Problem: Calculate the enthalpy of combustion of butane, C 4H10(g) for the formation of H2O(g) and CO2(g). The enthalpy of formation of butane is −126 kJ/mol.

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Recall: The enthalpy of reaction (ΔH˚rxn) can be calculated from the reactants' and products' enthalpy of formation (∆H˚f) using the equation:

In the combustion, C4H10(l) reacts with O2(g) to form H2O(g) and CO2(g). The chemical equation is:

This equation is not yet balanced. To balance it, add a coefficient of 4 to CO2 to balance the number of C. Add a coefficient of 5 to H2O to balance the number of H. The equation currently looks like this:

The equation currently has 2 O in the reactant side and 13 O in the product side. We add a coefficient of 13/2 to O2 to balance the number of O. The balanced equation is:

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Problem Details

Calculate the enthalpy of combustion of butane, C 4H10(g) for the formation of H2O(g) and CO2(g). The enthalpy of formation of butane is −126 kJ/mol.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.