Fuel Cells

Chemistry 12 --- Electrochemistry

1. What is a fuel cell?

• Electrochemical cell• Chemical energy

Electrical energy• Hydrogen is the most common fuel

2. How does it work?

• The anode reaction: 2H2(g) + 4OH-(aq) 4H2O(l) + 4e-

• The cathode reaction: O2(g) +2H2O (l) + 4e- 4OH- (aq)

• The overall reation: 2H2(g) + O2(g) 2H2O(l)

• Individual fuel cells

very small amountsof electricity• Placed in series • Electricity, water,heat and, and other emissions (NO2)…

3. Why Fuel Cells?

• Pollution free• Operates silently• High efficiency 70%-80% vs 35%• Never goes dead

4. Why not Fuel Cells?

• Corrode quickly• Constant maintenance• Cells expensive• Quite large

5. Applications

• Automobiles

• Bus

• Boats

• Submarines

• Space Capsule

6. References

•Students Workbook

•http://en.wikipedia.org/wiki/Fuel_cell

•http://auto.howstuffworks.com/fuel-efficiency/alternative-fuels/fuel-cell.htm