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To solve this problem, we need to calculate the number of moles of hydrogen gas (\( \text{H}_2 \)) produced when hydrochloric acid (HCl) reacts completely with 15 grams of aluminum (Al).

### Step-by-Step Approach

1. **Balanced Chemical Reaction:**
   The reaction provided is:
   \[
   \text{Al} + 3 \text{HCl} \rightarrow \text{AlCl}_3 + 1.5 \text{H}_2
   \]
   According to the reaction, 1 mole of aluminum produces 1.5 moles of hydrogen gas.

2. **Calculate the Moles of Aluminum:**
   The atomic mass of aluminum (Al) is given as \( 26.98 \, \text{g/mol} \).
   Using the formula for moles:
   \[
   \text{moles of Al} = \frac{\text{mass of Al}}{\text{atomic mass of Al}} = \frac{15 \, \text{g}}{26.98 \, \text{g/mol}} \approx 0.556 \, \text{mol}
   \]

3. **Relate Moles of Aluminum to Moles of Hydrogen Gas:**
   From the balanced equation, 1 mole of aluminum produces 1.5 moles of hydrogen gas. Therefore:
   \[
   \text{moles of H}_2 = 0.556 \, \text{mol of Al} \times 1.5 \, \frac{\text{mol of H}_2}{\text{mol of Al}} \approx 0.834 \, \text{mol of H}_2
   \]

### Final Answer:
Approximately **0.834 moles of hydrogen gas (H\(_2\))** will be released when 15 grams of aluminum reacts completely.

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Would you like further details or have any other questions?

Here are 5 related questions to expand on this topic:
1. How would the volume of hydrogen gas at STP (standard temperature and pressure) be calculated from moles?
2. What happens if more HCl is added than required for the reaction?
3. How can you determine the limiting reagent in a reaction like this?
4. How do you calculate the theoretical yield of a chemical reaction?
5. What is the relationship between moles and gas volume at different conditions?

**Tip:** When dealing with chemical reactions, always ensure that the reaction equation is balanced before making mole-to-mole conversions!

What number of moles of H2 are released when HCl reacts completely with 15 g of Al? Al + 3 HCl → AlCl3 + 1.5 H2. Atomic mass of Al = 26.98 g mol^(-1)

Learn how to calculate the moles of hydrogen gas (H2) released when 15 grams of aluminum (Al) reacts completely with HCl. This problem involves stoichiometry, the mole concept, and understanding balanced chemical reactions. Suitable for high school students (Grades 9-12).

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