Research reveals mechanism for direct synthesis of hydrogen peroxide

January 20, 2016 by Christine Des Garennes
Instead of reacting together on the surface of the catalyst (the palladium cluster), the hydrogen atoms dissociate into their components -- protons and electrons. The protons enter the surrounding solution of water and methanol, while the electrons flow through the palladium itself into oxygen molecules. Credit: American Chemical Society

From the polyurethane that makes our car seats to the paper made from bleached wood pulp, chlorine can be found in a variety of large-scale manufacturing processes. But while chlorine is good at activating the strong bonds of molecules, which allows manufacturers to synthesize the products we use on a daily basis, it can be an insidious chemical, sometimes escaping into the environment as hazardous byproducts such as chloroform and dioxin.

As a result, scientists and companies have been exploring a more environmentally benign alternative to chlorine—hydrogen peroxide, or H2O2. But it is an expensive reactant. Hydrogen peroxide is typically made in big, centralized facilities and requires significant energy for separation, concentration, and transportation. A handful of large-scale facilities around the globe have begun to produce H2O2 using the current process, but at the same facilities as the polyurethane precursors, which results in significant cost and energy savings and reduces environmental impact. Ideally smaller-scale factories would also be able to make hydrogen peroxide on site, but this would require a completely different set of chemistry, direct synthesis of H2O2 from hydrogen and oxygen gas, which has long been poorly understood according to researchers at the University of Illinois at Urbana-Champaign.

New research from David Flaherty, assistant professor of chemical and biomolecular engineering, and graduate student Neil Wilson reveals the mechanism for the direct synthesis of H2O2 on palladium cluster catalysts, and paves the way to design improved catalysts to produce H2O2 to use in place of harmful chlorine, regardless of the scale of the production facility. The research appears as the cover story for the Jan. 20, 2016 issue of the Journal of the American Chemical Society.

The commonly accepted mechanism for direct synthesis of H2O2 essentially states that hydrogen and oxygen atoms bind adjacent to one another on the catalyst surface and then react, Wilson said. To better understand what was going on, he spent over a year building a reactor, fine-tuning experimental procedures, then collecting and analyzing reaction rate data.

"What people thought was happening is after the hydrogen atoms broke apart and they're adsorbed onto the palladium surface, that they just reacted with the oxygen on the surface. But that's not really consistent with what we saw," said Wilson, a fourth-year graduate student in Flaherty's lab and first author of the article, "Mechanism for the Direct Synthesis of H2O2 on Pd Clusters: Heterolytic Reaction Pathways at the Liquid-Solid Interface."

Featured on the journal's cover is an image that depicts their findings: Instead of reacting together on the surface of the catalyst (the palladium cluster), the dissociate into their components—protons and electrons. The protons enter the surrounding solution of water and methanol, while the electrons flow through the palladium itself into oxygen molecules.

"When oxygen comes down onto the surface, it can react with pairs of protons and electrons to form hydrogen peroxide," Wilson said.

"The reason this is critical," Flaherty said, "is because it gives us guidance for how to make the next generation of these materials. This is all motivated by trying to make hydrogen peroxide more cheaply so it can be manufactured more easily, so we can use it in place of chlorine. But we didn't know how to go about making a catalyst that was better than what we have now."

Researchers will now have a better sense of what is happening at the catalyst surface and an appreciation for the role of proton and electron transfer processes in this chemistry. It was not recognized that the oxygen on the surface reacted with liquid phase species, and that the formation of H2O2 by direct synthesis is, therefore, strongly influenced by the solution itself. However, the formation of water (the undesired side reaction) is mostly influenced by properties of the catalyst surface.

"Now that we understand what's happening on the surface, we can start pushing towards rational catalyst design," Wilson said. The research group is now looking into another catalyst, gold-palladium, which has been shown in previous work to be very selective towards H2O2. "People still don't entirely know why gold-palladium is so selective," Wilson added, but it seems that this new mechanistic insight will help to explain the selectivity of these materials.

Several students in Flaherty's lab are currently exploring different ways of "coupling this chemistry directly with reactions that use hydrogen peroxide for green oxidations within very short length scales," that is, micrometers away, Flaherty said. "If we can put these H2O2 formation catalysts very close to something which performs the oxidation reaction, we can avoid the entire problem or concentrating and transporting ."

Explore further: How does an enzyme detoxify the cells of living beings?

More information: Neil M. Wilson et al. Mechanism for the Direct Synthesis of H O on Pd Clusters: Heterolytic Reaction Pathways at the Liquid–Solid Interface , Journal of the American Chemical Society (2016). DOI: 10.1021/jacs.5b10669

Related Stories

Micromotors for energy generation

April 28, 2015

Hydrogen is considered to be the energy source of the future: the first vehicles powered by hydrogen fuel cells are already on the market. However, the problem of hydrogen storage has not been solved in a satisfactory way. ...

Specific oxidation regulates cellular functions

December 18, 2014

For a long time, hydrogen peroxide has been considered as a dangerous metabolite that can damage cells through oxidation. This, however, is not its only role in the cell. Scientists from the German Cancer Research Center ...

Recommended for you

4 comments

Adjust slider to filter visible comments by rank

Display comments: newest first

baudrunner
1 / 5 (1) Jan 21, 2016
That sounds like dangerous research. Pure H2O2 has a tendency to spontaneously combust in air

2 H2O2 → 2 H2O + O2

..strongly exothermic because of the added oxygen this produces. That's why it is such a good rocket fuel, but it isn't used much because it needs handling and that's just dangerous.

Hydrogen Peroxide breaks down cell walls.

promile
Jan 21, 2016
This comment has been removed by a moderator.
promile
Jan 21, 2016
This comment has been removed by a moderator.
baudrunner
1 / 5 (1) Jan 22, 2016
2 H2O2 → 2 H2O + O2 2 H2O + O2 → H2O2
You know, I wish it were possible to get a time lapse video of this reaction. I'll bet it's brilliant ;-).
If we can put these H2O2 formation catalysts very close to something which performs the oxidation reaction, we can avoid the entire problem of [sic] concentrating and transporting hydrogen peroxide
I sure hope that this is not a pipe dream. This is money.

Please sign in to add a comment. Registration is free, and takes less than a minute. Read more

Click here to reset your password.
Sign in to get notified via email when new comments are made.