A fuel cell runs on H₂(g) + 12 O₂(g) → H₂O(l) at 298 K and standard pressure. Δf H° of H₂O(l) is -285.8 kJ mol⁻¹, and the standard molar entropies are H₂(g) 130.7, O₂(g) 205.1 and H₂O(l) 69.9 J K⁻¹ mol⁻¹. What is the largest amount of useful (non-expansion) work the cell can deliver from 1.00 kg of hydrogen (M = 2.016 g mol⁻¹)?

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A fuel cell runs on $\text{H}_2(g) + \tfrac12\,\text{O}_2(g) \rightarrow \text{H}_2\text{O}(l)$ at $298\ \text{K}$ and standard pressure. $\Delta_f H^\circ$ of $\text{H}_2\text{O}(l)$ is $-285.8\ \text{kJ mol}^{-1}$ , and the standard molar entropies are $\text{H}_2(g)$ $130.7$ , $\text{O}_2(g)$ $205.1$ and $\text{H}_2\text{O}(l)$ $69.9\ \text{J K}^{-1}\ \text{mol}^{-1}$ . What is the largest amount of useful (non-expansion) work the cell can deliver from $1.00\ \text{kg}$ of hydrogen ( $M = 2.016\ \text{g mol}^{-1}$ )?

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← For N₂(g) + 3 H₂(g) → 2 NH₃(g) at 298 K, Δr H° = -92.4 kJ mol⁻¹. The bond enthalpies are N≡N 946 kJ mol⁻¹ and H-H 435.8 kJ mol⁻¹; the molar mass of ammonia is 17.03 g mol⁻¹ and R = 8.314 J K⁻¹ mol⁻¹. Which of the following statements are correct?One mole of an ideal gas at 1.00 bar sits in a cylinder in a large water bath at 300 K. The external pressure on the piston is suddenly raised to 5.00 bar and held there, and the gas is squeezed until its pressure is 5.00 bar, ending at 300 K. Take R = 8.314 J K⁻¹ mol⁻¹ and 1 L bar = 100 J. What is the total entropy change of the gas and the water bath? →

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