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Chem Test 4 Stack I

Electrochemistry - 12

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
Created by: iceman15177