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5 September, 15:22

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.

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Answers (1)
  1. 5 September, 16:53
    0
    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
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