Question

For the following equation determine which reactant is the limiting reactant and which reactant is in excess. The amounts of reagent used are shown. 3Fe(40.0g) + 4H₂O(16.0g) ----> Fe₃O₄ + 4H₂

A) Iron is the limiting reactant; water is in excess
B) Water is the limiting reactant; iron is in excess
C) Both iron and water are in excess
D) Neither iron nor water is in excess

Answer 1

A) Iron is the limiting reactant; water is in excess.In the given equation, 3Fe(40.0g) + 4H₂O(16.0g) → Fe₃O₄ + 4H₂, iron is the limiting reactant while water is in excess.

Step-by-step explanation:

The limiting reactant in a chemical reaction is the reactant that determines the amount of product that can be formed.

In the given equation, 3Fe(40.0g) + 4H₂O(16.0g) → Fe₃O₄ + 4H₂, we need to compare the molar amounts of Fe and H₂O to determine the limiting reactant. To do this, we need to convert the given grams of each reactant to moles using their respective molar masses. Let's calculate:

1. Calculate the moles of Fe: moles = mass/molar mass = 40.0 g/55.85 g/mol = 0.715 mol
2. Calculate the moles of H₂O: moles = mass/molar mass = 16.0 g/18.02 g/mol = 0.888 mol

Since Fe has a lower number of moles compared to H₂O, it is the limiting reactant. Therefore, option A) Iron is the limiting reactant; water is in excess is the correct answer.