Question

Consider the following reaction:

3Fe + 4H2O ==> Fe3O4 + 4H2

A) Given the reaction of 52.55 grams of Fe and 20.28 grams of water, determine the limiting reactant.

______

B) Determine the grams of Fe3O4 formed.

______ grams Fe3O

Answer 1

number of moles of Fe = 52.55g / 55.845 g.mol^-1 = 0.941 mole

number of moles of H2O = 20.28g / 18.01 g.mol^-1 = 1.13 mole

from the balanced equation we can say that

3 mole of Fe requires 4 mole of H2O so

0.941 mole of Fe will require

= 0.941 mole of Fe *(4 mole of H2O/3 mole of Fe)

= 1.25 mole of H2O

we have 1.13 mole of H2O which is in short so H2O is limiting reactant.

4 mole of H2O produces 1 mole of Fe3O4 so

1.13 mole of H2O will produce

= 1.13 mole of H2O*(1 mole of Fe₃O₄ / 4 mole of H2O)

= 0.2825 mole of Fe3O4

1 mole of Fe3O4 = 231.533 g

0.2825 mole of fe3O4 = 65.4 g

Therefore, the mass of Fe3O4 produced will be 65.4 g