Question

54g of aluminum reacts with 216g of iron(II) oxide, forming 102g of aluminum oxide and 168g of iron. Balance the equation. Round the number of moles to the nearest whole number.

Al + FeO -> Al2O3 + Fe
A) 4Al + 3FeO -> 2Al2O3 + 3Fe
B) 2Al + FeO -> Al2O3 + Fe
C) 6Al + 5FeO -> 3Al2O3 + 5Fe
D) 3Al + 2FeO -> Al2O3 + 2Fe

Answer 1

The correct balanced chemical equation for the reaction between aluminum and iron(III) oxide is 2 Al(s) + Fe2O3(s) → 2 Fe(s) + Al2O3(s), representing a simple whole-number ratio of reactants to products.

Step-by-step explanation:

In this thermochemical equation, we are dealing with a reaction between solid aluminum (Al) and iron (III) oxide (Fe2O3). The products of this reaction are solid iron (Fe) and aluminum oxide (Al2O3) plus heat, indicating an exothermic reaction. The balanced chemical equation for this reaction is 2 Al(s) + Fe2O3(s) → 2 Fe(s) + Al2O3(s). All reagents and products have their coefficients in the simplest whole-number ratio, demonstrating the principle of conservation of mass.