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Voltaic Cells

Voltaic Cells. Produce electrical current using a spontaneous redox reaction Used to make batteries !

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Voltaic Cells

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  1. Voltaic Cells • Produce electrical current using a spontaneousredox reaction • Used to make batteries! • Materials needed: two beakers, piece of the oxidized metal (anode, - electrode), solution of the oxidized metal, piece of the reduced metal (cathode, + electrode), solution of the reduced metal, porous material (salt bridge), solution of a salt that does not contain either metal in the reaction, wire and a load to make use of the generated current! • Use Reference Table J to determine the metals to use • Higher = (-) anode Lower = (+) cathode (c) 2006, Mark Rosengarten

  2. Making Voltaic Cells More Info!!! Create Your Own Cell!!!! (c) 2006, Mark Rosengarten

  3. How It Works • The Zn0 anode loses 2 e-, which go up the wire and through the load. The Zn0 electrode gets smaller as the Zn0 becomes Zn+2 and dissolves into solution. The e- go into the Cu0, where they sit on the outside surface of the Cu0 cathode and wait for Cu+2 from the solution to come over so that the e- can jump on to the Cu+2 and reduce it to Cu0. The size of the Cu0 electrode increases. The negative ions in solution go over the salt bridge to the anode side to complete the circuit. Since Zn is listed above Cu, Zn0 will be oxidized when it reacts with Cu+2. The reaction: Zn + CuSO4  ZnSO4 + Cu (c) 2006, Mark Rosengarten

  4. You Start At The Anode (c) 2006, Mark Rosengarten

  5. Make Your Own Cell!!! (c) 2006, Mark Rosengarten

  6. Electrolytic Cells • Use electricity to force a nonspontaneous redox reaction to take place. • Uses for Electrolytic Cells: • Decomposition of Alkali Metal Compounds • Decomposition of Water into Hydrogen and Oxygen • Electroplating • Differences between Voltaic and Electrolytic Cells: • ANODE: Voltaic (-) Electrolytic (+) • CATHODE: Voltaic (+) Electrolytic (-) • Voltaic: 2 half-cells, a salt bridge and a load • Electrolytic: 1 cell, no salt bridge, IS the load (c) 2006, Mark Rosengarten

  7. Decomposing AlkaliMetal Compounds 2 NaCl  2 Na + Cl2 The Na+1 is reduced at the (-) cathode, picking up an e- from the battery The Cl-1 is oxidized at the (+) anode, the e- being pulled off by the battery (DC) (c) 2006, Mark Rosengarten

  8. Decomposing Water 2 H2O  2 H2 + O2 The H+ is reduced at the (-) cathode, yielding H2 (g), which is trapped in the tube. The O-2 is oxidized at the (+) anode, yielding O2 (g), which is trapped in the tube. (c) 2006, Mark Rosengarten

  9. Electroplating The Ag0 is oxidized to Ag+1 when the (+) end of the battery strips its electrons off. The Ag+1 migrates through the solution towards the (-) charged cathode (ring), where it picks up an electron from the battery and forms Ag0, which coats on to the ring. (c) 2006, Mark Rosengarten

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