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.

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

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

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