What is the approximate value of ΔS° for the fuel cell reaction at 25°C? — Electrochemistry Chemistry Question

💡 Solution & Explanation

Using the thermodynamic relationship ΔG° = ΔH° - TΔS°. Substituting the given values at 25°C (298.15 K): -237.39 kJ/mol = -285.8 kJ/mol - 298.15 × ΔS°. Rearranging gives 298.15 × ΔS° = -285.8 + 237.39 = -48.41 kJ/mol. Thus, ΔS° = -48.41 / 298.15 = -0.16236 kJ/(mol·K), which is equal to -162.4 J/(mol·K).