The standard Gibbs energy change for the reaction
H⁺ (aq) + OH^- (aq) → H₂O (l)
Is -80.1 kJ mol^-1 at 298 K. Determine the standard reaction potential for the cell
Pt (s) | O₂ (g) | H⁺ (aq) ║ OH^- (aq) | O₂ (g) | Pt (s)
At this temperature.

Question

Quizplus · Accepted Answer

The standard reaction potential (E°) can be calculated using the relation ΔG° = -nFE°, where ΔG° is the standard Gibbs energy change, n is the number of moles of electrons transferred, and F is the Faraday constant (96485 C/mol). For this reaction, n = 2. Solving for E° gives E° = -ΔG°/(nF) = 80.1 kJ/mol / (2 * 96485 C/mol) = 0.83 V.

The Standard Gibbs Energy Change for the Reaction