# One reaction that produces hydrogen gas can represented by the following unbalanced chemical equation: Mg(s) + HCl(aq) -> MgCl_2(aq) + H_2(g). What mass of HCl is consumed by the reaction of 2.50 moles of magnesium?

Apr 22, 2017

Well we need the stoichiometric equation..............and calculate that $182.3 \cdot g$ of $H C l$ are evolved..............
$M g \left(s\right) + 2 H C l \left(a q\right) \rightarrow M g C {l}_{2} \left(a q\right) + {H}_{2} \left(g\right) \uparrow$
And, given $2.5 \cdot m o l$ metal (and stoichiometric acid), CLEARLY, there are $5.0 \cdot m o l$ $H C l$ consumed.........
And thus mass of $H C l = 5.0 \cdot m o l \times 36.46 \cdot g = 182.3 \cdot g$.