Using the equations N₂ (g) + O₂ (g) → 2 NO (g) ∆H° = 180.6 kJ/mol N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol 2 H₂ (g) + O₂ (g) → 2 H₂O (g) ∆H° = -483.7 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g).
Using the equations N₂ (g) + O₂ (g) → 2 NO (g) ∆H° = 180.6 kJ/mol N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol 2 H₂ (g) + O₂ (g) → 2 H₂O (g) ∆H° = -483.7 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g).
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section16.9: Gibbs Free Energy And Biological Systems
Problem 16.13E
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Using the equations
N₂ (g) + O₂ (g) → 2 NO (g) ∆H° = 180.6 kJ/mol
N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol
2 H₂ (g) + O₂ (g) → 2 H₂O (g) ∆H° = -483.7 kJ/mol
Determine the molar enthalpy (in kJ/mol) for the reaction
4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g).
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