This document discusses hydrogen fuel cells, including their history, types, and connections to electrochemistry and thermodynamics. It describes how hydrogen fuel cells work through redox reactions, with hydrogen oxidizing at the anode to produce protons and electrons, and oxygen being reduced at the cathode by protons and electrons to produce water. Two main types are alkaline fuel cells, which use an alkaline electrolyte, and proton exchange membrane (PEM) fuel cells, which are more efficient and used in vehicles. Fuel cells can be more efficient than combustion engines and produce only water, making them more environmentally friendly than gasoline-powered vehicles. They may be powered by hydrogen produced through electrolysis using renewable energy.
4. Historical Overview
• 1838: discovered by German scientist
Christian Friedrich Schöenbein
• 1839: Demonstrated by Welsh scientist Sir
William Robert Grove
5. What are Fuel Cells?
• Battery that produces electricity
• overall reaction: oxidation of a fuel by oxygen
• 2H2(g) + O2(g) 2H2O(l)
(Hydrogen) Fuel + oxygen water
• Unlimited fuel supply:
reactants continuously
supplied from an external
source (open system)
• Also known as flow battery
• Used as a stack
6. Types of Fuel Cells
• Molten carbonate cells
• Solid oxide cells
• Direct methanol and other non-hydrogen
cells
• Biofuel cells
• Phosphoric Acid
• Proton Exchange Membrane
• Acid and alkaline cells
7. How Do Fuel Cells Work?
HYDROGEN FUEL CELLS
& ELECTROCHEMISTRY
9. Connection 2: FUEL CELLS
& CATALYSTS (rate of reaction)
• the splitting of H2 into p+ and e- at the anode is typically
speeded up by the presence of a catalyst (typically metal
placed on the anode, or the electrode itself)
• Platinum film is often used
10. • Electrolyte – permit only appropriate ions to pass
between anode and cathode; otherwise the chemical
reaction may be disrupted
• End product: water = drained
14. How Hydrogen Fuel Cells Work – PEM
• Proton exchange membrane cells
• A fuel cell produced electricity by combining Hydrogen
and Oxygen atoms electrochemically rather than through
combustion
• Hydrogen = fuel electrolysis – stored as a compressed
gas/liquid/metal compound
• A single fuel cell consists of an anode and a cathode with
an electrolyte in between
• Hydrogen molecules enter the anode react with
catalysts (1) split into H+ & e- H+ pass through
electrolyte, e- directed through an external circuit =
electrical current
• Oxygen molecules enter at the cathode + H+
+ e-
water & heat
• Individual fuel cells placed in a series = fuel cell stack
power vehicle
15.
16.
17. HYDROGEN FUEL CELLS
& REDOX REACTION
Alkaline Fuel Cells
@ Anode, H2 is oxidized:
H2 + 2OH-
2H2O + 2e-
H2 2H+
+ 2e-
Electrons flow through an external circuit and return to the cathode, reducing
oxygen:
O2 + 2H2O + 4e-
4OH-
4H+
+ 4e-
+ O2 2H2O
PEM Fuel Cells
19. Connection 4: HYDROGEN FUEL CELLS
& EFFICIENCY and
THERMODYNAMICS
• Automobile internal combustion engines
• inefficient – 25%
• Rechargeable batteries (modified lead-acid, nickel-
cadmium batteries)
• Run down quickly – 250 Km
• Recharged from external electrical source
• Takes hours
• Fuel cells
• Efficient – 80%
20. Connection 4: HYDROGEN FUEL CELLS
& EFFICIENCY and
THERMODYNAMICS
• Fuel cells create electricity chemically; ,
unlike combustion
are not subject to thermodynamic laws
• ∴ fuel cells are more efficient
• Some waste heat can also be harnessed
21. Connection 5: HYDROGEN FUEL CELLS
& THE ENVIRONMENT
• Automobile engines: gasoline = pollutants
• CO2, Nox, VOCs
• health & environmental problems: smog, greenhouse
effect
• Electric cars: hydrogen fuel cells = pollution free
• Cleaner, quieter, more efficient
• Product: water vapour
22. Connection 5: HYDROGEN FUEL CELLS
& THE ENVIRONMENT
• Production of hydrogen fuel – unnatural resource
• Hydrocarbon fuels (petroleum, methane) = pollution
• Electrolysis of water powered by solar energy or
hydroelectricity = low pollution
• Renewable energy source
24. Connection 6: HYDROGEN FUEL CELLS
AS AN ENERGY SOURCE
• Production of hydrogen fuel – unnatural resource
• Hydrocarbon fuels (petroleum, methane) = pollution
• Electrolysis of water powered by solar energy or
hydroelectricity = low pollution
26. References
• (Sørensen), B. S. (2005).Hydrogen and Fuel Cells: Emerging
Technologies and Applications (Sustainable World). Toronto:
Academic Press.
• Harkin, T., & Hoffmann, P. (2001). Tomorrow's Energy:
Hydrogen, Fuel Cells, and the Prospects for a Cleaner Planet.
London: The Mit Press.
• Holland, G., & Provenzano, J. (2007). Hydrogen Age, The.
Layton: Gibbs Smith, Publisher.
• ollecting the History of Proton Exchange Membrane Fuel
Cells. (n.d.). National Museum of American History. Retrieved
April 20, 2010, from
http://americanhistory.si.edu/fuelcells/basics.htm