Calculate the energy released by the reaction  $4\mathrm{Fe}\left(s\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)⟶2{\mathrm{Fe}}_2{\mathrm{O}}_3\left(s\right)$ when a $55.8 \mathrm{g}$ sample of iron reacts completely with $1.00$ mole of oxygen. The enthalpy of formation $\left(\mathrm{\Delta }{H}_f^{\circ }\right)$ of ${\mathrm{Fe}}_2{\mathrm{O}}_3\left(s\right)$ is $-826\mathrm{kJ}\times {\mathrm{mol}}^{-1}$