How Fuel cells work
An electrochemical reaction occurs between hydrogen and oxygen that converts chemical energy into electrical energy.
Which fuel is used in the fuel cell?
Think of them as big batteries, but ones that only operate when fuel—in this case, pure hydrogen—is supplied to them. When it is, an electrochemical reaction takes place between the hydrogen and oxygen that directly converts chemical energy into electrical energy. Various types of fuel cells exist, but the one automakers are primarily focusing on for fuel cell cars is one that relies on a proton-exchange membrane, or PEM.
PEM Fuel Cell Automotive
In the generic PEM fuel cell pictured here, the membrane lies sandwiched between a positively charged electrode (the cathode) and a negatively charged electrode (the anode). In the simple reaction that occurs here rests the hope of engineers, policymakers, and ordinary citizens that someday we’ll drive entirely pollution-free cars.
Types of fuel cell
Before we look at how fuel cells works, let’s look at the different types of fuel cells that are available.
- Polymer Electrolyte Membrane (PEM) fuel cell
- Direct Methanol Fuel cells
- Alkaline fuel cells
- Phosphoric acid fuel cells
- Molten carbonate fuel cells
- Solid oxide fuel cells
- Combined heat and power fuel cells
- Regenerative or Reversible fuel cells
Here’s what happens in the fuel cell and how fuel cells works
When hydrogen gas pumped from the fuel tanks arrives at the anode, which is made of platinum, the platinum catalyzes a reaction that ionizes the gas. Ionization breaks the hydrogen atom down into its positive ions (hydrogen protons) and negative ions (electrons). Both types of ions are naturally drawn to the cathode situated on the other side of the membrane, but only the protons can pass through the membrane (hence the name “proton-exchange”). The electrons are forced to go around the PEM, and along the way they are shunted through a circuit, generating the electricity that runs the car’s systems.
Cathode Reaction: O2 + 2H2O + 4e– → 4OH–
Anode Reaction: 2H2 + 4OH– → 4H2O + 4e–
Net Cell Reaction: 2H2 + O2 → 2H2O
Using the two different routes, the hydrogen protons and the electrons quickly reach the cathode. While hydrogen is fed to the anode, oxygen is fed to the cathode, where a catalyst creates oxygen ions. The arriving hydrogen protons and electrons bond with these oxygen ions, creating the two “waste products” of the reaction—water vapor and heat. Some of the water vapor gets recycled for use in humidification, and the rest drips out of the tailpipe as “exhaust.” This cycle proceeds continuously as long as the car is powered up and in motion; when it’s idling, output from the fuel cell is shut off to conserve fuel, and the ultra capacitor takes over to power air conditioning and other components.
How does fuel cell differ from Battery?
A single hydrogen fuel cell delivers a low voltage, so manufacturers “stack” fuel cells together in a series, as in a dry-cell battery. The more layers, the higher the voltage. Electrical current, meanwhile, has to do with surface area. The greater the surface area of the electrodes, the greater the current. One of the great challenges automakers face is how to increase electrical output (voltage times current) to the point where consumers get the power and distance they’re accustomed to while also economizing space in the tight confines of an automobile.
Fuel cell applications
Fuel cell technology can be used in a variety of ways. Currently, extensive testing is being carried out in order to develop a cost-effective fuel cell-powered vehicle. The below are a few examples of how this technology can be used.
- Fuel cell electric vehicles use clean fuels and are are more environmentally sustainable than vehicles powered by internal combustion engines.
- Many space expeditions, including the Apollo space programme, have relied on them for fuel.
- Heat and water are the most common by-products of these cells.
- Any fuel cells’ portability is highly useful in military applications.
- Several electronic devices may be powered by these electrochemical cells.
- In certain rural locations, fuel cells are used as a primary or secondary source of energy.