Question

The value of ΔS° for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S (s, rhombic) + O2 (g) → SO2 (g) is ________ J/K⋅mol. The value of S° for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S (s, rhombic) + O2 (g) SO2 (g) is ________ J/Kmol. +248.5 +485.4 +11.6 -11.6 -248.5

Answer 1

Answer:

$\large \boxed{\text{11.3 J \cdot K ^{-1} mol ^{-1} }}$

Explanation:

You can calculate the entropy change of a reaction by using the standard molar entropies of reactants and products.

The formula is

$\displaystyle \Delta_{r} S^{\circ} = \sum_n {nS_{\text{products}}^{\circ} - \sum_{m} {mS_{\text{reactants}}^{\circ}}}$

The equation for the reaction is

                        S(s, rhombic) + O₂(g) ⟶ SO₂(g)

ΔS°/J·K⁻¹mol⁻¹         31.8            205.0      248.1

$\Delta_{r} S^{\circ} = 248.1 - (31.8 + 205.0) =248.1 - 236.8 = \large \boxed{\textbf{11.3 J \cdot K ^{-1} mol ^{-1} }}$

The difference probably arises for our use of different sources for the molar entropies.