With the help of the balanced chemical equation
`2Al(s)+3H_(2)SO_(4)(aq) to Al_(2)(SO_(4))_(3)(aq)+3H_(2)(g)`
Answer the equations below :
How many moles of acid are required for each mole of `H_(2)` liberated?

Explanation

To solve the question, we need to analyze the balanced chemical equation provided:

**Balanced Chemical Equation:**
\[ 2 \text{Al}(s) + 3 \text{H}_2\text{SO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3 \text{H}_2(g) \]

### Step-by-Step Solution:

1. **Identify the relationship between reactants and products:**
From the balanced equation, we can see that for every 3 moles of sulfuric acid (H₂SO₄) used, 3 moles of hydrogen gas (H₂) are produced.

2. **Determine the mole ratio:**
The mole ratio of H₂SO₄ to H₂ can be determined from the coefficients in the balanced equation. The equation shows:
- 3 moles of H₂SO₄ produce 3 moles of H₂.

3. **Calculate the moles of acid required for each mole of H₂:**
Since 3 moles of H₂SO₄ yield 3 moles of H₂, we can simplify this to find the moles of acid required for 1 mole of H₂:
\[ \text{Moles of H}_2\text{SO}_4 \text{ required for 1 mole of H}_2 = \frac{3 \text{ moles of H}_2\text{SO}_4}{3 \text{ moles of H}_2} = 1 \text{ mole of H}_2\text{SO}_4 \]

### Conclusion:
Thus, **1 mole of H₂SO₄ is required for each mole of H₂ liberated.**