Using only the following data:
$\text{ I) }{\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+3\mathrm{CO}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{Fe}\left(\mathrm{s}\right)+3{\mathrm{CO}}_2\left(\mathrm{g}\right);{\mathrm{\Delta H}}^{\circ }=-26.8\mathrm{kJ}$
$\text{ II) }\mathrm{Fe}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)\rightleftharpoons \mathrm{FeO}\left(\mathrm{s}\right)+\mathrm{CO}\left(\mathrm{g}\right);{\mathrm{\Delta H}}^{\circ }=+16.5\mathrm{kJ}\text{ the }{\mathrm{\Delta H}}^0$ value, in kJ, for the reaction ${\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+\mathrm{CO}\left(\mathrm{g}\right)\to 2\mathrm{FeO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$ is calculated to be: