Butane Combustion Reaction and Enthalpy Calculation

Enthalpy Calculation in Butane Combustion Reaction

Butane C4 H10 (g), Hf = -125.7 kJ/mol, combusts in the presence of oxygen to form CO2 (g), Hf = -393.5 kJ/mol, and H2 O(g), Hf = -241.82 kJ/mol in the reaction:

2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

The enthalpy change for the combustion reaction is:

a. -5,314.8 kJ/mol

b. -2,657.4 kJ/mol

c. 2,657.4 kJ/mol

d. 5,314.8 kJ/mol

Answer: 2,657.4 kJ/mol

Explanation: -2,657.4 kJ/mol is the enthalpy of the given combustion reaction. Therefore, the correct option is option B.

What is Enthalpy?

A thermodynamic system's functional energy and the product of its own pressure as well as volume are added to form enthalpy, which is one of the system's properties. The labor necessary to determine the system's physical size, or to make more room for it through displacing its surrounds, is expressed by the pressure-volume phrase.

In chemical systems, enthalpy serves as a stand-in for energy; bond, lattice, solvation, and other concepts referred to as "energies" within chemistry are actually differences in enthalpy.

The enthalpy of combustion is calculated using the formula:

ΔH = ∑H(products) - ∑H(reactants)

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

ΔH = -5,314.8 kJ/mol

ΔH = -5,314.8 / 2

ΔH = -2,657.4 kJ/mol

Therefore, the correct option is option B.

What is the enthalpy calculation for the combustion reaction of butane?

The enthalpy calculation for the combustion reaction of butane is -2,657.4 kJ/mol.