Question

For the reaction shown, calculate how many grams of each product form when the following amounts of reactant completely react to form products. Assume that there is more than enough of the other reactant. 2Al(s)+Fe2O3(s)→Al2O3(s)+2Fe(l)

A.) 4.0 gFe2O3

Answer 1

Number of moles of Fe2O3 = 4.0 g / 159.69 g/mol = 0.0250 mole

from the balanced equation we can say that

1 mole of Fe2O3 produces 1 mole of Al2O3 so

0.0250 mole of Fe2O3 will produce 0.0250 mole of Al2O3

mass of 1 mole of Al2O3 = 101.96 g

so the mass of 0.0250 mole of Al2O3 = 2.55 g

Therefore, the mass of Al2O3 produced would be 2.55 g

1 mole of Fe2O3 produces 2 mole of Fe so

0.0250 mole of Fe2O3 will produce

= 0.0250 mole of Fe2O3 *(2 mole of Fe / 1 mole of Fe2O3)

= 0.0500 mole of Fe

mass of 1 mole of Fe = 55.845 g

so the mass of 0.0500 mole of Fe = 2.79 g

Therefore, the mass of Fe produced would be = 2.79 g