In the thermit reaction, aluminium displaces iron from iron(III) oxide.
Write a balanced equation
A mass of 8.38g of iron was produced. Calculate the amount of iron (III) oxide that reacted. (Ar Fe - 55.9)
And calculate to two decimal places the mass of aluminium that was used up in displacing iron from its oxide.
Use values (Al = 27.0g) (O=16)
2007-10-09 07:54:31 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
2Al + Fe2O3 ===> Al2O3 + 2Fe
Molar masses: Fe2O3 = 160
8.38gFe x 1molFe/55.9gFe x 1molFe2O3/2molFe x 160gFe2O3/1molFe2O3 = 11.99g Fe2O3
8.38gFe x 1molFe/55.9gFe x 2molAl/2molFe x 27gAl/1molAl = 4.05g Al
2007-10-09 08:10:04 · answer #1 · answered by steve_geo1 7 · 0⤊ 0⤋
2 Al + 1 Fe2O3 --> 1 Al2O3 + 2 Fe ratios at:
(53.96g) (159.69g) (111.69g)
? g of Fe2O3 = 8.38g of iron ( 159.69) / (111.69) = 11.98
? G OF Al = 8.38 g of iron (53.96) / (111.69) = 4.05
2007-10-09 08:10:22 · answer #2 · answered by Steve O 7 · 0⤊ 0⤋