Consider the following reaction occurring in the blast furnace: Fe_3 O_4( s ) +4 CO_( g ) → 3 Fe_( l ) +4 CO_2( g ) ' x ' kg of iron is produced when…

Consider the following reaction occurring in the blast furnace: $$\mathrm{Fe}_3 \mathrm{O}_{4(\mathrm{~s})}+4 \mathrm{CO}_{(\mathrm{g})} \rightarrow 3 \mathrm{Fe}_{(\mathrm{l})}+4 \mathrm{CO}_{2(\mathrm{~g})} $$ ' $\displaystyle x$ ' kg of iron is produced when $\displaystyle 2.32 \times 10^3 \mathrm{~kg} \mathrm{Fe}_3 \mathrm{O}_4$ and $\displaystyle 2.8 \times 10^2 \mathrm{~kg} \mathrm{CO}$ are brought together in the furnace. The value of ' $\displaystyle x$ ' is $\displaystyle \_\_\_\_$. (nearest integer) {Given: molar mass of $\displaystyle \mathrm{Fe}_3 \mathrm{O}_4=232 \mathrm{~g} \mathrm{~mol}^{-1}$ molar mass of $\displaystyle \mathrm{CO}=28 \mathrm{~g} \mathrm{~mol}^{-1}$ molar mass of $\displaystyle \left.\mathrm{Fe}=56 \mathrm{~g} \mathrm{~mol}^{-1}\right\}$