Che 466 566 lecture 1
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ChE 466/566 Lecture 1. Fuel Cell and Hydrogen Technology (ChE466/566: 466 for undergraduates and 566 for graduates) (3 Credits, Tu Th 2:35-3:50 pm, JH-203) Department of Chemical Engineering New Mexico State University. Instructors . Dr. Shuguang Deng Jett Hall 253 (Office)

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ChE 466/566 Lecture 1

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Che 466 566 lecture 1

ChE 466/566 Lecture 1

Fuel Cell and Hydrogen Technology

(ChE466/566: 466 for undergraduates and 566 for graduates)

(3 Credits, Tu Th 2:35-3:50 pm, JH-203)

Department of Chemical Engineering

New Mexico State University



Dr. Shuguang Deng

Jett Hall 253 (Office)

Tel: 575-646-4346

e-mail: [email protected]

Course description

Course Description

This course presents an introduction to the fundamentals and applications of fuel cell and hydrogen technology. It includes thermodynamics, electrochemical kinetics, fuel cell electrode catalysts, fuel cell systems, fuel reforming and H2 production, hydrogen storage, hydrogen safety. The applications of fuel cells in power generation, portable power, and automotives will also be covered. Students will also have a chance to work on a term project, write a term paper and present the term project.



  • Ryan P. O’Hayre, Suk-Won Cha, Whitney Colella and Fritz B. Prinz “Fuel Cell Fundamentals”, John Wiley & Sons, Inc, ISBN: 13 978-0-471-741-48-0 (2006).

  • “Fuel Cell Handbook”, 7th Edition, DOE/NETL-2004/1206, EG&G Technical Services, Inc. Science Applications International Corporation (Nov., 2004).



There will be two exams and one term paper and presentation. The guidelines for term paper and presentation will be provided.




Term Paper20%


A:85-100; B:75-84; C:65-74; D:60-64; F:<60

Course webpage

Course Webpage

Login Name: che466

Login Password:pemfc

Course sch edule

Course Schedule

30 Sessions

26 Lectures

2 Exams

2 Final presentations

Fuel cell basics

Fuel Cell Basics

Battery vs. fuel cells

What is fuel cell?

Why do we need fuel cell?

How does it work?

Where do we use it?



A device that converts chemical energy stored in a battery directly to electrical energy. It is a closed system.

Che 466 566 lecture 1

Volta’s Battery (1800)

Alessandro Volta 1745 - 1827

Paper moisturized with NaCl solution



Che 466 566 lecture 1

Zinc – Copper Battery

A simple fuel cell expt

A Simple Fuel Cell Expt.

  • Apparatus

  • One small glass with water and a common salt

  • One voltmeter with ranges of 0-2 and 0-20 VDC

  • One 4.5 volt battery

  • Experimental cables with small crocodile clips

  • 2 platinum wires as electrodes

Fuel cell expt

Fuel Cell Expt.

Fuel cell expt1

Fuel Cell Expt.

Fuel cell expt2

Fuel Cell Expt.

H2O  H2 + ½ O2

Fuel cell expt3

Fuel Cell Expt.

H2 + ½ O2 H2O

Electric power conversion

Electrolysis / Power consumption

Chemical Reactions

Electric Power

Electrochemical battery / Power generation

Electric Power Conversion

Fuel cell

Fuel Cell

A device that converts the chemical energy stored in a fuel directly to electrical energy. It is an open system.

Fuel cell history

Fuel Cell History

Design and technology

Design and Technology

Replacement technology

- Replaces an existing product

electric vs. gas light

- New product must cost less

Enabling technology

- Provides new capability

airplanes ––> flight

- Cost not so important

Conventional power generation

Conventional Power Generation

Fuel cell advantages

Fuel Cell Advantages

Fuel cells are needed because fuel cells possess:

1). the advantageous characteristics of high-energy conversion efficiency

2). environmental benign operation

3). alleviate and eliminate dependence on fossil-fuel reserves

4). flexible for a variety of different applications

5). compatible with renewable energy sources

6). carriers for energy security, economic growth, and sustainable development.

Fuel cell disadvantages

Fuel Cell Disadvantages

  • Too expensive for many applications

  • Power density limitation

  • Fuel availability and storage

  • Operation temperature compatibility concerns

  • Susceptibility to environmental poisons

  • Durability under start-stop cycling

Pem fuel cell basics

PEM Fuel Cell Basics

Pem fuel cell basics1

PEM Fuel Cell Basics

H2 + ½ O2  Energy + H2O + Waste Heat

Pem fuel cell basics2

PEM Fuel Cell Basics

Pem fuel cell basics3

PEM Fuel Cell Basics

  • Reactants (such as H2 or O2) transferred to the porous electrode surface, and the gas/electrolyte interface.

  • 2. The reactant dissolves into the liquid electrolyte at the two-phase interface.

  • 3. The dissolved reactant then diffuses through the liquid electrolyte to arrive at the electrode surface.

  • 4. Some pre-electrochemical homogeneous or heterogeneous chemical reactions may occur, such as electrode corrosion reaction, or impurities in the reactant stream may react with the electrolyte.

  • 5. Electroactive species (which could be reactant themselves as well as impurities in the reactant stream) are adsorbed onto the solid electrode surface.

Pem fuel cell basics4

PEM Fuel Cell Basics

6. Adsorbed species may migrate on the solid electrode surface, principally by the mechanism of diffusion.

7. Electrochemical reactions then occur on the electrode surface wetted by the electrolyte the so-called three phase boundary, giving rise to electrically charged species (or ions and electrons).

8. Electrically charged species and other neutral reaction products such as water, still adsorbed on the electrode surface, may migrate along the surface due to diffusion in what has been referred to as post-electrochemical surface migration.

9. The adsorbed reaction products become desorbed.

Pem fuel cell basics5

PEM Fuel Cell Basics

10. Some post-electrochemical homogeneous or heterogeneous chemical reactions may occur.

11. Electrochemical reaction products (neutral species, ions and electrons) are transported away from the electrode surface, mainly by diffusion but also for the ions, influenced by the electric field set up between the anode and cathode. The electron motion is dominated by the electric field effect.

12. Neutral reaction products diffuse through the electrolyte to reach the reactant gas/electrolyte interface.

13. Finally, the products will be transported out of the electrode and the cell in gas form.

Electrodes and electrolyte

Electrodes and Electrolyte

  • Functions of Electrodes

  • Provide a place for the electrochemical reaction to occur easily (reaction sites)

  • Provide a flow path for reactant supply to, and product removal from, the reaction sites

  • Collect the electrons and provide a flow path for electron transfer

  • Functions of Electrolyte

  • An ion conductor

  • An electron insulator

  • A barrier to separate the reactants (H2 and O2 in PEMFC)

Fuel cell perfromance

Fuel Cell Perfromance

Fuel cell applications

Fuel Cell Applications

  • Automotive applications (~100 kW)

  • Portable power applications (<200 W)

  • Residential applications (1-5 kW)

  • Onsite cogeneration power plants (0.2 – 1 MW)

  • Distributed electric power generation (2-20 MW)

  • Baseload electric power generation (100-300 MW)

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