seminae

1. Introduction to Hydrogen Fuel Cell Vehicles
Hydrogen fuel cell vehicles are powered by
an electric motor using energy from
hydrogen fuel stored in onboard tanks. The
only byproduct is water vapor, making
them environmentally friendly.

2. What is a hydrogen fuel cell?
•Hydrogen fuel cells (HFCs) are a type of
electrochemical cell.
•HFCs generate electricity by reduction and
oxidation reactions within the cell.
•They use three main components, a fuel, an oxidant
and an electrolyte.
•HFCs operate like batteries, although they require
external fuel.
•HFCs are a thermodynamically open system.
•HFCs use hydrogen as a fuel, oxygen as an oxidant,
a proton exchange membrane as an electrolyte, and
emit only water as waste.

3. Advantages of Hydrogen Fuel Cell Vehicles
Zero Emissions
They produce zero tailpipe
emissions, fostering a
greener environment and
contributing to cleaner air
quality.
Refueling takes minutes, similar
to the time it takes to refuel a
conventional gasoline vehicle.
Quick Refueling
They offer a longer driving range
compared to battery-electric
vehicles, making them suitable
for long-distance travel.
Long Driving Range

4. How do they work?
• Fuel (H2) is first transported to the
anode of the cell
• Fuel undergoes the anode reaction
• Anode reaction splits the fuel into H+
(a proton) and e-
• Protons pass through the electrolyte to
the cathode
• Electrons can not pass through the
electrolyte, and must travel through an
external circuit which creates a usable
electric current
• Protons and electrons reach the
cathode, and undergo the cathode
reaction

5. Chemistry behind the technology
Oxidation
At the anode of the cell, a
catalyst (platinum powder) is
used to separate the proton from
the electron in the hydrogen
fuel.
Anode half-reaction:
2H2  4H+ + 4e-
Eo = 0.00V
Reduction
At the cathode of the cell, a
second catalyst (nickel) is used to
recombine the protons, electrons,
and oxygen atoms to form water.
Cathode half- reaction:
4H+ + O2 + 4e-  2H2O
Eo = 0.68V
In electrochemistry, the Eo
cell value (energy) of a fuel cell is equal to the Eo of the cathode half-
reaction minus the Eo of the anode half-reaction. For a hydrogen fuel cell, the two half reactions
are shown above. So to calculate the energy of one fuel cell, we need to subtract the anode
energy from the cathode energy. For a HFC, the Eo
cell = 0.68V – 0.00V which equals 0.68V

6. Uses of hydrogen fuel cells
There are many different uses of fuel cells being utilized right now. Some of these uses are…
•Power sources for vehicles such as cars, trucks, buses and even boats and submarines
•Power sources for spacecraft, remote weather stations and military technology
•Batteries for electronics such as laptops and smart phones
•Sources for uninterruptable power supplies.

7. Problems regarding hydrogen fuel cells
• Lack of hydrogen infrastructure
• Need for refueling stations
• Lack of consumer distribution system
• Cost of hydrogen fuel cells
• 2009 Department of Energy estimated $61/kw
• Honda FCX Clarity costs about half a million dollars to make
• Carbon cost of producing hydrogen
• Problems with HFC cars
• Short range (~260 miles)
• Warm up time (~5 minutes)

8. Future Outlook for Hydrogen Fuel
Cell Vehicles
• Technological Advancements
Continuous improvements in fuel cell efficiency and
cost reduction are expected.
• Expansion of Infrastructure
Anticipated increase in hydrogen refueling stations
and production facilities globally.

9. Conclusion
• Energy Security
Hydrogen fuel cell vehicles diversify energy sources and reduce dependence on
traditional fossil fuels.
• Sustainable Transportation
They offer sustainable transportation solutions, aligning with global efforts to
minimize environmental impact.
• Industry Collaboration
Partnerships among automotive companies and energy providers drive the
development of hydrogen infrastructure.

10. Thanks