For complete combustion of ethanol C2H5OH(ℓ) + 3O2(g) → 2CO2(g) + 3H2O(ℓ), the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol–1 at 25°C. Assuming ideality the Enthalpy of combustion, ΔCH, for the reaction will be (R = 8.314 kJ mol

Engineering

Chemistry

Calorimetry

Enthalpy and Internal Energy Relation

Question

For complete combustion of ethanol

C₂H₅OH(ℓ) + 3O₂(g) → 2CO₂(g) + 3H₂O(ℓ), the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol^–1 at 25°C. Assuming ideality the Enthalpy of combustion, Δ_CH, for the reaction will be

(R = 8.314 kJ mol^–1)

– 1460.50 kJ mol^–1

– 1361.95 kJ mol^–1

– 1366.95 kJ mol^–1

– 1350.50 kJ mol^–1

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ΔH = ΔE + Δn_g.RT

= (–1364.47) + (2 – 3) × $\frac{8.314}{1000}$ × 298

= –1366.95 kJ/mol

(No need to solve exactly. Answer may be given directly)