Question

Iron and oxygen react to form iron(III) oxide; 4Fe(s)+3O2(g)-->2Fe2O3(s). Determine the limiting reactant in each of the following mixtures of reactants: a) 2.0 mol of Fe and 6.0 mol of O2. b) 5.0 mol of Fe and 4.0 mol of O2. c) 16.0 mol of Fe and 20.0 mol of O2. express your answer as a chemical formula.

Answer 1

The limiting reagent in all the three mixtures a, b and c is Iron.

Iron and Oxygen reacts with each other to form iron (III) as follows,

4Fe(s) + 3O₂(g) → 2Fe₂O₃(s)

So, as we can see,

4 moles of Fe reacts with  moles of O₂ to form iron(III) oxide.

So, for every 1 mole of Fe, 3/4 moles of O₂ will required.

Also,

Moles = Given mass/Molar Mass

Molar mass of Fe = 55 g/mol.

Molar mass of Oxygen = 16 g/mol.

a). In mixture of 2.0 mol of Fe and 6.0 mol of O₂,

There are 3 moles of O₂ are present for every one mole of Fe.

So, Fe is the limiting reagent here.

b) In mixture of 5.0 mol of Fe and 4.0 mol of O₂,

4/5 moles of O₂ are present for one mole of O₂.

So, the limiting reagent in this case is Iron.

c) In mixture of 16.0 mol of Fe and 20.0 mol of O₂,

There are 16/20 moles of O₂ are present for one mole of Iron.

So, the Limiting reagent in this case is Iron.

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