The following cell reactions occur spontaneously: (c) Which of the three cell reactions delivers the highest voltage?

Verified step by step guidance

1. Identify the three cell reactions provided in the problem.
2. For each cell reaction, determine the standard electrode potentials (E°) for the cathode and anode from a standard reduction potential table.
3. Calculate the standard cell potential (E°cell) for each reaction using the formula: E°cell = E°cathode - E°anode.
4. Compare the calculated E°cell values for each reaction to determine which one has the highest voltage.
5. Conclude which cell reaction delivers the highest voltage based on the comparison of E°cell values.

Key Concepts

Electrochemical Cells

Electrochemical cells convert chemical energy into electrical energy through redox reactions. They consist of two electrodes, an anode where oxidation occurs, and a cathode where reduction takes place. The voltage produced by a cell is determined by the difference in reduction potentials of the half-reactions occurring at each electrode.

Standard Electrode Potential

The standard electrode potential (E°) is a measure of the tendency of a chemical species to be reduced, measured under standard conditions. Each half-reaction has a specific E° value, and the overall cell potential can be calculated by subtracting the anode potential from the cathode potential. Higher E° values indicate a greater ability to gain electrons and thus a higher voltage output.

Nernst Equation

The Nernst equation relates the cell potential to the concentrations of the reactants and products at non-standard conditions. It allows for the calculation of the voltage of a cell under varying concentrations, temperature, and pressure. Understanding this equation is crucial for determining which cell reaction delivers the highest voltage based on the specific conditions of the reactions.