In the given equation, what does 'X' stand for?
`(2)Al +(X)H_(2)SO_(4) to Al_(2) (SO_(4))_(3) + (3)H_(2)`

Options

A. 2
B. 3
C. 1
D. 5

Explanation

To determine what 'X' stands for in the given chemical equation:

**Given Equation:**
\[ (2) \text{Al} + (X) \text{H}_2\text{SO}_4 \rightarrow \text{Al}_2(\text{SO}_4)_3 + (3) \text{H}_2 \]

**Step 1: Identify the reactants and products.**
- Reactants: Aluminum (Al) and sulfuric acid (H₂SO₄)
- Products: Aluminum sulfate (Al₂(SO₄)₃) and hydrogen gas (H₂)

**Step 2: Write the unbalanced equation.**
- The unbalanced equation is:
\[ 2 \text{Al} + X \text{H}_2\text{SO}_4 \rightarrow \text{Al}_2(\text{SO}_4)_3 + 3 \text{H}_2 \]

**Step 3: Count the number of atoms for each element in the reactants and products.**
- On the left side (reactants):
- Aluminum (Al): 2
- Hydrogen (H): 2X (from X moles of H₂SO₄)
- Sulfur (S): X (from X moles of H₂SO₄)
- Oxygen (O): 4X (from X moles of H₂SO₄)

- On the right side (products):
- Aluminum (Al): 2 (from Al₂(SO₄)₃)
- Hydrogen (H): 6 (from 3 moles of H₂)
- Sulfur (S): 3 (from Al₂(SO₄)₃)
- Oxygen (O): 12 (from Al₂(SO₄)₃)

**Step 4: Set up equations based on the number of atoms.**
- For Aluminum:
\[ 2 = 2 \] (This is balanced)

- For Sulfur:
\[ X = 3 \] (This means we need 3 moles of H₂SO₄)

- For Hydrogen:
\[ 2X = 6 \]
- Solving for X gives:
\[ X = 3 \]

**Step 5: Conclusion**
- The value of 'X' is 3. Therefore, the balanced equation is:
\[ 2 \text{Al} + 3 \text{H}_2\text{SO}_4 \rightarrow \text{Al}_2(\text{SO}_4)_3 + 3 \text{H}_2 \]

**Final Answer:**
X = 3

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