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Coulometry definitions

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  • Electrochemical Cell
    A system where chemical reactions involve electron transfer, classified by reaction spontaneity and energy flow.
  • Galvanic Cell
    A device that converts spontaneous chemical energy into electrical energy, producing electricity as it operates.
  • Electrolytic Cell
    A setup requiring external energy to drive non-spontaneous reactions, consuming electricity to function.
  • Spontaneity
    A property indicating whether a reaction proceeds naturally without external energy input, linked to cell type.
  • Gibbs Free Energy
    A thermodynamic quantity predicting reaction direction; negative values indicate spontaneous processes.
  • Equilibrium Constant
    A ratio expressing the concentrations of products to reactants at equilibrium, revealing reaction favorability.
  • Cell Potential
    The voltage difference between electrodes, determining the ability of a cell to drive electron flow.
  • Entropy
    A measure of disorder or randomness in a system, influencing reaction spontaneity and cell classification.
  • Reaction Quotient
    A value comparing current reactant and product concentrations to those at equilibrium, indicating reaction direction.
  • Anode
    The electrode where oxidation occurs, with its charge depending on cell type—negative in galvanic, positive in electrolytic.
  • Cathode
    The electrode where reduction takes place, with its charge reversed between galvanic and electrolytic cells.
  • Oxidation
    A process involving electron loss at one electrode, always occurring at the same location in both cell types.
  • Reduction
    A process involving electron gain at one electrode, consistently occurring at the same site in all electrochemical cells.
  • Equilibrium
    A state where all driving forces balance, resulting in no net reaction and representing a 'dead battery' in cells.
  • Battery
    An external energy source required to drive non-spontaneous reactions in electrolytic cells, forcing electron movement.