What is the value of ΔS° for the reaction involving propane and oxygen?

To determine the value of ΔS° (the change in standard entropy) for the reaction involving propane and oxygen, it's essential to analyze the molecular changes that occur during the reaction. The combustion of propane (C₃H₈) in oxygen (O₂) produces carbon dioxide (CO₂) and water (H₂O).

In general, the entropy of a system can be influenced by changes in the number of moles of gas, the state of matter (solid, liquid, gaseous), and the complexity of the molecules involved. When propane combusts, it converts from a relatively complex hydrocarbon to simpler molecules like CO₂ and H₂O.

When you compare the number of moles of gaseous reactants to product moles, the reaction tends to increase the number of moles of gas, which typically results in a positive change in entropy. This is due to the increase in disorder or randomness as fewer complex molecules (like propane) are transformed into gaseous products.

Given the likely outputs from standard data tables of entropy values, ΔS° for the combustion of propane generally reflects this tendency toward increased disorder, leading to a positive ΔS° value of approximately 24.2 kJ. This positive value