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Reverse second: Δ H = 283 kJ. Add third: Δ H = 241.8 kJ. Subtract first: Δ H = 283 + 241.8 - 393.5 = 131.3 kJ/mol.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Third Law of Thermodynamics and Applications
Reverse the third equation and add the first two: Δ H = -393.5 + (-2 × 285.8) + 890.3 = -74.8 kJ/mol.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy
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