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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) Calculate the mass of Al2O3 formed when 4.1 g of Al completely reacts.
Express your answer using two significant figures.
b)Calculate the mass of Fe formed when 4.1 g Al completely reacts.
Express your answer using two significant figures.
c)Calculate the mass of Fe formed when 4.1 g Fe2O3 completely reacts.
Express your answer using two significant figures.

Respuesta :

dsdrajlin

According to the given balanced equation:

  • a) 4.1 g of Al form 7.7 g of Al₂O₃.
  • b) 4.1 g of Al form 8.5 g of Fe.
  • c) 4.1 g of Fe₂O₃ form 2.9 g of Fe.

We want to calculate the mass of products when certain amounts of reactants react. This is a stoichiometry problem.

What is stoichiometry?

Stoichiometry refers to the relationship between the quantities of reactants and products before, during, and following chemical reactions.

Let's consider the following balanced equation.

2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(l)

a) Calculate the mass of Al₂O₃ formed when 4.1 g of Al completely reacts.

The mass ratio of Al to Al₂O₃ is 53.96:101.96.

4.1 g Al × 101.96 g Al₂O₃/53.96 g Al = 7.7 g Al₂O₃

b) Calculate the mass of Fe formed when 4.1 g Al completely reacts.

The mass ratio of Al to Fe is 53.96:111.70.

4.1 g Al × 111.70 g Fe/53.96 g Al = 8.5 g Fe

c) Calculate the mass of Fe formed when 4.1 g Fe₂O₃ completely reacts.

The mass ratio of Fe₂O₃ to Fe is 159.69:111.70.

4.1 g Fe₂O₃ × 111.70 g Fe/159.69 g Fe₂O₃ = 2.9 g Fe

According to the given balanced equation:

  • a) 4.1 g of Al form 7.7 g of Al₂O₃.
  • b) 4.1 g of Al form 8.5 g of Fe.
  • c) 4.1 g of Fe₂O₃ form 2.9 g of Fe.

Learn more about stoichiometry here: https://brainly.com/question/16060223