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Ch.19 - Electrochemistry
McMurry - Chemistry 8th Edition
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Tutti i libri di testoMcMurry 8th EditionCh.19 - ElectrochemistryProblema 79
Capitolo 19, Problema 79

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

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

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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.
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Electrochemical Cells

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.
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Standard Cell Potential

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.
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The Nernst Equation
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The following cell reactions occur spontaneously: (a) Arrange the following reduction half-reactions in order of decreasing tendency to occur:

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