promising candidate for future transportation-related energy needs. Several roadblocks stand in the way of realizing that vision, however. They include poor rechargeability, reduced efficiency due to high over-potentials (more charge energy than discharge energy) and low specific energy.
Two instabilities contribute to these roadblocks. Much of the previous work done in the lab of Lynden Archer, professor of engineering in the Robert F. Smith School of Chemical and Biomolecular Engineering (CBE) at Cornell University, has centered on one. The nucleation and growth of dendrites from one electrode to the other, which causes short-circuiting, a source of premature cell failure that invariably ends in fires.
It's the other instability – the loss of battery power, also known as capacity fade – that is the focus of the lab's most recent work. Snehashis Choudhury, a doctoral student in the Archer research group, has come up with what Archer terms an "ingenious" answer to the problem of capacity fade. This work is detailed in a paper in Science Advances; Choudhury is co-first author along with Charles Wan, a chemical engineering major.
Capacity fade occurs when the electrolyte, which transports charged ions from the negative electrode (anode) to the positive (cathode), reacts with the electrodes. "It starts to consume the electrodes," Choudhury said. "It forms many insulating products that impede ion transport. Over time, these build up to produce such prohibitive internal cell resistance that finally the battery fades."
The problem then is how do you stop one electrolyte-electrode reaction, when it's another necessary reaction between the two – the transfer of ions – that produces power? Choudhury's solution is called an artificial solid-electrolyte interphase (SEI), a material that protects the electrodes while promoting the flow of electrons from one end of the cell to the other.
"[The reaction between the electrolyte and electrodes] starts to consume the electrodes. It forms many insulating products that impede ion transport. Over time, these build up to produce such prohibitive internal cell resistance that finally the battery fades."Snehashis Choudhury, Cornell University
"Such interphases form naturally in all electrochemical cells ... and their chemo-mechanical stability is critical to the success of the graphite anode in lithium-ion batteries," Archer said.
Choudhury's approach for creating a functional designer interphase is based on bromide-containing ionic polymers (ionomers) that selectively tether to the lithium anode, forming a few-nanometers-thick conductive coating that protects the electrode from degradation and fade. The SEI ionomers display three attributes that allow for increased stability during electrodeposition: protection of the anode against growth of dendrites; reduction-oxidation (redox) mediation, which reduces charge over-potentials; and the formation of a stable interphase with lithium, protecting the metal while promoting ion transport.
One challenge still exists: all research-grade lithium-oxygen electrochemical cells are evaluated using pure oxygen as the active cathode material. For a commercially-viable lithium-oxygen (or lithium-air, as it's also known) cell, it would need to pull oxygen out of the air, and that oxygen comes with other reactive components, such as moisture and carbon dioxide.
If the inefficiencies that limit the performance of lithium-oxygen fuel cells can be resolved, the exceptional energy storage options offered by the cell chemistry would be a giant step forward for electrified transportation and a revolutionary advance for autonomous robotics, Archer said.
"It is telling from observations of the most advanced humanoid robots that they are always either tethered to an ultra-long electrical cable or are using something like a loud lawnmower engine to generate energy," he said. "Either energy source compares poorly to those found in nature. Energy storage technologies such as lithium-air cells, which harness materials from the surroundings, promise to close this gap."
This story is adapted from material from Cornell University, with editorial changes made by Materials Today. The views expressed in this article do not necessarily represent those of Elsevier. Link to original source.