−278 kJ molClick to see full answer. Herein, what is the enthalpy of c2h5oh?Standard enthalpies of formation are: C2H5OH(l) -228, CO2(g) -394, and H2O(l) -286 kJ/mol. what is the enthalpy of formation of butane? Thermodynamic properties Phase behavior Std enthalpy change of formation, ΔfHogas –125.6 kJ/mol Standard molar entropy, Sogas 310.23 J/(mol K) Enthalpy of combustion, ΔcHo –2877.5 kJ/mol Heat capacity, cp 98.49 J/(mol K) at 25°C Accordingly, which equation represents the standard enthalpy of formation for ethanol c2h5oh? Given the standard enthalpies of formation (C2H5OH(l) = -267.0 kJ/mol, H2O(g) = -241.8 kJ/mol, and CO2(g) = -393.5 kJ/mol), how many grams of ethanol must be combusted to release 30.5 kJ of energy?How do you find enthalpy? Use the formula ∆H = m x s x ∆T to solve. Once you have m, the mass of your reactants, s, the specific heat of your product, and ∆T, the temperature change from your reaction, you are prepared to find the enthalpy of reaction. Simply plug your values into the formula ∆H = m x s x ∆T and multiply to solve.