Researchers take a step toward carbon-capturing batteries
What if there were a battery that could release energy while trapping carbon dioxide? This isn’t science fiction; it’s the promise of lithium-carbon dioxidebatteries, which are currently a hot research topic.
Li-CO₂ batteries could be a two-in-one solution to the current problems of storing renewable energy and taking carbon emissions out of the air. They absorb carbon dioxide and convert it into a white powder called lithium carbonate while discharging energy.
These batteries could have profound implications for cutting emissions from vehicles and industry—and might even enable long-duration missions on Mars, where the atmosphere is 95% CO₂.
To make these batteries commercially viable, researchers have mainly been wrestling with problems related to recharging them. Now, our team at the University of Surrey has come up with a promising way forward. So how close are these “CO₂-breathing” batteries to becoming a practical reality?
Like many great scientific breakthroughs, Li-CO₂ batteries were a happy accident. Slightly over a decade ago, a U.S.-French team of researchers were trying to address problems with lithium air batteries, another frontier energy-storage technology. Whereas today’s lithium-ion batteries generate power by moving and storing lithium ions within electrodes, lithium air batteries work by creating a chemical reaction between lithium and oxygen.
The problem has been the “air” part, since even the tinyvolume of CO₂ that’s found in air is enough to disrupt this careful chemistry, producing unwanted lithium carbonate. As many battery scientists will tell you, the presence of Li₂CO₃ can also be a real pain in regular lithium-ion batteries, causing unhelpful side reactions and electrical resistance.
Nonetheless the scientists noticed something interesting about this CO₂ contamination: It improved the battery’s amount of charge. From this point on, work began on intentionally adding CO₂ gas to batteries to take advantage of this, and the lithium-CO₂ battery was born.
How it works
Their great potential relates to the chemical reaction at the positive side of the battery, where small holes are cut in the casing to allow CO₂ gas in. There it dissolves in the liquid electrolyteand reacts with lithium that has already been dissolved there. During this reaction, it’s believed that four electrons are exchanged between lithium ions and carbon dioxide.
This electron transfer determines the theoretical charge that can be stored in the battery. In a normal lithium-ion battery, the positive electrode exchanges just one electron per reaction.The greater exchange of electrons in the lithium-carbon dioxide battery, combined with the high voltage of the reaction, explains their potential to greatly outperform today’s lithium-ion batteries.
However, the technology has a few issues. The batteries don’t last very long. Commercial lithium-ion packs routinely survive 1,000 to 10,000 charging cycles; most LiCO₂ prototypes fade after fewer than 100.
They’re also difficult to recharge. This requires breaking down the lithium carbonate to release lithium and CO₂, which can be energy intensive. This energy requirement is a little like a hill that must be cycled up before the reaction can coast, and is known as overpotential.
You can reduce this requirement by printing the right catalyst material on the porous positive electrode. Yet these catalysts are typically expensive and rare noble metals, such as ruthenium and platinum, making for a significant barrier to commercial viability.
Our team has found an alternative catalyst, caesium phosphomolybdate, which is far cheaper and easy to manufacture at room temperature. This material made the batteries stable for 107 cycles, while also storing 2.5 times as much charge as a lithium ion. And we significantly reduced the energy cost involved in breaking down lithium carbonate, for an overpotential of 0.67 volts, which is only about double what would be necessary in a commercial product.
Our research team is now working to further reduce the cost of this technology by developing a catalyst that replaces caesium, since it’s the phosphomolybdate that is key. This could make the system more economically viable and scalable for widespread deployment.
We also plan to study how the battery charges and discharges in real time. This will provide a clearer understanding of the internal mechanisms at work, helping to optimize performance and durability.
A major focus of upcoming tests will be to evaluate how the battery performs under different CO₂ pressures. So far, the system has only been tested under idealized conditions. If it can work at 0.1 bar of pressure, it will be feasible for car exhausts and gas boiler flues, meaning you could capture CO₂ while you drive or heat your home.
Demonstrating that this works will be an important confirmation of commercial viability, albeit we would expect the battery’s charge capacity to reduce at this pressure. By our rough calculations, 1kg of catalyst could absorb around 18.5kg of CO₂. Since a car driving 100 miles emits around 18kg to 20kg of CO₂, that means such a battery could potentially offset a day’s drive.
If the batteries work at 0.006 bar, the pressure on the Martian atmosphere, they could power anything from an exploration rover to a colony. At 0.0004 bar, Earth’s ambient air pressure, they could capture CO₂ from our atmosphere and store power anywhere. In all cases, the key question will be how it affects the battery’s charge capacity.
Meanwhile, to improve the battery’s number of recharge cycles, we need to address the fact that the electrolyte dries out. We’re currently investigating solutions, which probably involve developing casings that only CO₂ can move into. As for reducing the energy required for the catalyst to work, it’s likely to require optimizing the battery’s geometry to maximize the reaction rate—and to introduce a flow of CO₂, comparable to how fuel cells work.
If this continued work can push the battery’s cycle life above 1,000 cycles, cut overpotential below 0.3 V, and replace scarce elements entirely, commercial Li-CO₂ packs could become reality. Our experiments will determine just how versatile and far-reaching the battery’s applications might be, from carbon capture on Earth to powering missions on Mars.
Daniel Commandeur is a Surrey Future Fellow at the School of Chemistry & Chemical Engineering at the University of Surrey.
Mahsa Masoudi is a PhD researcher of chemical engineering at the University of Surrey.
Siddharth Gadkari is a lecturer in chemical process engineering at the University of Surrey.
This article is republished from The Conversation under a Creative Commons license. Read the original article.
