Electrochemical Cells Quiz

Galvanic Cells

• A galvanic cell, also known as a voltaic cell, uses a spontaneous redox reaction to generate electrical energy.
• The cell consists of two half-cells, each containing an electrode and an electrolyte, connected by an electrically conducting wire and a salt bridge.

Electromotive Force (EMF)

• The electromotive force (EMF) of a galvanic cell is calculated using the Nernst equation: Ecell = E°cell - (RT/nF) ln(Q).
• EMF is the maximum potential difference developed between the two electrodes of a galvanic cell.

Standard Potential

• The standard potential of a cell is the potential difference developed under standard conditions, i.e., at 25°C, 1 atm, and 1 M concentration of reactants.

Molar Conductivity

• Molar conductivity (Λm) is the conductivity of an ionic solution per unit concentration of the electrolyte.
• It is calculated as the conductivity of the solution (κ) divided by the concentration of the electrolyte (c): Λm = κ / c.

Kohlrausch's Law

• Kohlrausch's law states that the molar conductivity of an ionic solution at infinite dilution (Λm°) is the sum of the molar conductivity of the individual ions.
• The law allows for the calculation of the molar conductivity of an ionic solution at infinite dilution from the conductivity of the individual ions.