Catalytic Key Found to Make Methanol From Carbon Dioxide

Brookhaven National Laboratory experiments and computational modeling studies definitively identify the ‘active site’ of a catalyst commonly used for making methanol from CO2. The results will guide the design of improved catalysts for transforming CO2 back into useful chemicals.

Scientists are intensely interested in the catalysts that facilitate this type of chemical conversion. Like molecular dealmakers, catalysts bring the reacting chemicals together in a way that makes it easier for them to break and rearrange their chemical bonds. Understanding details of these molecular interactions could point to strategies to improve the catalysts for more energy-efficient reactions.

The results, published in the journal Science, resolve a longstanding debate about exactly which catalytic components take part in the chemical reactions and should be the focus of efforts to boost performance.

Brookhaven chemist Ping Liu, the study’s lead author, who also holds an adjunct position at nearby Stony Brook University (SBU) said, “This catalyst-made of copper, zinc oxide, and aluminum oxide-is used in industry, but it’s not very efficient or selective. We want to improve it, and get it to operate at lower temperatures and lower pressures, which would save energy.”

But prior to this study, different groups of scientists had proposed two different active sites for the catalyst-a portion of the system with just copper and zinc atoms, or a portion with copper zinc oxide.

Co-author Jose Rodriguez, another Brookhaven chemist associated with SBU explained, “We wanted to know which part of the molecular structure binds and breaks and makes bonds to convert reactants to product-and how it does that.”

To find out, Rodriguez performed a series of laboratory experiments using well-defined model catalysts, including one made of zinc nanoparticles supported on a copper surface, and another with zinc oxide nanoparticles on copper. To tell the two apart, he used an energetic x-ray beam to zap the samples, and measured the properties of electrons emitted. These electronic “signatures” contain information about the oxidation state of the atoms the electrons came from-whether zinc or zinc oxide.

Meanwhile Liu, Jingguang Chen of Brookhaven Lab and Columbia University, and Shyam Kattel, the first author of the paper and a postdoctoral fellow co-advised by Liu and Chen, used computational resources at Brookhaven’s Center for Functional Nanomaterials and the National Energy Research Scientific Computing Center to model how these two types of catalysts would engage in the CO2-to-methanol transformations. These theoretical studies use calculations that take into account the basic principles of breaking and making chemical bonds, including the energy required, the electronic states of the atoms, and the reaction conditions, allowing scientists to derive the reaction rates and determine which catalyst will give the best rate of conversion.

“We found that copper zinc oxide should give the best results, and that copper zinc is not even stable under reaction conditions,” said Liu. “In fact, it reacts with oxygen and transforms to copper zinc oxide.”

Those predictions matched what Rodriguez observed in the laboratory. “We found that all the sites participating in these reactions were copper zinc oxide,” he said.

“In our simulations, all the reaction intermediates – the chemicals that form on the pathway from CO2 to methanol bind at both the copper and zinc oxide,” Kattel said. “So there’s a synergy between the copper and zinc oxide that accelerates the chemical transformation. You need both the copper and the zinc oxide.”

The scientists said optimizing the copper/zinc oxide interface will become the driving principal for designing a new catalyst.

“This work clearly demonstrates the synergy from combining theoretical and experimental efforts for studying catalytic systems of industrial importance,” said Chen. “We will continue to utilize the same combined approaches in future studies.”

For example, said Rodriguez, “We’ll try different configurations of the atoms at the copper/zinc oxide interface to see how that affects the reaction rate. Also, we’ll be going from studying the model system to systems that would be more practical for use by industry.”

An essential tool for this next step will be Brookhaven’s National Synchrotron Light Source II (NSLS-II), another Office of Science User Facility. NSLS-II produces extremely bright beams of x-rays-about 10,000 times brighter than the broad-beam laboratory x-ray source used in this study. Those intense x-ray beams will allow the scientists to take high-resolution snapshots that reveal both structural and chemical information about the catalyst, the reactants, and the chemical intermediates that form as the reaction occurs.

“And we’ll continue to expand the theory,” said Liu. “The theory points to the mechanistic details. We want to modify interactions at the copper/zinc oxide interface to see how that affects the activity and efficiency of the catalyst, and we’ll need the theory to move forward with that as well.”

This is good work and progress. Yet , there is a very long way to go for economic viability in CO2 recycling and getting humanity current with the earth’s carbon cycle.