#researchers #take #step #toward #carboncapturingResearchers take a step toward carbon-capturing batteries
What if there were a battery that could release energy while trapping carbon dioxide? This isn’t science fiction; it’s the promise of lithium-carbon dioxidebatteries, which are currently a hot research topic.
Li-CO₂ batteries could be a two-in-one solution to the current problems of storing renewable energy and taking carbon emissions out of the air. They absorb carbon dioxide and convert it into a white powder called lithium carbonate while discharging energy.
These batteries could have profound implications for cutting emissions from vehicles and industry—and might even enable long-duration missions on Mars, where the atmosphere is 95% CO₂.
To make these batteries commercially viable, researchers have mainly been wrestling with problems related to recharging them. Now, our team at the University of Surrey has come up with a promising way forward. So how close are these “CO₂-breathing” batteries to becoming a practical reality?
Like many great scientific breakthroughs, Li-CO₂ batteries were a happy accident. Slightly over a decade ago, a U.S.-French team of researchers were trying to address problems with lithium air batteries, another frontier energy-storage technology. Whereas today’s lithium-ion batteries generate power by moving and storing lithium ions within electrodes, lithium air batteries work by creating a chemical reaction between lithium and oxygen.
The problem has been the “air” part, since even the tinyvolume of CO₂ that’s found in air is enough to disrupt this careful chemistry, producing unwanted lithium carbonate. As many battery scientists will tell you, the presence of Li₂CO₃ can also be a real pain in regular lithium-ion batteries, causing unhelpful side reactions and electrical resistance.
Nonetheless the scientists noticed something interesting about this CO₂ contamination: It improved the battery’s amount of charge. From this point on, work began on intentionally adding CO₂ gas to batteries to take advantage of this, and the lithium-CO₂ battery was born.
How it works
Their great potential relates to the chemical reaction at the positive side of the battery, where small holes are cut in the casing to allow CO₂ gas in. There it dissolves in the liquid electrolyteand reacts with lithium that has already been dissolved there. During this reaction, it’s believed that four electrons are exchanged between lithium ions and carbon dioxide.
This electron transfer determines the theoretical charge that can be stored in the battery. In a normal lithium-ion battery, the positive electrode exchanges just one electron per reaction.The greater exchange of electrons in the lithium-carbon dioxide battery, combined with the high voltage of the reaction, explains their potential to greatly outperform today’s lithium-ion batteries.
However, the technology has a few issues. The batteries don’t last very long. Commercial lithium-ion packs routinely survive 1,000 to 10,000 charging cycles; most LiCO₂ prototypes fade after fewer than 100.
They’re also difficult to recharge. This requires breaking down the lithium carbonate to release lithium and CO₂, which can be energy intensive. This energy requirement is a little like a hill that must be cycled up before the reaction can coast, and is known as overpotential.
You can reduce this requirement by printing the right catalyst material on the porous positive electrode. Yet these catalysts are typically expensive and rare noble metals, such as ruthenium and platinum, making for a significant barrier to commercial viability.
Our team has found an alternative catalyst, caesium phosphomolybdate, which is far cheaper and easy to manufacture at room temperature. This material made the batteries stable for 107 cycles, while also storing 2.5 times as much charge as a lithium ion. And we significantly reduced the energy cost involved in breaking down lithium carbonate, for an overpotential of 0.67 volts, which is only about double what would be necessary in a commercial product.
Our research team is now working to further reduce the cost of this technology by developing a catalyst that replaces caesium, since it’s the phosphomolybdate that is key. This could make the system more economically viable and scalable for widespread deployment.
We also plan to study how the battery charges and discharges in real time. This will provide a clearer understanding of the internal mechanisms at work, helping to optimize performance and durability.
A major focus of upcoming tests will be to evaluate how the battery performs under different CO₂ pressures. So far, the system has only been tested under idealized conditions. If it can work at 0.1 bar of pressure, it will be feasible for car exhausts and gas boiler flues, meaning you could capture CO₂ while you drive or heat your home.
Demonstrating that this works will be an important confirmation of commercial viability, albeit we would expect the battery’s charge capacity to reduce at this pressure. By our rough calculations, 1kg of catalyst could absorb around 18.5kg of CO₂. Since a car driving 100 miles emits around 18kg to 20kg of CO₂, that means such a battery could potentially offset a day’s drive.
If the batteries work at 0.006 bar, the pressure on the Martian atmosphere, they could power anything from an exploration rover to a colony. At 0.0004 bar, Earth’s ambient air pressure, they could capture CO₂ from our atmosphere and store power anywhere. In all cases, the key question will be how it affects the battery’s charge capacity.
Meanwhile, to improve the battery’s number of recharge cycles, we need to address the fact that the electrolyte dries out. We’re currently investigating solutions, which probably involve developing casings that only CO₂ can move into. As for reducing the energy required for the catalyst to work, it’s likely to require optimizing the battery’s geometry to maximize the reaction rate—and to introduce a flow of CO₂, comparable to how fuel cells work.
If this continued work can push the battery’s cycle life above 1,000 cycles, cut overpotential below 0.3 V, and replace scarce elements entirely, commercial Li-CO₂ packs could become reality. Our experiments will determine just how versatile and far-reaching the battery’s applications might be, from carbon capture on Earth to powering missions on Mars.
Daniel Commandeur is a Surrey Future Fellow at the School of Chemistry & Chemical Engineering at the University of Surrey.
Mahsa Masoudi is a PhD researcher of chemical engineering at the University of Surrey.
Siddharth Gadkari is a lecturer in chemical process engineering at the University of Surrey.
This article is republished from The Conversation under a Creative Commons license. Read the original article.
#researchers #take #step #toward #carboncapturing
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