Answer
Can be harnessed to do work.
Work Step by Step
$\Delta_{r}G^{\circ}=\Sigma n_{p}\Delta_{f}G^{\circ}(products)-\Sigma n_{r}\Delta _{f}G^{\circ}(reactants)$
$=[2\Delta_{f}G^{\circ}(CO_{2},g)]-[2\Delta_{f}G^{\circ}(CO,g)+\Delta_{f}G^{\circ}(O_{2},g)]$
$=[2(-394.359\,kJ/mol)]-[2(-137.168\,kJ/mol)+0]$
$=-514.382\,kJ/mol$
As $\Delta _{r}G^{\circ}$ is negative, the reaction can be harnessed to do work.
