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Standard Cell Potential & the Equilibrium Constant definitions

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  • Galvanic Cell
    A device that generates electricity from a spontaneous redox reaction before equilibrium is reached.
  • Voltaic Cell
    An electrochemical system producing electrical energy from a chemical reaction, operating until equilibrium.
  • Equilibrium Constant
    A value representing the ratio of product to reactant concentrations when a reaction reaches equilibrium.
  • Reaction Quotient
    A measure of the relative amounts of products and reactants at any point, used to predict reaction direction.
  • Nernst Equation
    A formula relating cell potential to standard cell potential, temperature, number of electrons, and reaction quotient.
  • Standard Cell Potential
    The voltage difference between two half-cells under 1 M concentration and 25°C, calculated without the Nernst equation.
  • Gibbs Free Energy
    A thermodynamic quantity indicating the maximum reversible work obtainable from a chemical reaction.
  • Faraday's Constant
    A physical constant representing the charge of one mole of electrons, used in electrochemical calculations.
  • Cathode
    The electrode where reduction occurs, and whose potential is used to determine overall cell voltage.
  • Anode
    The electrode where oxidation occurs, and whose potential is subtracted when finding cell voltage.
  • Standard Conditions
    A set of reference parameters: 1 M concentration, 25°C, and 1 atm pressure, simplifying electrochemical calculations.
  • Logarithm
    A mathematical function used in the Nernst equation to relate cell potential to concentrations and equilibrium.
  • Number of Electrons Transferred
    A value indicating how many electrons move in a redox reaction, crucial for calculating cell potential and energy.
  • Voltage
    The electrical potential difference generated by an electrochemical cell, measured in volts.
  • Spontaneous Reaction
    A process that proceeds on its own, producing electrical energy in a galvanic or voltaic cell.