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Questions and Answers
Which type of cell uses a spontaneous redox reaction to generate electrical energy?
What is the equation used to calculate the electromotive force (emf) of a galvanic cell?
What is the standard potential of a cell?
What is the molar conductivity (✆m) of an ionic solution?
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What does Kohlrausch's law state?
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Study Notes
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.
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Description
Test your knowledge on electrochemical cells, Nernst equation, standard potential, and Gibbs energy with this quiz. Gain a deeper understanding of how to differentiate between galvanic and electrolytic cells and calculate the emf of a galvanic cell using the Nernst equation. Explore the relationship between standard potential, Gibbs energy, and equilibrium constant. Challenge yourself on concepts related to resistance in electrochemical cells.
