We can use the following equation to solve for **ΔG˚**** _{rxn}**:

$\overline{){\mathbf{\u2206}\mathbf{G}\mathbf{\xb0}}_{\mathbf{rxn}\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{\u2206}}{\mathbf{G}}{{\mathbf{\xb0}}}_{{\mathbf{prod}}}{\mathbf{-}}{\mathbf{\u2206}}{\mathbf{G}}{{\mathbf{\xb0}}}_{\mathbf{react}\mathbf{}}}$

Note that we need to *multiply each G° by the stoichiometric coefficient* since G˚ is in kJ/mol.

The given reaction is

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

From textbook or internet, we have

ΔG° Cl_{2(g }= 0

ΔG° Fe_{2}O_{3 (s)} = -742.2 kJ/mol

ΔG° FeCl_{3(s)} = -334.0 kJ/mol

ΔG° O_{2(g)} = 0

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

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

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