Iron ore is impure Fe₂O₃. When Fe₂O₃ is heated with an excess of carbon (coke) , iron metal is produced. How many moles of Fe can be produced from 250 g of Fe₂O₃ by the following reaction?
Fe₂O₃ (s) + 3 C(s) $\rightarrow$ 2 Fe(l) + 3 CO(g)

Question

Iron ore is impure Fe₂O₃. When Fe₂O₃ is heated with an excess of carbon (coke) , iron metal is produced. How many moles of Fe can be produced from 250 g of Fe₂O₃ by the following reaction?
Fe₂O₃ (s) + 3 C(s)

\rightarrow

2 Fe(l) + 3 CO(g)

Quizplus · Accepted Answer

The molar mass of Fe₂O₃ is approximately 159.7 g/mol. 250 g of Fe₂O₃ is equivalent to 250 / 159.7 = 1.57 moles. According to the balanced equation, 1 mole of Fe₂O₃ produces 2 moles of Fe. Therefore, 1.57 moles of Fe₂O₃ will produce 1.57 x 2 = 3.14 moles of Fe, which is approximately 3.13 moles.

Iron Ore Is Impure Fe2O3 →\rightarrow→ 2 Fe(l) + 3 CO(g) A) 5

Iron Ore Is Impure Fe₂O₃ $\rightarrow$ 2 Fe(l) + 3 CO(g)
A) 5