Butane c4 h10 ( = –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

Following is the balanced reaction for combustion of butane,

2 C4H10   +      13 O2       →      8 CO2   +     10H2O

Given, Heat of formation of C4H10 =  = -125.7 kJ/mol

Heat of formation of water =  = -241.82 kJ/mol

Heat of formation of CO2 =  = -393.5 kJ/mol

Thus, enthalpy of combustion = ΔH = ∑Hproducts - ∑Hreactants

                                              = 8 + 10 - 2 

                                              = (-393.5X8) + (-241.82X10) - (-125.7X2)

                                              = -5314.8 kJ/mol

This energy would result in combustion of 2 moles of butane

∴ For 1 mole, energy required for combustion of butane = -5314.8/2 = -2657.4 kJ/mol

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