Final answer:
The value for ∆S°reaction for the given chemical reaction is -68.6 J/(mol·K).
Step-by-step explanation:
The value of the standard entropy change, ∆S°reaction, for the given reaction can be calculated by using the standard entropy values of the reactants and products. The formula is: ∆S°reaction = Σ(S°products) - Σ(S°reactants). For the given reaction: 2H2S(g) + SO2(g) → 3Srhombic(s) + 2H2O(g), the standard entropy values are:
- S°(H2S) = 206.7 J/(mol·K)
- S°(SO2) = 248.1 J/(mol·K)
- S°(Srhombic) = 42.9 J/(mol·K)
- S°(H2O) = 188.7 J/(mol·K)
Using the formula, ∆S°reaction = (3*S°(Srhombic)) + (2*S°(H2O)) - (2*S°(H2S)) - (S°(SO2)), we can calculate:
∆S°reaction = (3*42.9) + (2*188.7) - (2*206.7) - 248.1
∆S°reaction = -68.6 J/(mol·K)