Use reaction stoichiometry to calculate amounts of reactants

Use reaction stoichiometry to calculate amounts of reactants and products. The substances iron(III) oxide and aluminum react to form aluminum oxide an iron. Unbalanced equation: Fe_2O_3(s) + Al (s) rightarrow Al_2O_3 (s) + Fe (s) In one reaction, 65.8 g of Fe is produced. What amount (in mol) of Al was consumed? What mass (in grams) of Al_2O_3 is produced? mol Al consumed g Al_2O_3 produced

Solution

Balanced equation is

Fe2O3 (s) + 2Al (s) ------> Al2O3 (s) +   2Fe (s)

number of moles of Fe = 65.8 g / 55.845 g.mol^-1 = 1.18 mole

from the balanced equation we can say that

2 mole of Fe is produced by 2 mole of Al so

1.18 mole of Fe will be produced by 1.18 mole of Al

Therefore, the amount of Al consumed is 1.18 mole

from the balanced equation we can say that

2 mole of Fe produces 1 mole of Al2O3 so

1.18 mole of Fe will produce

= 1.18 mole of Fe*(1 mole of Al2O3/2 mole of Fe)

= 0.59 mole of Al2O3

1 mole of Al2O3 = 101.96 g

0.59 mole of Al2O3 = 101.96*0.59 = 60.16 g

Therefore, the amount of Al2O3 produced will be 60.16 g