The **standard free energy change of a reaction (ΔG˚ _{rxn})** is given by the following equation:

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{\u2206}}{\mathbf{H}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{T}}{\mathbf{\u2206}}{\mathbf{S}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}}$

The balanced equation is:

6Cl_{2}(g) + 2Fe_{2}O_{3} (s) → 4FeCl_{3}(s) + 3O_{2}(g)

We are going to do the following steps:

Step 1: Calculate ΔH°_{rxn}

Step 2: Calculate ΔS°_{rxn }

Step 3: Calculate ΔG°_{rxn}

Calculate the standard change in Gibbs free energy for the following reaction at 25 °C.

6Cl_{2}(g) + 2Fe_{2}O_{3} (s) → 4FeCl_{3}(s) + 3O_{2}(g)

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