Introduction :
A Fuel Cell is a device that converts the energy of the chemical reaction between a fuel and an oxidant into electricity and heat. It is easy to make a fuel cell working, by using an anode, cathode, catalysts and most often an electrolyte. Fuels and oxidants are also necessary to make a fuel cell. Fuel cells are combined into groups to obtain a usable voltage and power output, called stacks. Fuel cells generate electricity electrochemically, rather than mechanically, so they are more efficient over a wider load factor and can cut greenhouse gases by over 50 percent. Fuel cells are very much different from batteries. Fuel cells consume reactant from an external source, which must be replenished. Fuel cells produce electricity with an efficiency of about 70 % compared to thermal plants whose efficiency is about 40%.
To make a fuel cell, we would need:
One of the most successful fuel cells uses the reaction of hydrogen as fuel and oxygen as oxidant to form water (Hydrogen oxygen fuel cell). The cell was used for providing electrical power in the Apollo space programme. The water vapors produced during the reaction were condensed and added to the drinking water supply for the astronauts. In the cell, hydrogen and oxygen are bubbled through porous carbon electrodes into concentrated aqueous solutions of sodium hydroxide. Catalysts like finely divided platinum or palladium metal are incorporated into the electrodes for increasing the rate of electrode reactions.
Catalysis plays a very important role in Hydrogen oxygen fuel cells, separating the electrons and protons of the reactant fuel (at the anode), and forcing the electrons to travel though a circuit, generating electrical power. At the cathode, another catalytic process takes the electrons back, combining them with the protons, which have traveled across the electrolyte and the oxidant to form waste products like carbon dioxide and water.
The electrode reactions of Hydrogen oxygen fuel cell are given below:
Cathode reaction: O2 (g) + 2H2O (l) + 4e+
4OH–(aq)
Anode reactions: 2H2 (g) + 4OH–(aq)
4H2O (l) + 4e–
Overall reactions: 2H2 (g) + O2 (g)2 H2O (l)
The cell can run continuously as long as the reactants are supplied.
A Fuel Cell is a device that converts the energy of the chemical reaction between a fuel and an oxidant into electricity and heat. It is easy to make a fuel cell working, by using an anode, cathode, catalysts and most often an electrolyte. Fuels and oxidants are also necessary to make a fuel cell. Fuel cells are combined into groups to obtain a usable voltage and power output, called stacks. Fuel cells generate electricity electrochemically, rather than mechanically, so they are more efficient over a wider load factor and can cut greenhouse gases by over 50 percent. Fuel cells are very much different from batteries. Fuel cells consume reactant from an external source, which must be replenished. Fuel cells produce electricity with an efficiency of about 70 % compared to thermal plants whose efficiency is about 40%.
How to make a fuel cell
We can make a fuel cell (Hydrogen Fuel Cell) in our kitchen in just 10 minutes, and demonstrate how hydrogen and oxygen combines to give clean electricity.To make a fuel cell, we would need:
- One foot of platinum coated nickel wire along with small piece of wood or Popsicle stick.
- A 9 volt battery clip and a 9 Volt battery.
- A little transparent sticky tape.
- One glass full of water.
- Volt meter device.
Hydrogen-oxygen Fuel cell
One of the most successful fuel cells uses the reaction of hydrogen as fuel and oxygen as oxidant to form water (Hydrogen oxygen fuel cell). The cell was used for providing electrical power in the Apollo space programme. The water vapors produced during the reaction were condensed and added to the drinking water supply for the astronauts. In the cell, hydrogen and oxygen are bubbled through porous carbon electrodes into concentrated aqueous solutions of sodium hydroxide. Catalysts like finely divided platinum or palladium metal are incorporated into the electrodes for increasing the rate of electrode reactions.
Catalysis plays a very important role in Hydrogen oxygen fuel cells, separating the electrons and protons of the reactant fuel (at the anode), and forcing the electrons to travel though a circuit, generating electrical power. At the cathode, another catalytic process takes the electrons back, combining them with the protons, which have traveled across the electrolyte and the oxidant to form waste products like carbon dioxide and water.
The electrode reactions of Hydrogen oxygen fuel cell are given below:
Cathode reaction: O2 (g) + 2H2O (l) + 4e+
4OH–(aq)Anode reactions: 2H2 (g) + 4OH–(aq)
4H2O (l) + 4e–Overall reactions: 2H2 (g) + O2 (g)
2 H2O (l)The cell can run continuously as long as the reactants are supplied.
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