Answer:
[tex]\large \boxed{\text{11.3 J$\cdot$K$^{-1}$mol$^{-1}$}}[/tex]
Explanation:
You can calculate the entropy change of a reaction by using the standard molar entropies of reactants and products.
The formula is
[tex]\displaystyle \Delta_{r} S^{\circ} = \sum_n {nS_{\text{products}}^{\circ} - \sum_{m} {mS_{\text{reactants}}^{\circ}}}[/tex]
The equation for the reaction is
S(s, rhombic) + O₂(g) ⟶ SO₂(g)
ΔS°/J·K⁻¹mol⁻¹ 31.8 205.0 248.1
[tex]\Delta_{r} S^{\circ} = 248.1 - (31.8 + 205.0) =248.1 - 236.8 = \large \boxed{\textbf{11.3 J$\cdot$K$^{-1}$mol$^{-1}$}}[/tex]
The difference probably arises for our use of different sources for the molar entropies.
