Electrochemical Cells Quiz

Galvanic cells convert chemical energy into electrical energy through spontaneous redox reactions, while electrolytic cells use electrical energy to drive non-spontaneous redox reactions.

The Nernst equation relates the emf of a galvanic cell to the concentrations of reactants and products at non-standard conditions. It is used to calculate the emf of a galvanic cell when the concentrations of species are not at their standard states.

The standard potential of a cell is related to the Gibbs energy of the cell reaction and its equilibrium constant through the equation ΔG = -nFE°, where ΔG is the Gibbs energy change, n is the number of moles of electrons transferred, F is the Faraday constant, and E° is the standard cell potential.

Resistivity (ρ) is a measure of a material's ability to resist the flow of electric current, conductivity (κ) is the reciprocal of resistivity and measures the ability to conduct electric current, and molar conductivity (Λm) is the conductivity of a solution containing 1 mole of the electrolyte.

Kohlrausch's law states that the molar conductivity of an electrolyte at infinite dilution is the sum of the individual ion molar conductivities. It is significant because it allows for the determination of molar conductivity at infinite dilution, which provides insights into the behavior of ions in solution.