Question$\text{Calculate } \Delta G_{\mathrm{rxn}} \text{ for the following reaction at 298 K. Use the } \Delta G_{\mathrm{f}}^{\circ} \text{ values in this table of thermodynamic properties.}$
$\mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s}) + 3 \mathrm{CO}(\mathrm{g}) \longrightarrow 2 \mathrm{Cr}(\mathrm{s}) + 3 \mathrm{CO}_{2}(\mathrm{g})$
$\Delta G_{\mathrm{rxn}}^{\circ} = \square$
$\square \text{ kJ}$
\text{Is this reaction spontaneous or nonspontaneous at 298 K?}
\text{nonspontaneous}
\text{spontaneous}
\text{The standard Gibbs free energy of formation values are:}
$\Delta G_{\mathrm{f}}^{\circ} \text{ for } \mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s}) \text{ is } -1058.1 \text{ kJ/mol}$
$\Delta G_{\mathrm{f}}^{\circ} \text{ for } \mathrm{CO}(\mathrm{g}) \text{ is } -137.2 \text{ kJ/mol}$
$\Delta G_{\mathrm{f}}^{\circ} \text{ for } \mathrm{Cr}(\mathrm{s}) \text{ is } 0 \text{ kJ/mol}$
$\Delta G_{\mathrm{f}}^{\circ} \text{ for } \mathrm{CO}_{2}(\mathrm{g}) \text{ is } -394.4 \text{ kJ/mol}$