Butane c4h10 ( = –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:
2c4h10 (g) + 13o2 (g) = 8co2 (g) + 10h2o (g)
what is the enthalpy of combustion, per mole, of butane? (a) -2,657.5 kj/mol(b) -5315.0 kj/mol(c) -509.7 kj/mol(d) -254.8 kj/mol

Explanation:

The formula for calculating the enthalpy change of a reaction by using the enthalpies of formation of reactants and products is

                          2C₄H₁₀ g) + 13O₂(g) ⇌ 8CO₂(g) + 10H₂O(g)

ΔH°f/kJ·mol⁻¹:      -125.7            0            -393.5      -241.82

your answers are a,b,,e and f

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