**Given equation:** 2 CO(g) + O_{2}(g) ⇌ 2 CO_{2}(g)

Recall that **Δ****G****˚**_{rxn} * and K* are related to each other:

$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

To solve for **Δ****G****˚***_{rxn}*:

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

Use data from appendix iib in the textbook to calculate the equilibrium constants at 25 degrees Celsius for each of the following reaction:

2 CO (g) + O2(g) ↔ 2CO2 (g)

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