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The question requires us to find the mass of aluminum (\( \text{Al} \)) needed to react completely with 2.19 moles of hydrochloric acid (\( \text{HCl} \)) according to the balanced chemical equation:

\[
2 \text{Al}(s) + 6 \text{HCl}(aq) \rightarrow 2 \text{AlCl}_3(aq) + 3 \text{H}_2(g)
\]

### Step-by-Step Solution:

1. **Analyze the Mole Ratio**:
   The balanced equation shows that 2 moles of \( \text{Al} \) react with 6 moles of \( \text{HCl} \). Therefore, the mole ratio of \( \text{Al} \) to \( \text{HCl} \) is:
   \[
   \frac{2 \text{ moles of Al}}{6 \text{ moles of HCl}} = \frac{1}{3}
   \]

2. **Calculate Moles of Aluminum Required**:
   Since we have 2.19 moles of \( \text{HCl} \), we can calculate the moles of \( \text{Al} \) needed:
   \[
   \text{Moles of Al} = \frac{1}{3} \times 2.19 = 0.73 \text{ moles of Al}
   \]

3. **Calculate Mass of Aluminum**:
   The atomic mass of aluminum (\( \text{Al} \)) is approximately 27 g/mol. Using this, we can find the mass:
   \[
   \text{Mass of Al} = 0.73 \text{ moles} \times 27 \text{ g/mol} = 19.71 \text{ g}
   \]

### Answer:
The mass of aluminum needed is approximately **19.71 grams**.

Would you like more details or have any questions?

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Here are some related questions:
1. What mass of hydrochloric acid would be required to react with 1 mole of aluminum?
2. If 50 grams of aluminum were available, how many moles of hydrochloric acid would be needed for a complete reaction?
3. How much \( \text{H}_2 \) gas (in grams) would be produced from 0.73 moles of aluminum?
4. What is the theoretical yield of \( \text{AlCl}_3 \) if 2.19 moles of \( \text{HCl} \) are used?
5. What would happen to the reaction if there were an excess of \( \text{HCl} \) but limited \( \text{Al} \)?

**Tip:** Always ensure equations are balanced before calculating mole ratios in stoichiometry problems.

According to the equation above, what mass of aluminum is needed to completely react with 2.19 mol of hydrochloric acid?

This page provides a step-by-step guide to calculating the mass of aluminum needed to react with 2.19 mol of hydrochloric acid. Key concepts include stoichiometry, mole ratios, and mass calculation. Suitable for high school students studying chemistry.

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