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Chemistry · Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions

values for the half cell reactions are given: What will be the of the half-cell:

\( E^{o} \) values for the half cell reactions are given: \( \boldsymbol{C u}^{2+}+\boldsymbol{e}^{-} \rightarrow \boldsymbol{C u}^{+} ; \boldsymbol{E}^{o}=\mathbf{0 . 1 5 V} \) \( \boldsymbol{C u}^{2+}+\mathbf{2} e^{-} \rightarrow \boldsymbol{C u} ; \boldsymbol{E}^{o}=\mathbf{0 . 3 4} \mathbf{v} \) What will be the \( E^{o} \) of the half-cell: \( \boldsymbol{C u}^{+}+\boldsymbol{e}^{-} \rightarrow \boldsymbol{C u} ? \)

  • A. \( +0.49 v \)
  • B. \( +0.19 v \)
  • C. +0.53 v \)
  • D. \( +0.30 v \)

Step-by-step solution

The standard Gibbs free energy change for the overall reduction Cu²⁺ → Cu is the sum of that for Cu²⁺ → Cu⁺ and Cu⁺ → Cu. Using ΔG° = -nFE°, we have -2F(0.34) = -1F(0.15) + (-1F)(E° for Cu⁺/Cu). Solving gives E° = 0.68 - 0.15 = 0.53 V.
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