Chemical Cells and Fuel Cells
Have you ever wondered how batteries work? They're based on redox reactions where one metal loses electrons (oxidation) and another gains them (reduction). When two different metals are placed in a salt solution and connected by a wire, the more reactive metal donates electrons to the less reactive one, creating a flow of electric current.
In a simple cell, the voltage produced depends on the difference in reactivity between the metals. The greater this difference, the higher the voltage. This is why combining reactive magnesium with less reactive copper produces a higher voltage than pairing magnesium with zinc, which is closer to it in reactivity.
Fuel cells represent an exciting application of energy changes, particularly hydrogen fuel cells. Unlike traditional batteries, fuel cells can generate electricity continuously as long as fuel (hydrogen) is supplied. They work by oxidising hydrogen at the negative electrode while oxygen is reduced at the positive electrode, with water as the only waste product.
Think about this: Hydrogen fuel cells could revolutionize transportation with zero harmful emissions, but challenges remain in hydrogen production and storage.
Hydrogen fuel cells offer significant advantages - they don't need electrical recharging, produce no pollutants, and can be sized for different applications. However, they also present challenges: hydrogen is highly flammable, often produced using non-renewable sources, and difficult to store safely. Despite these challenges, fuel cell technology continues to advance as we seek cleaner energy solutions.