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The Yellow Powder Miracle: How a 1979 Battery Paper Holds the Key to Electric Flight

Heavy nickel and cobalt cathodes limit the flight range of electric aircraft; abundant elemental sulfur offers five times the theoretical energy storage capacity at a fraction of the cost. Ignored for three decades due to rapid polysulfide dissolution, this 1979 paper laid the electrochemical blueprint for lightweight aviation batteries.

Author
R. D. Rauh et al.
Published
1979
Journal
Journal of The Electrochemical Society
Last updated
September 2026
The Yellow Powder Miracle: How a 1979 Battery Paper Holds the Key to Electric Flight

In the quest to build electric regional airplanes and long-haul trucks, battery packs are weighed down by heavy, mined metals like cobalt and nickel. Lithium-ion batteries are simply too heavy to get passenger planes off the ground for long journeys.

In 1979, battery researchers discovered that abundant, lightweight yellow sulfur could store five times more electrical energy than cobalt. The early challenge was that sulfur dissolved into battery fluids like sugar in tea, but this paper laid out the exact chemical ether solvents needed to stabilize sulfur ions.

Awakened by the electric flight race, sulfur electrochemistry is making zero-emission flight a reality. By eliminating reliance on scarce cobalt mines, by slashing battery manufacturing costs by half, and by cutting battery weight by sixty percent, lithium-sulfur chemistry unlocks electric aviation.

Reference

Rauh, R. D., Abraham, K. M., Pearson, G. F., Surprenant, J. K., & Brummer, S. B. (1979). A Lithium/Dissolved Sulfur Battery with an Organic Electrolyte. Journal of the Electrochemical Society, 126(4), 523–527.

Title

A Lithium/Dissolved Sulfur Battery with an Organic Electrolyte

Abstract

Prototype cells of the configuration Li/∼5M S as , THF, have been characterized with regard to capacity, rate, and rechargeability. Virtually 100% of the theoretical capacity could be realized at 50°C at rates below 1.0 mA/cm 2 . In high rate cell configurations, 75% cathode utilization is possible at ∼4 mA/cm 2 (C/3–C/4 rate). The capacities at high rate are enhanced by Lewis acids, although the ultimate cause of rate limitation is passivation of the current collector by discharge products. The self‐discharge rates of Li in contact with 4–5M S (as ) solutions reveal capacity losses of 0.5%/day at 25°C to 4.4%/day at 71°C. Based on the experimental results, a practical energy density of ∼300 W‐hr kg −1 is possible using a standard cell design. Results on the battery's rechargeability are briefly reviewed.

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