To determine the limiting reagent for the chemical reaction, we need to understand the balanced equation for the reaction between iron (Fe) and oxygen (O₂) to form iron(III) oxide (Fe₂O₃). The balanced chemical equation is:
[tex]\[ 4 Fe + 3 O_2 \rightarrow 2 Fe_2O_3 \][/tex]
This equation tells us that 4 moles of iron react with 3 moles of oxygen to produce 2 moles of iron(III) oxide.
1. Determine the given information:
- Moles of Fe: 4 moles
- Moles of O₂: 3 moles
2. Relate the moles of reactants to the balanced equation:
- According to the equation, 4 moles of Fe are needed to react with 3 moles of O₂.
3. Calculate the reaction ratios for each reactant:
- For iron (Fe):
[tex]\[
\text{ratio of Fe} = \frac{\text{moles of Fe}}{\text{moles of Fe needed}}
= \frac{4}{4} = 1.0
\][/tex]
- For oxygen (O₂):
[tex]\[
\text{ratio of O₂} = \frac{\text{moles of O₂}}{\text{moles of O₂ needed}}
= \frac{3}{3} = 1.0
\][/tex]
4. Comparing the ratios:
- Since the ratio of Fe is 1.0 and the ratio of O₂ is 1.0, they are equal.
5. Determining the limiting reagent:
- In stoichiometry, the limiting reagent is the reactant that is completely consumed first, limiting the amount of product formed.
- Here, both ratios are equal, but by convention and to avoid ties, we typically consider Fe, the first reactant listed, when both ratios are equal.
Therefore, the limiting reagent in this reaction is iron (Fe).
This means that all 4 moles of Fe will react with 3 moles of O₂ to form iron(III) oxide until the Fe is completely consumed.
