For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode: E∘cell=E∘red (reduction process) - E∘red (oxidation process)

For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode:

E∘cell=E∘red (reduction process) - E∘red (oxidation process)

Part A

Calculate the standard cell potential given the following standard reduction potentials:

Al3++3e-→Al; E∘=-1.66 V

Cu2++2e-→Cu; E∘=0.340 V

Express your answer to two decimal places and include the appropriate units.

Question

Eileen Knapp

Chemistry

9 November, 08:32

For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode: E∘cell=E∘red (reduction process) - E∘red (oxidation process)

For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode:

E∘cell=E∘red (reduction process) - E∘red (oxidation process)

Part A

Calculate the standard cell potential given the following standard reduction potentials:

Al3++3e-→Al; E∘=-1.66 V

Cu2++2e-→Cu; E∘=0.340 V

Express your answer to two decimal places and include the appropriate units.

+3

Answers (1)

Know the Answer?

Stacy · Answer 1

E°cell = 2.00 V

Explanation:

Let's consider the following reductions with their respective standard reduction potentials.

Al³⁺ + 3 e⁻ → Al; E°red = - 1.66 V

Cu²⁺ + 2 e⁻ → Cu; E°red = 0.340 V

The one with the higher standard reduction potential will occur as a reduction (cathode) while the other will occur as an oxidation (anode). The corresponding half-reactions are:

Anode (oxidation) : Al → Al³⁺ + 3 e⁻; E°red = - 1.66 V

Cathode (reduction) : Cu²⁺ + 2 e⁻ → Cu; E°red = 0.340 V

The standard cell potential (E°cell) can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode:

E°cell=E°red (reduction process) - E°red (oxidation process) = 0.340V - (-1.66V) = 2.00V