Question

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?

Answer 1

Well we need the stoichiometric equation..............and calculate that `182.3*g` of `HCl` are evolved..............

Explanation:

`Mg(s) + 2HCl(aq) rarr MgCl_2(aq) + H_2(g)uarr`

And, given `2.5*mol` metal (and stoichiometric acid), CLEARLY, there are `5.0*mol` `HCl` consumed.........

And thus mass of `HCl=5.0*molxx36.46*g=182.3*g`.