Butane C4 H10 (g), (Hf = - 125.7), combusts in the presence of oxygen to form CO2 (g) (Hf = - 393.5 kJ/mol), and H2O (g) (Hf = - 241.82) in the reaction: What is the enthalpy of combustion, per mole, of butane? Use

Question

Chemistry

Ruth Robbins

14 August, 04:37

Butane C4 H10 (g), (Hf = - 125.7), combusts in the presence of oxygen to form CO2 (g) (Hf = - 393.5 kJ/mol), and H2O (g) (Hf = - 241.82) in the reaction: What is the enthalpy of combustion, per mole, of butane? Use

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Owen Poole · Answer 1

The combustion reaction, assuming complete combustion and water is gaseous, is

C4 H10 + 13/2 O2 - - - > 4 CO2 + 5 H2O

The enthalpy of combustion is

4 (-393.5) + 5 (-241.82) - (-125.7 + (13/2) (0)) = - 2657.4 kJ/mol