Question

Iron and oxygen react to produce rust. The reaction is actually is a little more complicated, but can be represented below

2 Fe + 3/2 O₂ ---> Fe2O₃
in a particular experiment, 750 grams of Fe is reacted with 750 g of O₂. Is there a limiting reagent
a.) yes: Fe
b.) yes: O₂
c.) no
d.) not enough information to tell

Answer 1

In the given reaction between iron and oxygen, the moles of Fe and O₂ are compared to determine the limiting reagent. By calculating the moles of each substance and comparing it to the stoichiometric ratio, we find that Fe is the limiting reagent.

Step-by-step explanation:

In the given reaction, 2 Fe + 3/2 O₂ → Fe₂O₃, the coefficients in front of the reactants and products represent the stoichiometric ratio of the reaction. To determine the limiting reagent, we need to compare the number of moles of Fe and O₂ used in the reaction.

Using the molar masses of Fe (55.85 g/mol) and O₂ (32.00 g/mol), we can calculate:

Moles of Fe = 750 g / 55.85 g/mol = 13.42 mol

Moles of O₂ = 750 g / 32.00 g/mol = 23.44 mol

Since the stoichiometric ratio of Fe to O₂ is 2:3/2, we can calculate the number of moles of Fe that would be required to react with all of the O₂. Using the ratio:

Moles of Fe required = (3/2) * 23.44 mol = 35.16 mol

Since we only have 13.42 mol of Fe, which is less than the required amount, Fe is the limiting reagent.