1 Electrodes and Electrochemical Cells “Batteries”

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Presentation transcript:

1 Electrodes and Electrochemical Cells “Batteries”

2 Electric power conversion in electrochemistry Chemical Reactions Electric Power Electrolysis / Power consumption Electrochemical battery / Power generation

Types of the electrochemical system for electric power generation Primary batteries POWER Fuel cells Reaction products (exhaust) Reductant (fuel) Oxidant POWER Secondary batteries Recharge POWER

4 Types of Electrode (Summery)

5 Types of Electrode (continued)

6 Simple Type: Anode| electrolyte | Cathode Complex Type: A | Anolyte || Catholyte|C Cell Conventions

7 Cells Connections

Me 1 n+ SO 4 2- Me 2 n+ SO 4 2- Me 2 Me ne - = Me 2 n+ ANODE Me 2 n+ - ne - = Me 2 0 CATHODE Salt Bridge Me 1 Principles of power generation in the electrochemical systems

Me 1 n+ SO 4 2- Me 2 n+ SO 4 2- Me 2 Me ne - = Me 2 n+ ANODE Me 2 n+ - ne - = Me 2 0 CATHODE Me 1 Diaphragm Membrane or Principles of power generation in the electrochemical systems

Pt|H 2 (g)| HCl | AgCl(s),Ag(s). H 2  2H + +2e AgCl+e  Ag+Cl- Simple Cell

11 Zn --> Zn e- Cu e- --> Cu <--AnionsCations--> OxidationAnodeOxidationAnode Reduction Cathode Reduction Cathode RED CAT Zn|Zn 2+ ||Cu 2+ |Cu Complex Cell

Pt | Fe 2+,Fe 3+ | | Ag + | Ag

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 13

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 14 Zn|ZnSO 4 ||HCL|H 2,Pt Zn  Zn 2+ +2e H++2e  H2

15 Dry Cell Battery ZnCl 2 Anode Zn ---> Zn e- Cathode 2 NH e- -  2 NH 3 + H 2

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