Determine $\Delta$S^$\circ$ for the reaction SO₃(g) + H₂O(l) $\rarr$ H₂SO₄(l). $\begin{array}{lc} &\mathrm{S}^{\circ}(\mathrm{J} / \mathrm{K} \cdot \mathrm{~mol})\\hline \mathrm{SO}_{3} & 256.2 \ \mathrm{H}_{2} \mathrm{O} & 69.9 \ \mathrm{H}_{2} \mathrm{SO}_{4} & 156.9 \end{array}$ A) 169.2 J/K·mol B) 1343.2 J/K·mol C) -169.2 J/K·mol D) -29.4 J/K·mol E) 29.4 J/K·mol

Question

Quizplus · Accepted Answer

We can use Hess's Law to determine the enthalpy change for the reaction. First, we need to reverse the direction of the last reaction and change the sign of its enthalpy change: H₂SO₄(l) → SO₃(g) + H₂O(l) ΔH° = -F1F1F10 Next, we can use the enthalpy changes for the following reactions: SO₃(g) + O2(g) → SO₄(l) ΔH° = -F1F1F1S1 H₂O(l) + O2(g) → HO2₂O(l) ΔH° = -SF1F1F1 SO₃(g) + HO2₂O(l) → SO₄(l) + O2(g) + H2O(l) ΔH° = -F1F1F1S1 By adding these reactions, we get: SO₃(g) + H₂O(l) → SO₄(l) ΔH° = -F1F1F1S1 - SF1F1F1 - F1F1F1S1 = -169.2 J/K·mol Therefore, the answer is C.

Determine Δ\DeltaΔ S ∘\circ∘ for the Reaction SO3(g) + H2O(l) →\rarr→ H2SO4(l)

Determine $\Delta$ S^$\circ$ for the Reaction SO₃(g) + H₂O(l) $\rarr$ H₂SO₄(l)