In a bomb calorimeter at 298 K, the internal energy change for the complete combustion of liquid ethanol is ΔU = −1364.5 kJ mol⁻¹: C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) What is ΔH for this reaction at 298 K? (R = 8.314 J K⁻¹ mol⁻¹)

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In a bomb calorimeter at 298 K, the internal energy change for the complete combustion of liquid ethanol is ΔU = −1364.5 kJ mol⁻¹: C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) What is ΔH for this reaction at 298 K? (R = 8.314 J K⁻¹ mol⁻¹)

More NEET Chemistry chapters

Practising is step one. Knowing what to practise next is the hard part.

Practising is step one. Knowing what to practise next is the hard part