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# Cell Potential: Standard

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Sections
Standard Reduction Potentials
Intro to Electrochemical Cells
Galvanic Cell
Electrolytic Cell
Cell Potential: Standard
Cell Potential: The Nernst Equation
Cell Potential and Gibbs Free Energy
Cell Potential and Equilibrium
Cell Potential: G and K
Cell Notation
Electroplating
###### Understanding Standard Cell Potential

Concept #1: The calculated standard cell potential is measured in units of volts (V).

Example #1: What is E°cell for a voltaic cell based on the following reduction reactions in which the copper electrode is the cathode and the zinc electrode is the anode?

Zn2+ (aq) + 2 e → Zn (s)     E°red = - 0.7621

Cu2+ (aq) + 2 e­ → Cu (s)     E°red = + 0.3394

Concept #2: A galvanic cell possesses a standard cell potential that is greater than zero.

Example #2: Given the following redox reaction: Ce (s) + Al3+ (aq) → Al (s) + Ce3+ (aq). Find its standard cell potential when given the following half-reactions.

Standard Reduction Potentials

Ce3+ + 3 e-  → Ce (s)                          E°red = – 2.336

Al3+ + 3 e-  →  Al (s)                            E°red = – 1.677

Practice: Calculate the standard cell potential of an electrolytic cell when given the following half reactions.

Standard Reduction Potentials

Fe3+ (aq) + e →  Fe2+ (aq)        E°red = + 0.769 V

Li+ (aq) + e →  Li (s)                  E°red = – 3.04 V

Practice: Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.

3 Cl (g) + 2 Fe (s)  →  6 Cl – (aq) + 2 Fe3+ (aq)

Standard Reduction Potentials

Cl(g) + 2 e →  2 Cl – (aq)                      E°red = + 1.396 V
Fe3+ (aq) + 3 e →  Fe (s)                         E°red = – 0.040 V

Practice: Predict whether the following reaction will occur as written based on the calculated Eºcell.

Ag(aq) + Au (s)  →  Ag (s) + Au3+ (aq)

Standard Reduction Potentials

Ag+(aq) + e →  Ag (s)                         E°red = + 0.80 V
Au3+ (aq) + 3 e →  Au (s)                    E°red = + 1.50 V