Consider the following reaction occurring in the blast furnace: $Fe_3O_{4(s)} + 4CO_{(g)} \rightarrow 3Fe_{(l)} + 4CO_{2(g)}$. '$x$' kg of iron is produced when $2.32 \times 10^3 \ kg$ of $Fe_3O_4$ and $2.8 \times 10^2 \ kg$ of $CO$ are brought together in the furnace. The value of '$x$' is $.............$ (nearest integer). Given: Molar mass of $Fe_3O_4 = 232 \ g \ mol^{-1}$,Molar mass of $CO = 28 \ g \ mol^{-1}$,Molar mass of $Fe = 56 \ g \ mol^{-1}$.
- A$420$
- B$320$
- C$220$
- D$250$
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