If 2.08 g of Al is reacted with an excess of Fe2O3 how many grams of Al2O3 are produced

To solve this problem, we need to perform a series of calculations based on the balanced chemical reaction between aluminum (Al) and iron(III) oxide (Fe₂O₃) to produce aluminum oxide (Al₂O₃) and iron (Fe). Let's go through the steps one by one.

### Step 1: Write the Balanced Chemical Equation

The reaction between aluminum and iron(III) oxide is:

\[
2 \text{Al} + \text{Fe}_2\text{O}_3 \rightarrow \text{Al}_2\text{O}_3 + 2 \text{Fe}
\]

### Step 2: Calculate the Molar Masses

- Molar mass of Al (Aluminum): \(27.0 \, \text{g/mol}\)
- Molar mass of Al₂O₃ (Aluminum oxide): \(2(27.0) + 3(16.0) = 102.0 \, \text{g/mol}\)

### Step 3: Determine the Moles of Aluminum

Given that we have 2.08 g of Al, we can calculate the moles of Al:

\[
\text{Moles of Al} = \frac{\text{Mass of Al}}{\text{Molar Mass of Al}} = \frac{2.08 \, \text{g}}{27.0 \, \text{g/mol}}
\]

\[
\text{Moles of Al} = 0.07704 \, \text{mol}
\]

### Step 4: Use Stoichiometry to Find Moles of Al₂O₃

According to the balanced chemical equation, 2 moles of Al produce 1 mole of Al₂O₃. So, we use the mole ratio to find the moles of Al₂O₃ produced:

\[
\text{Moles of Al}_2\text{O}_3 = \frac{0.07704 \, \text{mol Al}}{2} = 0.03852 \, \text{mol Al}_2\text{O}_3
\]

### Step 5: Calculate the Mass of Al₂O₃ Produced

Finally, we calculate the mass of Al₂O₃ produced using its molar mass:

\[
\text{Mass of Al}_2\text{O}_3 = \text{Moles of Al}_2\text{O}_3 \times \text{Molar Mass of Al}_2\text{O}_3 = 0.03852 \, \text{mol} \times 102.0 \, \text{g/mol}
\]

\[
\text{Mass of Al}_2\text{O}_3 = 3.92904 \, \text{g}
\]

### Conclusion

Therefore, if 2.08 g of Al is reacted with an excess of Fe₂O₃, **3.93 g of Al₂O₃** (rounded to two decimal places) will be produced.

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### Additional Questions for Exploration:

1. What would be the mass of iron (Fe) produced in this reaction?
2. How would the amount of Al₂O₃ change if only 1.00 g of Al were used?
3. What is the limiting reagent if 2.08 g of Al is reacted with 10.0 g of Fe₂O₃?
4. How much Fe₂O₃ would be required to completely react with 5.00 g of Al?
5. What is the theoretical yield of Al₂O₃ if 5.00 g of Al is reacted?

### Tip:

When performing stoichiometric calculations, always ensure your chemical equation is balanced and you are using the correct mole ratios.

Discover how to calculate the mass of Al2O3 produced when 2.08 g of Al reacts with excess Fe2O3. This problem involves key stoichiometric principles, molar mass calculations, and chemical reaction balancing. Perfect for students in Grades 10-12.

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