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?

ChemistryAdvancedHigh School (11–12)Chemical Thermodynamics › Enthalpy and Hess's Law JEE Advanced

For $\text{N}_2(g) + 3\,\text{H}_2(g) \rightarrow 2\,\text{NH}_3(g)$ at $298\ \text{K}$ , $\Delta_r H^\circ = -92.4\ \text{kJ mol}^{-1}$ . The bond enthalpies are $\text{N}{\equiv}\text{N}$ $946\ \text{kJ mol}^{-1}$ and $\text{H{-}H}$ $435.8\ \text{kJ mol}^{-1}$ ; the molar mass of ammonia is $17.03\ \text{g mol}^{-1}$ and $R = 8.314\ \text{J K}^{-1}\ \text{mol}^{-1}$ . Which of the following statements are correct?

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← For 2 NO(g) + O₂(g) → 2 NO₂(g): Δf H° of NO(g) is +90.25 and of NO₂(g) +33.18 kJ mol⁻¹; the standard molar entropies are NO(g) 210.8, O₂(g) 205.1 and NO₂(g) 240.1 J K⁻¹ mol⁻¹. Take Δ H° and Δ S° as constant. Which of the following statements are correct?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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