If 3.0 moles of HCl are consumed in the reaction shown, how many moles of FeCl_(3) Ch are produced? 6HCl+Fe_(2)O_(3)arrow 2FeCl3H_(2)O A. 0.50 mol B. 1.0 mol C. 2.0 mol D. 4.0 mol A B D

To determine the number of moles of $FeCl_{3}$ produced when 3.0 moles of $HCl$ are consumed, we need to use the stoichiometric relationship between $HCl$ and $FeCl_{3}$ in the balanced chemical equation.<br /><br />The balanced chemical equation is:<br />$O_{3} \rightarrow 2FeCl_{3} + 3H_{2}O$<br /><br />From the equation, we can see that 6 moles of $HCl$ to produce 2 moles of $FeCl_{3}$.<br /><br />To find the number of moles of $FeCl_{3}$ produced, we can set up a proportion:<br /><br />$\frac{6 \text{ moles of } HCl}{2 \text{ moles of } FeCl_{3}} = \frac{3.0 \text{ moles of } HCl}{x \text{ moles of } FeCl_{3}}$<br /><br />Solving for $x$, we get:<br /><br />$x = \frac{3.0 \text{ moles of } HCl \times 2 \text{ moles of } FeCl_{3}}{6 \text{ moles of } HCl} = 1.0 \text{ moles of } FeCl_{3}$<br /><br />Therefore, the correct answer is B. 1.0 mol.