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The Nernst Equation definitions

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Terms in this set (15)

  • Nernst Equation
    Relates cell potential to concentrations of compounds under non-standard conditions.
  • Cell Potential
    The voltage difference between two electrodes in an electrochemical cell.
  • Standard Conditions
    Conditions where concentration is 1 M, temperature is 25°C, pH is 7, and pressure is 1 atm.
  • Gas Constant
    A constant (R) equal to 8.314 J/(mol·K) used in thermodynamic equations.
  • Faraday's Constant
    A constant (F) equal to 96485 C/mol, representing charge per mole of electrons.
  • Reaction Quotient
    A ratio (Q) of product activities to reactant activities in a reaction.
  • Equilibrium Constant
    A constant (K) representing the ratio of product to reactant concentrations at equilibrium.
  • Gibbs Free Energy
    Energy associated with a chemical reaction that can be used to do work.
  • Redox Reaction
    A chemical reaction involving the transfer of electrons between two species.
  • Electrochemical Cell
    A device that generates electrical energy from chemical reactions.
  • Anode
    The electrode where oxidation occurs in an electrochemical cell.
  • Cathode
    The electrode where reduction occurs in an electrochemical cell.
  • Activity Coefficient
    A factor used to account for deviations from ideal behavior in solutions.
  • Equilibrium
    A state where the forward and reverse reactions occur at the same rate.
  • Dead Battery
    A state where the cell potential is zero, indicating equilibrium has been reached.