Butane Combustion: Calculating Enthalpy of Combustion

Calculating Enthalpy of Combustion of Butane

Butane (C₄H₁₀) combusts in the presence of oxygen to form CO₂ (g) and H₂O(g) as shown in the reaction:

2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

Given the heat of formation of:

  • C₄H₁₀ (butane) = -125.7 kJ/mol
  • CO₂ = -393.5 kJ/mol
  • H₂O = -241.82 kJ/mol

Using the formula for enthalpy of combustion:

ΔH = ∑Hproducts - ∑Hreactants

Calculating for the enthalpy of combustion:

ΔH = 8(-241.82) + 10(-393.5) - 2(-125.7)

ΔH = -5314.8 kJ/mol

This energy corresponds to the combustion of 2 moles of butane. Therefore, for 1 mole, the energy required for the combustion of butane is:

-2657.4 kJ/mol

What is the enthalpy of combustion, per mole, of butane?

The enthalpy of combustion, per mole, of butane is -2657.4 kJ/mol.

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