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The Nernst Equation quiz #1

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Terms in this set (10)

  • What factors affect the cell potential (E_cell) under nonstandard conditions?
    Under nonstandard conditions, E_cell is affected by the concentrations of reactants and products, temperature, and pressure, as described by the Nernst equation.
  • The Nernst equation represents the balance between which two quantities in an electrochemical cell?
    The Nernst equation represents the balance between the standard cell potential (E°_cell) and the effect of the reaction quotient (Q) on cell potential under nonstandard conditions.
  • What is the value of E°_cell (standard cell potential) for a cell measured under standard conditions?
    E°_cell is the cell potential measured under standard conditions: 1 M concentration, 1 atm pressure, 25°C temperature, and pH 7.
  • What does the variable 'n' represent in the Nernst equation?
    The variable 'n' represents the number of electrons transferred in the redox reaction.
  • How is the gas constant (R) used in the Nernst equation, and what is its value?
    R is the gas constant used in the Nernst equation, and its value is 8.314 joules per mole per kelvin.
  • What happens to the cell potential as the reaction quotient Q increases over time in an electrochemical cell?
    As Q increases, the cell potential decreases until it reaches zero at equilibrium, indicating a dead battery.
  • How can the Nernst equation be rewritten using the log function instead of the natural logarithm?
    By multiplying the natural logarithm term by 2.303, the Nernst equation can be rewritten using the log function with a coefficient of 0.05916 volts divided by n.
  • What is the relationship between the equilibrium constant (K) and the standard cell potential (E°_cell) according to the Nernst equation?
    At equilibrium, ln K equals n times E°_cell divided by 0.0257 volts, or K equals 10 to the power of n times E°_cell divided by 0.05916 volts when using the log function.
  • How does Gibbs free energy (ΔG) relate to the equilibrium constant (K) at equilibrium?
    At equilibrium, ΔG equals zero, and ln K equals ΔG° divided by RT, so K equals e to the power of ΔG° divided by RT.
  • Why is the Nernst equation used instead of the standard cell potential equation under nonstandard conditions?
    The Nernst equation is used when concentrations, temperature, or pressure differ from standard conditions, allowing calculation of cell potential under these nonstandard conditions.