Iron is produced from its ore by the following reactions:
2C(s) + O₂(g) → 2CO(g)
Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g)
How many moles of C₍_s₎ are needed to produce 2.4 mol Fe(s) ?

Question

Iron is produced from its ore by the following reactions: 2C(s) + O₂(g) → 2CO(g) Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) How many moles of C₍_s₎ are needed to produce 2.4 mol Fe(s)?

Quizplus · Accepted Answer

To produce 2.4 mol of Fe(s), 3.6 mol of C(s) are needed because the stoichiometry of the reactions shows that 3 moles of CO(g) are required to produce 2 moles of Fe(s), and 1 mole of C(s) produces 1 mole of CO(g). Therefore, to produce 2.4 mol of Fe(s), 3.6 mol of C(s) are required (1.8 mol of CO(g) per mol of Fe(s) times 2.4 mol of Fe(s) equals 3.6 mol of C(s)).

Iron Is Produced from Its Ore by the Following Reactions