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Electrochemistry - Battery cells

Electrochemistry - Battery cells. Sec 4 Chemistry 2010. Metals of the reactivity series. Arrange the highlighted metals according to their reactivity. Displacement Reactions. More reactive metal (Cu) + Less reactive metal ion (Ag + ). Displacement Reactions. K.

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Electrochemistry - Battery cells

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  1. Electrochemistry - Battery cells Sec 4 Chemistry 2010

  2. Metals of the reactivity series Arrange the highlighted metals according to their reactivity.

  3. Displacement Reactions • More reactive metal (Cu) + Less reactive metal ion (Ag+)

  4. Displacement Reactions K Cu(s) + Ag+ Cu2+ + Ag(s) Na Ca Mg oxidation Cu(s)  Cu2+ + 2e- Al Zn reduction Fe e- + Ag+ Ag(s) Sn Pb Half-reactions Cu Ag Au

  5. Displacement Reactions K Zn(s) + Cu2+ Cu(s) + Zn2+ Na Ca Mg oxidation Zn(s)  Zn2+ + 2e- Al Zn reduction Fe 2e- + Cu2+ Cu(s) Sn Pb Half-reactions Cu Ag Au

  6. Zn e- Cu2+ e- e- e- e- Half-reactions Oxidation: Zn  Zn2++ 2e- Reduction: Cu2++ 2e- Cu

  7. Cu2+ Electrodes Electrodes Doesn't react with Cu2+, e.g. Cu Zn Doesn't react with Zn, e.g. Zn2+ A half-cell

  8. Half-cells • A half-cell contains half of the redox reaction. • The anode is where the oxidation half-reaction takes place. • The cathodeis where the reduction half-reaction takes place. • What properties must the two electrodes have? • Note: by convention, we draw the anode half-cell on the left hand side.

  9. e- e- ? cathode anode ? reduction oxidation Cu2++ 2e- Cu Zn  Zn2++ 2e- Is the circuit complete? Cu Zn Cu2+ Zn2+

  10. The salt bridge • Allows the flow of ions between the two half-cells. • Consists of an electrolyte: • Doesn't react with the chemical reagents in the cell. • Example: NaNO3 or KNO3

  11. e- e- ? cathode anode salt bridge ? reduction oxidation The salt bridge  anions (A-) Cu Zn cations (C+)  Cu2+ Zn2+

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