Final answer:
The chemical equation for the reaction between aluminum and iron(II) oxide forming aluminum oxide and iron is balanced as 2 Al(s) + Fe2O3(s) → 2 Fe(s) + Al2O3(s), following stoichiometry and the law of conservation of mass.
Step-by-step explanation:
Balancing a Chemical Reaction
The question involves balancing a chemical equation for a reaction between aluminum (Al) and iron(II) oxide (FeO) to produce aluminum oxide (Al2O3) and iron (Fe). To balance the equation, we consider the following balanced chemical equation: 2 Al(s) + Fe2O3(s) → 2 Fe(s) + Al2O3(s).
The coefficients indicate that for every 2 moles of Al that reacts with 1 mole of Fe2O3, 2 moles of Fe and 1 mole of Al2O3 are produced. This reaction is a part of stoichiometry, which is the calculation of reactants and products in chemical reactions in chemistry.
According to the given mass of reactants and products, the balanced equation correctly represents the conservation of mass, as there is a total of 270 grams (54g Al + 216g FeO) of reactants and 270 grams (102g Al2O3 + 168g Fe) of products. This follows the law of conservation of mass.
This type of reaction, where aluminum is used to reduce iron from its oxide, is also referred to as the thermite reaction, and it is exothermic, releasing heat as a product.