Question

If 3.50 mol of Fe reacts with 3.00 mol of oxygen in the following reaction: 4 Fe(s) + 3 O₂(g) → 2 Fe₂O₃(s) Which of the following statements is correct? If 3.50 mol of Fe reacts with 3.00 mol of oxygen in the following reaction: 4 Fe(s) + 3 O₂(g) → 2 Fe₂O₃ (s) Which of the following statements is correct?

a)Fe is the limiting reactant and 1.75 mol of product can be produced.
b)O₂ is the limiting reactant and 2.00 mol of product can be produced.
c)Fe is the excess reactant and 1.75 mol of product can be produced.
d)O₂ is the excess reactant and 2.00 mol of product can be produced.

Answer 1

Fe is the limiting reactant, and 1.75 mol of Fe₂O₃ can be produced based on the given moles of reactants and the balanced chemical equation. Therefore, the correct option is C.

Step-by-step explanation:

To determine which reactant is the limiting reactant and the amount of product that can be produced, we need to compare the mole ratio of the reactants to their coefficients in the balanced equation. The balanced equation for the reaction is:

4 Fe(s) + 3 O₂(g) → 2 Fe₂O₃(s)

According to the coefficients in the balanced equation, 4 moles of Fe react with 3 moles of O₂. If we have 3.50 mol of Fe and 3.00 mol of O₂, we will compare the available moles to the stoichiometry of the reaction.

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For Fe: (3.50 mol Fe) / (4 mol Fe) = 0.875

For O₂: (3.00 mol O₂) / (3 mol O₂) = 1.00

Since the ratio for Fe is less than that for O₂, Fe is the limiting reactant. We can now calculate the moles of Fe₂O₃ that can be produced using the molar ratio from the balanced equation.

For Fe₂O₃: (3.50 mol Fe) x (2 mol Fe₂O₃) / (4 mol Fe) = 1.75 mol Fe₂O₃

Therefore, Fe is the limiting reactant and 1.75 mol of product can be produced, which makes option c the correct statement.