Final answer:
To determine the standard entropy change for the reaction given, the sum of the standard entropies of the products is subtracted from the sum of the standard entropies of the reactants using their stoichiometric coefficients from the balanced equation.
Step-by-step explanation:
To calculate the standard entropy change (ΔS°) for the reaction 2CH3OH(g) + 3O2(g) → 2CO2(g) + 4H2O(g) at 25 °C, use the standard molar entropy values from Appendix G or Table 13.6.1. The entropy change is equal to the sum of the standard entropies of the products minus the sum of the standard entropies of the reactants, each multiplied by their stoichiometric coefficients in the balanced equation.
The formula to compute the entropy change is:
ΔS° = Σ(nS°products) - Σ(nS°reactants)
Where 'n' is the stoichiometric coefficient and S° are the standard molar entropies of the substances involved in the reaction. Once the appropriate values for CH3OH, O2, CO2, and H2O are retrieved from the provided data sources, they can be plugged into the formula as follows:
ΔS° = [2 × S°(CO2) + 4 × S°(H2O)] - [2 × S°(CH3OH) + 3 × S°(O2)]
Calculate this value using the given entropies to determine the standard entropy change for this particular reaction.