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groups are bound to the polymer chain, but cations are freely conducted through the material. This allows the material to conduct hydrogen or other cations between the anode and the cathode. Other types of materials are used as electrolytes in fuel cells for non-automotive applications. For example, phosphoric acid is used an electrolyte in larger stationary fuel cells. Other stationary fuel cells use solid oxides as electrolyte membranes. More on the history of fuel cells Electrochemical cells were invented in the late 1700s. The connection between electricity and chemical reactions provided a fruitful field for researchers of the early 1800s. Scientists like Humphry Davy improved cell designs while using their current to decompose compounds by electrolysis to discover new elements like sodium, potassium, magnesium, calcium, strontium, and barium. Meanwhile, William Nicholson and Anthony Carlisle discovered that water could be decomposed by electrolysis into hydrogen and oxygen. In 1839, Sir William Grove experimented with reversing the process to generate electricity while synthesizing water from hydrogen and oxygen. Even so, it would be another fifty years before the first practical fuel cell was built by Charles Langer and Ludwig Mond in 1889, powered by methane. Francis Bacon worked to develop better fuel cells from the 1930s through the 1950s. Fuel cell development really took off with the birth of the space age, when NASA needed compact and efficient sources of electricity for spacecraft. Connections to Chemistry Concepts 1. Oxidation and reduction—All the reactions that power fuel cells are redox processes, regardless of the fuel involved. 2. Half reactions—Fuel cells are a real-world application in which it makes sense to describe the chemical reaction taking place as two half-reactions. In fuel cells, oxidation and reduction take place in different locations. Half-reactions provide a realistic description of the chemistry. 3. Energy and chemical reactions—The chemical reactions in fuel cells are necessarily exothermic, just as combustion reactions are exothermic. 4. Ions—All fuel cells involve the passage of cations through a membrane while electrons travel separately through a wire to the same destination at the cathode catalyst on the far side of the fuel cell. 5. Atomic structure—The nature of atoms as being made of protons, neutrons, and electrons is central to understanding how ions form and convert to neutral molecules again in fuel cells. 6. Electrochemical cells—To understand fuel cells, students will apply concepts familiar from other electrochemical cells and reinforce those concepts. 7. Polymers—The membrane separating the anode and cathode of a fuel cell is usually made of a polymer electrolyte of some sort. 8. Catalysis—The anode and cathode of a fuel cell not only conduct electrons from one side of the fuel cell to the other, but they also catalyze the oxidation of the fuel molecules and the reduction of the resulting ions to form waste products. 9. Gases and liquids—The fact that there is a lot of empty space between the molecules of a gas becomes important when the economics of transporting hydrogen need to be evaluated. The fact that liquid fuels have much less empty space in between their molecules makes them more economical to transport.PDF Image | BEYOND HYDROGEN
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