Chemistry · Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions
The oxidation potential of a hydrogen electrode at and is:
The oxidation potential of a hydrogen electrode at \( p H=10 \) and \( P_{H_{2}}=1 \) is:
- A. \( +0.51 V \)
- B. \( 0.00 V \)
- C. \( +0.590 V \)
- D. \( +0.059 V \)
Step-by-step solution
The half-reaction for hydrogen oxidation is H2 → 2H⁺ + 2e⁻. Using the Nernst equation for the reduction potential (2H⁺ + 2e⁻ → H2): E = E° - (0.05916/2) log(P_H2/[H⁺]²). With E° = 0 V, P_H2 = 1 atm, and pH = 10 → [H⁺] = 10⁻¹⁰ M, the reduction potential is E_red = -0.05916 × pH = -0.5916 V. The oxidation potential is the negative of the reduction potential, giving +0.5916 V ≈ +0.590 V.
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