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The chemical reaction given is:

\[
2 \, \text{Fe} + 3 \, \text{Cl}_2 \rightarrow 2 \, \text{FeCl}_3
\]

This means that 2 moles of iron (Fe) react with 3 moles of chlorine gas (Cl₂) to produce 2 moles of iron(III) chloride (FeCl₃).

We are asked how many moles of FeCl₃ can be formed from 5.0 moles of Fe.

From the balanced equation, the mole ratio of Fe to FeCl₃ is 2:2 (or 1:1), meaning that for every 1 mole of Fe, 1 mole of FeCl₃ is produced.

Thus, if we start with 5.0 moles of Fe:

\[
\text{Moles of FeCl}_3 = 5.0 \, \text{mol of Fe} \times \frac{2 \, \text{mol of FeCl}_3}{2 \, \text{mol of Fe}} = 5.0 \, \text{mol of FeCl}_3
\]

The correct answer is 5.0 moles of FeCl₃. So the correct choice is **5.0 mol**, not **7.5 mol**.

Would you like more details or further explanation? Here are five related questions to expand on this topic:

1. How would the result change if you started with 10 moles of Fe?
2. What happens if chlorine is the limiting reagent instead of iron?
3. How do you determine the limiting reagent in a chemical reaction?
4. Can you explain the significance of a balanced chemical equation in terms of mass and moles?
5. How do mole ratios in a reaction help in predicting product quantities?

**Tip:** Always check the stoichiometric ratio from the balanced equation when determining how much product is formed from a given amount of reactant.

Given 5.0 moles of Fe, how many moles of iron(III) chloride (FeCl₃) can be formed according to the chemical reaction: 2 Fe + 3 Cl₂ → 2 FeCl₃?

Learn how to solve a stoichiometry problem involving the balanced reaction 2 Fe + 3 Cl₂ → 2 FeCl₃. Find how many moles of iron(III) chloride are produced from 5.0 moles of iron. Understand key concepts such as mole ratios and stoichiometric calculations.

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