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Galvanic Cells in Electrochemistry

Learn about galvanic cells, where chemical energy converts to electrical energy through oxidation-reduction reactions transferring electrons. Explore galvanic cell components like voltage meter, salt bridge, and key reactions like Zn to Cu. Discover electrodes, cell potential, and standard reduction potentials. Get examples and detailed half-reactions to grasp the concept fully.

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Galvanic Cells in Electrochemistry

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  1. Chp 17 Electrochemistry

  2. Galvanic Cells • A device in which chemical energy is converted into electrical energy Oxidation – reduction (redox) reactions e- ‘s transfer from reducing agent to oxidizing agent

  3. Galvanic Cell Voltage meter e- e- e- Salt Bridge Why? Zn Cu Zn 2+ SO4 2- Cu 2+ SO42- http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/galvan5.swf

  4. What is happening to the Zn and the Cu? Zn is making electrons (oxidization) Cu is gaining electrons (reduction) Anode where electrons are produced. Cathode where electrons are used. Cell potential cell (volt) or (V) Zn disappearing Forming Cu

  5. Standard Reduction Potentials Anode: Zn(s)  Zn 2+(aq) + 2 e- Cathode: Cu 2+(aq) + 2 e-  Cu (s) ocell = ocat + oan ocell = (+0.76V) + (+0.34V) = +1.10 V Must be positive

  6. Examples Fe 3+(aq) + Cu (s)  Cu 2+(aq) + Fe 2+(aq) Half reactions Red: ( Fe 3+ + 1e -  Fe 2+) Ox: Cu  Cu 2+ + 2e – 2Fe 3+(aq) + Cu (s)  Cu 2+(aq) + 2Fe 2+(aq) ocell = ocat + oan ocell = 0.43 V o = 0.77 V 2 o = - 0.34 V Opposite sign because of Ox = 0.77 V + (-0.34 V)

  7. Line Notation Zn (s) + Cu 2+(aq)  Zn 2+(aq) + Cu (s) Zn(s) l Zn 2+(aq) ll Cu 2+(aq) l Cu(s) electrode electrode

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