Given the standard enthalpies of formation for the following substances,determine the change in enthalpy for the combustion of 1.0 mol of butane. Substance

Question

Quizplus · Accepted Answer

The balanced combustion equation for butane is:

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

Using the standard enthalpies of formation given in kJ/mol:

ΔH°rxn = ΣnΔH°f(products) - ΣnΔH°f(reactants)

ΔH°rxn = [8(-393.5 kJ/mol) + 10(-241.8 kJ/mol)] - [2(-124.7 kJ/mol) + 13(0 kJ/mol)]

ΔH°rxn = -2658 kJ/mol

Therefore, the change in enthalpy for the combustion of 1.0 mol of butane is -2658 kJ/mol, which corresponds to choice C.

Given the Standard Enthalpies of Formation for the Following Substances,determine