What is the value for DeltaS^o"_(reaction) for the following reaction, given the standard entropy values? Fe_2O_3(s) + 3H_2(g) -> 2Fe(s) + 3H_O(g)

Jun 28, 2017

$\Delta {S}^{\circ} = + 138 \cdot J \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$

Explanation:

For........

$F {e}_{2} {O}_{3} \left(s\right) + 3 {H}_{2} \left(g\right) \rightarrow 2 F e \left(s\right) + 3 {H}_{2} O \left(g\right)$

DeltaS^@""_"rxn"=S^@("products")-S^@("reactants")

$\left\{3 \times 189 + 2 \times 27 - 90 - 3 \times 131\right\} \cdot J \cdot K \cdot m o {l}^{-} 1$

$= + 138 \cdot J \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$

Has entropy increased or decreased?