We’re being asked **to determine the standard enthalpy change of formation (ΔH˚ _{f})** for

$\overline{){\mathbf{\u2206}}{\mathbf{H}}{{\mathbf{\xb0}}}_{\mathbf{r}\mathbf{x}\mathbf{n}}{\mathbf{}}{\mathbf{=}}{\mathbf{\u2206}}{\mathbf{H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{p}\mathbf{r}\mathbf{o}\mathbf{d}\mathbf{u}\mathbf{c}\mathbf{t}\mathbf{s}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{\u2206}}{\mathbf{H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{p}\mathbf{r}\mathbf{o}\mathbf{d}\mathbf{u}\mathbf{c}\mathbf{t}\mathbf{s}}}$

We’re given the **ΔH˚ _{rxn}** for the combustion of 2 moles of CO

2 CO_{(g)} + O_{2}_{(g)} → 2CO_{2}_{(g)}

This equation is already balanced.

The ΔH_{f}° for CO_{2} (g) is -393 kJ/mole and ΔH_{rxn} for the reaction

2CO(g) + O_{2}(g) → 2CO_{2}(g) is -560 kJ. The ΔH_{f}° for CO(g) is (in kJ/mole):

(a) +113

(b) -673

(c) -113

(d) -209

(e) -226

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