A new process could make recycling plastic bags much easier.
Polyethylene plastics—in particular, the ubiquitous plastic bag that blights the landscape—are notoriously hard to recycle.
They’re sturdy and difficult to break down, and if they’re recycled at all, they’re melted into a polymer stew useful mostly for decking and other low-value products.
The new process uses catalysts to break the long polyethylene (PE) polymers into uniform chunks—the three-carbon molecule propylene—that are the feedstocks for making other types of high-value plastic, such as polypropylene.
The process, admittedly in the early stages of development, would turn a waste product—not only plastic bags and packaging, but all types of PE plastic bottles—into a major product in high demand. Previous methods to break the chains of polyethylene required high temperatures and gave mixtures of components in much lower demand. The new process could not only lower the need for fossil fuel production of propylene, often called propene, but also help fill a currently unmet need by the plastics industry for more propylene.
“To the extent they get recycled, a lot of polyethylene plastics get turned into low-grade materials. You can’t take a plastic bag and then make another plastic bag with the same properties out of it,” says John Hartwig, chair in organic chemistry at the University of California, Berkeley. “But if you can take that polymer bag back to its monomers, break it down into small pieces and repolymerize it, then instead of pulling more carbon out of the ground, you use that as your carbon source to make other things—for example, polypropylene. We would use less shale gas for that purpose, or for the other uses of propene, and to fill the so-called propylene gap.”
Polyethylene plastics make up about one-third of the entire plastics market worldwide, with more than 100 million tons produced yearly from fossil fuels, including natural gas obtained by hydraulic fracturing, often called shale gas.
Despite recycling programs—recyclable PE products are designated with plastic numbers 2 and 4—only about 14% of all polyethylene plastic products are recycled. Because of their stability, polyethylene polymers are difficult to break down into their component parts, or depolymerize, so most of the recycling involves melting it and molding it into other products, like yard furniture, or burning it as fuel.
Depolymerizing polyethylene and turning into proplylene is a way of upcycling—that is, producing higher-value products from essentially zero-value waste, while reducing the use of fossil fuels.
Hartwig specializes in using metal catalysts to insert unusual and reactive bonds into hydrocarbon chains, most of which are petroleum based. Novel chemical groups can then be added at these reactive bonds to form new materials. The hydrocarbon polyethylene, which typically occurs as a polymer chain of perhaps 1,000 ethylene molecules—each ethylene is composed of two carbon and four hydrogen atoms—provided his team with a challenge because of its general non-reactivity.
Hartwig and graduate students Steven Hanna and Richard J. “RJ” Conk came up with the idea of breaking two carbon-hydrogen bonds on polyethylene with a catalyst—initially, an iridium catalyst and, later, with platinum-tin and platinum-zinc catalysts—to create a reactive carbon-carbon double bond, which would serve as an Achilles’ heel. With this chink in the armor of the polymer’s carbon-hydrogen bonds, they could then unravel the polymer chain by reaction with ethylene and two additional catalysts that react cooperatively.
“We take a saturated hydrocarbon—all carbon-carbon single bonds—and remove a few molecules of hydrogen from the polymer to make carbon-carbon double bonds, which are more reactive than carbon-carbon single bonds. A few people had looked at that process, but nobody had achieved it on a true polymer,” Hartwig says.
“Once you’ve got that carbon-carbon double bond, then you use a reaction called olefin metathesis, which was the subject of a Nobel Prize in 2005, with ethylene to cleave at the carbon-carbon double bond. Now, you’ve taken this long-chain polymer, and you’ve broken it into smaller pieces that contain a carbon-carbon double bond at the end.”
Addition of a second catalyst, made of palladium, enabled propylene molecules (three-carbon molecules) to be repeatedly clipped off the reactive end. The result: 80% of the polyethylene was reduced to propylene.
“Once we have a long chain with a carbon-carbon double bond at the end, our catalyst takes that carbon-carbon double bond and isomerizes it, one carbon in. Ethylene reacts with that initial isomerized product to make propylene and a nearly identical, just shorter, polymer with a double bond at the end. And then it does the same thing again and again. It walks one step in, cleaves; walks in, cleaves; walks in and cleaves until the whole polymer is cut into three-carbon pieces. From one end of the chain, it just chews down on the chain and spits off propylenes until there is no chain left.”
The reactions were conducted in a liquid solution with soluble, or “homogeneous,” catalysts. The researchers are currently working on a process using non-soluble, or “heterogeneous,” catalysts to achieve the same result, since solid catalysts can be reused more easily.
The group demonstrated that the process works with a variety of PE plastics, including translucent milk bottles, opaque shampoo bottles, PE packaging, and the hard black plastic tops that link aluminum can four-packs. All were efficiently reduced to propylene, with only coloring agents having to be removed.
Hartwig’s lab also recently used innovative catalysis to create a process that turns polyethylene bags into adhesives, another valuable product. Together, these new processes could make a dent in the proliferating piles of plastic that end up in landfills, rivers and, ultimately, the oceans.
“Both are far from commercialization,” he says. “But it is easy to see how this new process would convert the largest amount of plastic waste to a huge chemical feedstock—with much further development, of course.”
The new research appears in the journal Science. Additional coauthors are from UC Berkeley and Berkeley Lab.
A grant from the US Department of Energy to investigate new catalytic reactions funded the work.
Source: UC Berkeley