A new catalyst developed by University of Toronto researchers could make it cheaper and easier to produce hydrogen from water – a process some say is key to storing energy from renewable, but intermittent, sources like solar and wind.
The new catalyst, developed in the lab of University Professor Ted Sargent, uses abundant, low-cost elements to split water molecules into hydrogen and oxygen under conditions like those found in ordinary seawater. That, in turn, could make it feasible to use renewable electricity to produce hydrogen from water and then later reverse the process in an electrochemical fuel cell, resulting in clean power on demand.
“Hydrogen is a hugely important industrial feedstock, but unfortunately today it is derived overwhelmingly from fossil fuels, resulting in a large carbon footprint,” says Sargent, who is the senior author of a paper in Nature Energy that describes the new catalyst. “Electrolysis – water splitting to produce renewable hydrogen and oxygen – is a compelling technology, but it needs further improvements in efficiency, cost, and longevity. “This work offers a fresh strategy to pursue these critically important aims.”
Sargent’s lab, in U of T’s Edward S. Rogers Sr. Department of Electrical and Computer Engineering, is among several research groups around the world racing to create catalysts that lower the amount of electricity needed to split water into hydrogen and oxygen. Currently, the best-performing catalysts rely on platinum, a high-cost material, and operate under acidic conditions.
“Our new catalyst is made from copper, nickel and chromium, which are all more abundant and less costly than platinum,” says Cao Thang Dinh, a co-lead author on the paper along with his fellow postdoctoral researchers Pelayo Garcia De Arquer and Ankit Jain. “But what’s most exciting is that it performs well under pH-neutral conditions, which opens up a number of possibilities.”
Seawater, for example, is the most abundant source of water on earth, Dinh points out. But using seawater with traditional catalysts under acidic conditions would require the salt to be removed first, an energy-intensive process. Operating at neutral pH avoids the high cost of desalination. It could also enable the use of microorganisms to make chemicals such as methanol and ethanol. “There are bacteria that can combine hydrogen and CO2 to make hydrocarbon fuels,” says Garcia De Arquer. “They could grow in the same water and take up the hydrogen as it’s being made, but they cannot survive under acidic conditions.”
Using renewable energy to convert waste CO2 into fuels or other value-added products is the goal of the NRG COSIA Carbon XPrize. A team from Sargent’s lab is among the five finalists in the international competition, vying for a US$7.5-million grand prize. In the paper, the team reports that the “overpotential” achieved with the new catalyst – the amount of electrical energy required to liberate the hydrogen from water – is the lowest ever observed under neutral conditions, though it still lags behind traditional platinum catalysts operated at acidic conditions.
“Creating hydrogen from water under neutral conditions is inherently tough – it’s like trying to make an ice sculpture on a sunny day,” says Phil De Luna, a PhD candidate in materials science and engineering and another of the study’s co-authors.
“As far as we know, this catalyst is the best way to do it.”