We’re being asked to determine the **ΔG° (kJ) **for the reaction below at **298 K:**

**SiCl _{4(g) }+ 2 Mg_{(s) }→ Si_{(s)} + 2 MgCl_{2}**

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

$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{prod}}{\mathbf{-}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{react}}}$

At 298 K, ΔG°f is -620 kJ/mol for SiCl4(g) and -592 kJ/mol for MgCl2(s). Calculate ΔG° (kJ) for the reaction below at 298 K if the pressure of SiCl4(g) is 1 atm. Enter your answer as the nearest whole number with no units.

SiCl4(g) + 2Mg(s) --> Si(s) + 2 MgCl_{2}(s)

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