Consider the following reaction occurring in the blast furnace.Fe3O4(s)+4CO(g)→3Fe(l)+4CO2(g)'x' kg of iron is produced when 2.32 × 103 kg Fe3O4 and 2.8 × 102 kg CO are brought together in the furnace. The value of 'x' is ____. (nearest integer){Given :Molar mass of Fe3O4 = 232 g mol-1Molar mass of CO = 28 g mol-1Molar mass of Fe = 56 g mol-1}

moles of Fe3O4=2.32×103×103232=10000 mol moles of CO=2.8×102×10328=10000 molFe3O4+4CO⟶3Fe+4CO2 104mol 104molCO is L.R.mole of Fe=34×104mass of Fe=34×104×561000kg=420kg

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Consider the following reaction occurring in the blast furnace.
${Fe}_{3} O_{4 (s)} + 4 {CO}_{(g)} \to 3 {Fe}_{(l)} + 4 {CO}_{2 (g)}$
'x' kg of iron is produced when 2.32 × 10³ kg Fe₃O₄ and 2.8 × 10² kg CO are brought together in the furnace. The value of 'x' is ____. (nearest integer)
{Given :
Molar mass of Fe₃O₄ = 232 g mol^-1
Molar mass of CO = 28 g mol^-1
Molar mass of Fe = 56 g mol^-1}

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answer is 420.

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Detailed Solution

$moles of {Fe}_{3} O_{4} = \frac{2.32 \times 10^{3} \times 10^{3}}{232} = 10000 mol moles of CO = \frac{2.8 \times 10^{2} \times 10^{3}}{28} = 10000 mol$