Electrochemistry - 12
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| Redox Reactions | One chemical species gains electrons while another species loses electrons
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| Reduced | Gains electrons
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| Oxidized | Loses electrons
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| Half-equation Method | Splitting reaction up so that electrons appear explicitly
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| Disproportionation | Different atoms of the same chemical element are oxidized and reduced in the course of a single reaction
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| Electrochemical Cell | Oxidation and reduction half-reactions are carried out at physically separated electrodes
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| Anode | Electrons released by oxidation
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| Cathode | Electrons take up by reduction
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| Salt-bridge | Small passage between anode and cathode
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| Galvanic (voltaic) Cell | Electric current produced by a cell can be used to do work
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| Electrolytic Cell | External souce forces a current through the cell and non-spontaneous reactions are caused to occur
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| Faraday Constant | Gives the charge per mole of electrons
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| Electrical Work | Equal to the change in Gibbs energy of the redox reaction and to the product of the total charge passing through the external circuit and the cell voltage
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| Standard Cell Voltage | Voltage developed by an electrochemical cell in which all reactants and products are in thermodynamic standard states
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| Half-Cell Reduction Potentials | Expresses the intrinsic tendency of a reduction half-reaction to occur when both the reactant and product are in standard states
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| Nernst Equation | The effect of changes of concentrations or pressures on cell voltages
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| pH Meter | An application of the Nernst Equation
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