Butane C4 H10 (g),(Delta. Hf = –125.7), combusts in the presence of oxygen to form CO2 (g) (Delta. Hf = –393.5 kJ/mol), and H2 O(g) (Delta. Hf = –241.82) in the reaction:

2 upper C subscript 4 upper H subscript 10 (g) plus 13 upper O subscript 2 (g) right arrow 8 upper C upper O subscript 2 plus 10 upper H subscript 2 upper O (g).

What is the enthalpy of combustion, per mole, of butane?
Use Delta H r x n equals the sum of delta H f of all the products minus the sum of delta H f of all the reactants..
–5,314.8 kJ/mol
–2,657.4 kJ/mol
2,657.4 kJ/mol
5,314.8 kJ/mol