Stoichiometry help #3

Question

In a blast furnace, iron(III) oxide is used to produce iron by the following (unbalanced) reaction.

Fe₂O₃(s) + CO(g) —> Fe(s) + CO₂(g)

(a) If 3.60 kg Fe₂O₃ are available to react, how many moles of CO are needed?

_ mol

(b) How many moles of each product are formed?

Fe

_ mol

CO₂

_ mol

Answer 1

first you need to balance out the equation to figure the moles of each substance.

Fe₂O₃(s) + 3CO(g) —> 2Fe(s) + 3CO₂(g)

next calculate the no. of moles of Fe2O3(s) which is 3600g/159.69g/mol=22.54 moles.

a)For every Fe₂O₃(s), you have 3CO(g), so 22.54*3=67.63 moles

b)For every Fe₂O₃(s), you have 2Fe(s), so 22.54*2=45.08 moles

For every Fe₂O₃(s), you have 3CO₂(g), so 22.54*3=67.03 moles