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Using the equations N2 (g) + O2 (g) → 2 NO (g) AH° = 180.6 kJ/mol N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (g) AH° = -483.7 kJ/mol %3D %3D |I. %3D Determine the 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) AH° = 180.6 kJ/mol N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (g) AH° = -483.7 kJ/mol %3D %3D |I. %3D Determine the enthalpy (in kJ/mol) for the reaction 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g).

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
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Using the equations N2 (g) + O2 (g) → 2 NO (g) AH° = 180.6 kJ/mol N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (g) AH° = -483.7 kJ/mol %3D Determine the enthalpy (in kJ/mol) for the reaction 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g).
Transcribed Image Text:Using the equations N2 (g) + O2 (g) → 2 NO (g) AH° = 180.6 kJ/mol N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (g) AH° = -483.7 kJ/mol %3D Determine the enthalpy (in kJ/mol) for the reaction 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g).
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