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Chem Test 4 Stack I
Electrochemistry - 12
Term | Definition |
---|---|
Redox Reactions | One chemical species gains electrons while another species loses electrons |
Reduced | Gains electrons |
Oxidized | Loses electrons |
Half-equation Method | Splitting reaction up so that electrons appear explicitly |
Disproportionation | Different atoms of the same chemical element are oxidized and reduced in the course of a single reaction |
Electrochemical Cell | Oxidation and reduction half-reactions are carried out at physically separated electrodes |
Anode | Electrons released by oxidation |
Cathode | Electrons take up by reduction |
Salt-bridge | Small passage between anode and cathode |
Galvanic (voltaic) Cell | Electric current produced by a cell can be used to do work |
Electrolytic Cell | External souce forces a current through the cell and non-spontaneous reactions are caused to occur |
Faraday Constant | Gives the charge per mole of electrons |
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 |
Standard Cell Voltage | Voltage developed by an electrochemical cell in which all reactants and products are in thermodynamic standard states |
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 |
Nernst Equation | The effect of changes of concentrations or pressures on cell voltages |
pH Meter | An application of the Nernst Equation |