What is the ΔH° for the reaction involving propane and oxygen?

To determine the standard enthalpy change (ΔH°) for the combustion reaction involving propane (C₃H₈) and oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O), we need to consider the overall energy change that occurs when the bonds in the reactants are broken and the bonds in the products are formed.

The combustion of propane can be represented by the balanced reaction:

C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g)

In this reaction, propane and oxygen undergo a reaction that releases a significant amount of energy as carbon dioxide and water are formed. This energy release signifies an exothermic process, where heat is released to the surroundings.

The value for ΔH° represents the heat change for the reaction at standard conditions (1 atm, 25°C). For the combustion of propane, standard enthalpy values obtained from tabulated data indicate that the reaction is highly exothermic. The value -488.7 kJ is indicative of the amount of heat released per mole of propane combusted.

The specific value chosen indicates the heat released when one mole of propane reacts completely with