Solar-powered Chemistry Uses Carbon Dioxide and Water to Make Feedstock for Fuels, Chemicals

Solar-powered Chemistry Uses Carbon Dioxide and Water to Make Feedstock for Fuels, Chemicals

Producing synthesis gas, a precursor of a variety of fuels and chemicals, no longer requires natural gas, coal or biomass.

Solar-powered synthesis gas could recycle carbon dioxide into fuels and useful chemicals, an international team of researchers has shown.

“If we can generate syngas from carbon dioxide utilizing only solar energy, we can use this as a precursor for methanol and other chemicals and fuels. This will significantly reduce overall CO2 emissions,” said Zetian Mi, professor of electrical and computer engineering at the University of Michigan, who led the study published in the Proceedings of the National Academy of Science.

Composed mainly of hydrogen and carbon monoxide with a little methane, syngas is commonly derived from fossil fuels with the help of electricity. In addition, toxic chemicals are often added to make the process more efficient.

“Our new process is actually pretty simple, but it’s exciting because it’s not toxic, it’s sustainable and it’s very cost effective,” said Roksana Rashid, first author of the study, who performed the experiments as a doctoral student in electrical and computer engineering at McGill University in Canada.

To create a process that uses only solar energy, Mi’s group overcame the difficulty of splitting carbon dioxide molecules, which are among the most stable in the universe. For this, they peppered a forest of semiconductor nanowires with nanoparticles. Those nanoparticles, made of gold coated with chromium oxide, attracted the carbon dioxide molecules and bent them, weakening the bonds between the carbon and oxygen.


A diagram of the semiconductor nanowires made of indium, gallium and nitrogen—decorated with gold and chromium oxide nanoparticles

A diagram of the semiconductor nanowires made of indium, gallium and nitrogen—decorated with gold and chromium oxide nanoparticles. When the light hits the nanowire, it frees up electrons and the positively charged “holes” that electrons leave behind. On the nanowire itself, the holes oxidize water into protons (hydrogen) and oxygen. Meanwhile, some electrons are drawn into the metal nanoparticles, where they break apart carbon dioxide. The molecules recombine into the carbon monoxide, hydrogen and methane molecules that make up syngas. 


The gallium nitride nanowires used the light energy to free electrons and the positively charged spaces they leave behind, known as holes. The holes split water molecules, separating the protons (hydrogen) from the oxygen. Then, at the metal catalysts, the electrons split the carbon dioxide, producing carbon monoxide and sometimes drawing in the free hydrogen to make methane. Processes are under development to separate the oxygen from the other gases.

“Our technology sheds light on how to build distributed syngas production from air, water and sunlight,” said Baowen Zhou, co-corresponding author of the study with Mi and a former postdoctoral research fellow in Mi’s lab at McGill University and U-M. 

By changing the ratio of gold to chromium oxide in the nanoparticles, Mi’s team was able to control the relative amounts of hydrogen and carbon monoxide produced in the reaction. This is important because the ratio of hydrogen to carbon monoxide affects how easy it is to produce a type of fuel or chemical.

“What is surprising is the synergy between gold and chromium oxide to make the CO2 reduction to syngas efficient and tunable. That was not possible with a single metal catalyst,” Mi said. “This opens up many exciting opportunities that were not previously considered.”

Mi’s tunable syngas setup uses standard industrial manufacturing processes, and is scalable. While Rashid used distilled water in this experiment, seawater and other electrolyte solutions are also expected to work, and Mi has used them in related water-splitting studies. 

“The semiconductor we use as the light absorber is based on silicon and gallium nitride, which are the most commonly produced semiconductors, and we use very little material for the gallium nitride. Each nanowire is about one micrometer in thickness,” Mi said.

Mi’s next goal is to increase the efficiency of the device, which currently stands at 0.89%. When 10% of the light energy is converted to chemical energy, he hopes that the technology could see the technology be adopted for renewable energy, similar to solar cells.

Read the original article on University of Michigan.