6.54 g of zinc are treated with 11.5 g of `H_2SO_4`. Calculate the volume of hydrogen evolved at S.T.P. How much `H_2SO_4` will be left in excess?

Explanation

To solve the problem step by step, we will follow the stoichiometric relationships in the reaction between zinc and sulfuric acid.

### Step 1: Write the balanced chemical equation
The reaction between zinc (Zn) and sulfuric acid (H₂SO₄) can be represented as:
\[ \text{Zn} + \text{H}_2\text{SO}_4 \rightarrow \text{ZnSO}_4 + \text{H}_2 \]

### Step 2: Determine the molar masses
- Molar mass of Zinc (Zn) = 65.4 g/mol
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