Making hydrogen peroxide where you need it, from oxygen and water, without a factory

Published in ENGINEERING Energy, 2026. Beijing University of Chemical Technology.

Hydrogen peroxide is everywhere in modern industry. It disinfects water, sterilizes medical equipment, bleaches paper and textiles, and serves as an oxidizer in chemical synthesis. It ranks among the world's 100 most important industrial chemicals. Yet the way we produce it has barely changed in decades: the anthraquinone process, a multi-step industrial method that requires large centralized plants, high energy inputs, and the storage and transport of concentrated solutions that can be hazardous.

There is a simpler reaction that could replace it. The two-electron oxygen reduction reaction (2e- ORR) generates hydrogen peroxide directly from oxygen and water under mild conditions, using electricity as the energy input. The catch has always been the catalyst: the reaction needs materials that selectively produce H2O2 rather than allowing oxygen to fully reduce to water through the competing four-electron pathway.

A comprehensive review published in ENGINEERING Energy by researchers at the Beijing University of Chemical Technology now maps the state of the art across three catalyst classes and assesses how close the field is to making on-site H2O2 production a practical reality.

Three routes to the same product

Noble metal alloys like platinum-mercury and gold-palladium have demonstrated near-perfect selectivity for H2O2 production. They work by tuning the adsorption energy of the key reaction intermediate, *OOH, through synergistic effects between the two metals. The selectivity is impressive, but the cost of noble metals limits scalability.

Carbon-based nanomaterials offer a cheaper alternative. By doping carbon structures with heteroatoms such as nitrogen, boron, or phosphorus, or engineering specific surface defects, researchers have created catalysts that promote "end-on" oxygen adsorption. In this configuration, only one end of the oxygen molecule binds to the catalyst surface, preserving the O-O bond that needs to remain intact for H2O2 formation rather than water. These materials have shown remarkable efficiency in laboratory settings.

Transition metal compounds, including single-atom catalysts and transition metal chalcogenides, represent the newest frontier. These use earth-abundant elements rather than precious metals. Notable among recent results are zirconium nitride-based catalysts that can produce H2O2 directly from ambient air with long-term stability, a finding that brings the concept of decentralized production closer to reality.

From laboratory to wastewater plant

The review describes how some of these catalysts are already being tested in "heterogeneous Fenton" systems for wastewater treatment. In these systems, electrochemically generated H2O2 reacts with iron catalysts to produce highly reactive hydroxyl radicals that break down organic pollutants that conventional treatment cannot handle. Producing the H2O2 on-site eliminates the need for delivery trucks carrying concentrated peroxide solutions to treatment plants.

"The core challenge lies in designing catalysts that are not only active but also highly selective," said Professor Yongjun Feng, one of the study's corresponding authors. "We must prevent the oxygen from over-reducing into water and instead stabilize the key intermediate, *OOH, to ensure the production of hydrogen peroxide."

What stands in the way

The primary unsolved problem is durability. Non-noble metal catalysts, which are the most economically viable for large-scale deployment, tend to degrade in the acidic conditions that many applications require. How quickly performance drops off and whether catalysts can be regenerated economically are questions that laboratory demonstrations have not yet fully answered.

The review also does not address the full system-level economics of on-site electrochemical production versus the established anthraquinone process, which benefits from decades of optimization and enormous economies of scale. A catalyst that works brilliantly at the milligram scale in a research lab may face entirely different challenges when integrated into a continuous-flow reactor at industrial throughput.

Still, the direction of the field is clear. If electrocatalysts can be made selective, durable, and cheap enough, the centralized production-and-transport model for hydrogen peroxide becomes unnecessary for many applications. Generate it where you use it, from oxygen and water, powered by renewable electricity. The chemistry is already there. The engineering is catching up.