Iron is produced from its ore by the following reactions: 2C(s) + O₂(g) $\rightarrow$ 2CO(g)
Fe₂O₃(s) + 3CO(g) $\rightarrow$ 2Fe(s) + 3CO₂(g)
How many moles of O₂(g) are needed to produce 1.4 mol Fe(s) ?

Question

Iron is produced from its ore by the following reactions: 2C(s) + O₂(g)

\rightarrow

2CO(g)
Fe₂O₃(s) + 3CO(g)

\rightarrow

2Fe(s) + 3CO₂(g)
How many moles of O₂(g) are needed to produce 1.4 mol Fe(s) ?

Quizplus · Accepted Answer

From the second reaction, 3 moles of CO are needed to produce 2 moles of Fe. So, 1.4 moles of Fe require 2.1 moles of CO. From the first reaction, 2 moles of CO require 1 mole of O2. Therefore, 2.1 moles of CO require 1.05 moles of O2.

Iron Is Produced from Its Ore by the Following Reactions →\rightarrow→

Iron Is Produced from Its Ore by the Following Reactions $\rightarrow$