A fuel cell converts chemical energy directly into electricity through electrochemical reactions between hydrogen and oxygen. The voltage generated by a single fuel cell is typically less than 1 volt, so multiple cells are connected in series to produce a useful voltage. There are different types of fuel cells that use various electrolytes, including alkaline, solid oxide, phosphoric acid, proton exchange membrane, molten carbonate, and direct methanol fuel cells.

2. A fuel cell is a
device that
converts chemical
energy into
electrical energy,
water, and heat
through
electrochemical
reactions.
The voltage generated by a single cell is typically rather small (< 1 volt), so
many cells are connected in series to create a useful voltage.
What is a Fuel Cell?

3.  our society is dependent upon fossil fuels such as coal, oil
and gas
 fossil fuels are a non-renewable energy resource
 fuel prices are rising and resources dwindling
 food, transport and electricity costs are affected by fuel
prices
 the atmosphere is becoming more and more polluted
 carbon dioxide contributes to climate change and the
greenhouse effect
Why to use fuel cell ?

4. Parts of fuel cells

5. REACTIONS
 Anode Reaction:
2H2 + 2O2− → 2H2O + 4e−
 Cathode Reaction:
O2 + 4e− → 2O2−
 Overall Cell Reaction:
2H2 + O2 → 2H2O

6. Working of Fuel Cell

7. There are different types of fuel cells, differentiated
by the type of electrolyte separating the hydrogen
from the oxygen.
The types of fuel cells are:
 Alkaline fuel cells (AFC)
 Solid oxide fuel cells (SOFC)
 Phosphoric Acid Fuel Cell (PAFC)
 Proton Exchange Membrane Fuel Cells (PEMFC)
 Molten Carbonate fuel cells (MFFC)
 Direct methanol fuel cells (DMFC)
Types of fuel cells

8. Alkaline fuel cells
 Operates on compressed hydrogen
and oxygen.
Efficiency is about 70 %, and
operating temperature is 50 to 100°C.
Used in Apollo spacecraft to provide
both electricity and drinking water.
They require pure hydrogen fuel,
however, and have platinum electrode
catalysts.

9. Solid oxide fuel cells
Uses a hard, ceramic compound of
metal oxides as electrolyte
Efficiency is about 60%
Operating temperatures are about
1,000 ° C, so no reformer is required
for extracting hydrogen from fuel
Utility applications

10. Phosphoric acid fuel cell
 Uses phosphoric acid as the
electrolyte
 Efficiency ranges from
40 to 80 %
Typically used for stationary
power generation

11. Proton exchange membrane fuel cells
Work with a polymer
electrolyte in the form of a thin,
permeable sheet
Efficiency is about 40 to 50 %
Suitable for homes and cars

12. Molten carbonate fuel cell
Uses high-temperature compounds
of salt carbonates as electrolyte
Efficiency ranges from 60 to 80
percent, and operating
temperature is about 650 degrees C
Developed for natural gas and
coal-based power plants to
generate power for industry and
military use

13. Direct Methanol Fuel Cells
 Use to power cellular phones and laptops
 Use a polymer membrane as the electrolyte
 The anode catalyst itself draws the hydrogen
from the liquid methanol (no reformer needed)
 Efficiency of about 40%
 typically operate at a temperature between 120-
190 degrees F
 Higher efficiencies are achieved at higher
temperatures

14. BENEFITS OF FUEL CELL TECHNOLOGY
 Physical Security
 Reliability
 Efficiency
 Environmental Benefits (Non- Polluted) =
Less Green House Gases Emissions
 Battery Replacements / Alternatives
 Refueled in 5 minutes
 40% higher fuel economy than diesel vehicles

15. Applications
Stationary
Transportation
Consumer Electronics
Providing power for base
stations or cell sites
Food preservation
Small heating appliances
Notebook computers
Hybrid vehicles

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