8. How many moles of H_(2) can be produced from 33 moles of HCI?

To determine how many moles of \( H_2 \) can be produced from 33 moles of \( HCl \), we need to consider the balanced chemical equation for the reaction. The reaction between \( HCl \) and another reactant (e.g., \( Na \)) to produce \( H_2 \) can be represented as:<br /><br />\[ 2HCl + 2Na \rightarrow 2NaCl + H_2 \]<br /><br />From the balanced equation, we see that 2 moles of \( HCl \) produce 1 mole of \( H_2 \).<br /><br />Given:<br />- 33 moles of \( HCl \)<br /><br />We need to find the moles of \( H_2 \) produced.<br /><br />Using the stoichiometric ratio from the balanced equation:<br />\[ \frac{2 \text{ moles of } HCl}{1 \text{ mole of } H_2} = \frac{33 \text{ moles of } HCl}{x \text{ moles of } H_2} \]<br /><br />Solving for \( x \):<br />\[ x = \frac{33 \text{ moles of } HCl}{2} = 16.5 \text{ moles of } H_2 \]<br /><br />Therefore, 33 moles of \( HCl \) can produce 16.5 moles of \( H_2 \).