Scientists at Stanford University in California have demonstrated a new water electrolysis device that can produce hydrogen from salt water. While using electricity to split water to produce hydrogen is a mature technology with commercial applications beginning to emerge in a variety of markets, most electrolysers require purified water to operate, and system components degrade rapidly in the presence of salts. If the technology is scaled up to represent a significant part of our energy mix, this could put heavy pressure on water resources. According to researchers at Stanford University, the amount of hydrogen needed to fuel cars and power city scenarios cannot be produced with pure water, but if all water from seawater was available, the problem could be solved. "Seawater is the most abundant aqueous electrolyte raw material on Earth," reads the abstract of the research paper. "But its implementation in the water splitting process poses many challenges, especially for the anodic reaction." Key to the system demonstrated at Stanford is a new anode that protects against salt corrosion through a negatively charged layer. The researchers explain that the anode consists of a nickel foam core that delivers electricity from the source, nickel iron hydride on top of the nickel hydroxide layer initiates the electrolysis process, and nickel sulfide creates a negative charge during the electrolysis process. During the process, the core material is protected from the chlorides in the salt water. The researchers explain this concept as similar to the idea that the negative ends of two magnets repel each other. An experiment conducted by Kee, described in a paper that sustainably splits seawater into hydrogen and oxygen fuels at high altitudes, was published in the Journal Proceedings of the National Academy of Sciences of the United States of America, using a solar-powered demonstration powered by water collected from San Francisco Bay. Machine to produce hydrogen and oxygen from sea water. The electrolytic cell worked continuously for more than 1,000 hours at a current density of 400mA/cm2 and a voltage of 2.12, with no obvious decay. The researchers noted that without the coating, the anode would typically fall apart after less than 12 hours of operation...the entire electrode would crumble into pieces, but with this layer, it could last for more than a thousand hours," Michael Ken "What's impressive about this study is that we were able to operate with the same currents used in industry today. Professor Hongjie Dai, a professor of chemistry at Expansion Stanford, noted that his lab has proven the concept of the technology with this demonstration, but scale and mass production will be left to industrial companies. However, he went on to point out that anodes incorporating protective layers could be incorporated into existing of electrolysers, greatly simplifying the adoption of the technology. “It’s not like starting from scratch,” Day explains. “It’s more like starting from 80 or 90 percent. "

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