4) 35.42g of magnesium react with 62.34 moles of sulfuric acid.Determine the moles of hydrogen and identify the liming reactant. Balanced Equation: __ 11

## Step 1<br />The balanced chemical equation for the reaction between magnesium and sulfuric acid is:<br />### \( \text{Mg} + \text{H}_2\text{SO}_4 \rightarrow \text{MgSO}_4 + \text{H}_2 \)<br />From this equation, we can see that 1 mole of magnesium reacts with 1 mole of sulfuric acid to produce 1 mole of hydrogen.<br /><br />## Step 2<br />Given that we have 35.42g of magnesium, we first need to convert this mass into moles. The molar mass of magnesium is approximately 24.305g/mol. Therefore, the number of moles of magnesium is calculated as:<br />### \( \text{Moles of Mg} = \frac{35.42g}{24.305g/mol} \approx 1.46 \text{ moles} \)<br /><br />## Step 3<br />Since the reaction is 1:1, the number of moles of hydrogen produced will also be 1.46 moles.<br /><br />## Step 4<br />To identify the limiting reactant, we compare the number of moles of each reactant. Since we have more moles of sulfuric acid (62.34 moles) than magnesium (1.46 moles), magnesium is the limiting reactant.