Question

The reaction between iron(II) oxide and carbon monoxide produces iron and carbon dioxide. How many moles of iron can be obtained when 3.00
mol FeO
reacts with an excess of CO
?

FeO+CO⟶Fe+CO2

Answer 1

The reaction between iron(II) oxide and carbon monoxide produces iron and carbon dioxide. 3.00 moles of iron can be obtained when 3.00 mol FeO  reacts with an excess of CO

Explanation:

During the chemical reaction, products are formed on the basis of the number of moles of reactants available, especially limiting factors. The moles from those reactants is then adapted to balanced chemical reaction factors to form products.

The balanced chemical equation is  

                $1 \mathrm{FeO}+1 \mathrm{CO}>1 \mathrm{Fe}+1 \mathrm{CO}_{2}$

Mole ratio of FeO : Fe is 1:1

That is mole of FeO produces 1 mole of Fe

Given, $n_{Fe O}=3.00 \mathrm {moles}$

So,

                   $n_{F e}=n_{F e 0} \times \frac{1 \text { mole } F_{e}}{1 \text { mole } F_{e O}}$

                   = $3.00 \mathrm{mol} \mathrm{FeO} \times \frac{1 \mathrm{mol} \mathrm{Fe}}{1 \mathrm{mol} \mathrm{FeO}}$

                  = 3.00mol Fe is obtained.