What are the basic principles of hydrogen-oxygen fuel cells?

Hydrogen-oxygen fuel cells generate electricity by combining hydrogen and oxygen in a chemical reaction.

Hydrogen-oxygen fuel cells, also known as proton exchange membrane (PEM) fuel cells, operate based on two basic principles: electrochemistry and the conservation of energy. The fuel cell converts the chemical energy stored in hydrogen and oxygen into electrical energy, with water and heat as the only by-products. This process is both efficient and environmentally friendly, as it does not produce any harmful emissions.

The operation of a hydrogen-oxygen fuel cell involves two half-reactions. At the anode (the positive electrode), hydrogen gas is split into protons (H+) and electrons (e-). This process is facilitated by a catalyst, typically platinum. The protons then pass through a proton exchange membrane, which acts as an electrolyte, allowing only protons to pass through while blocking electrons. This forces the electrons to travel through an external circuit, creating an electric current.

Meanwhile, at the cathode (the negative electrode), oxygen gas from the air reacts with the protons and the electrons that have travelled through the external circuit to form water. This reaction also requires a catalyst. The overall reaction in a hydrogen-oxygen fuel cell is the combination of these two half-reactions.

The efficiency of a hydrogen-oxygen fuel cell is determined by the rate at which the reactions occur, which is influenced by factors such as temperature, pressure, and the nature of the catalyst. The fuel cell will continue to produce electricity as long as there is a supply of hydrogen and oxygen. This makes hydrogen-oxygen fuel cells a promising technology for sustainable energy production.