Question

Consider the following reaction:

Mg(s) + 2 HCl (aq) → H2(g) + MgCl2(aq)
If 3.65 mol of magnesium and 3.65 mol of hydrochloric acid are reacted, how many
moles of hydrogen gas are produced?

Answer 1

Answer: 1.825 moles of hydrogen gas are produced.

Step-by-step explanation:

The balanced chemical equation is:

`Mg(s)+2HCl(aq)\rightarrow H_2(g)+MgCl_2(aq)`

According to stoichiometry :

2 moles of
`HCl` require = 1 mole of
`Mg`

Thus 3.65 moles of
`HCl` will require=
`(1)/(2)* 3.65=1.825moles` of
`Mg`

Thus
`HCl` is the limiting reagent as it limits the formation of product and
`Mg` is the excess reagent.

As 2 moles of
`HCl` give = 1 mole of
`H_2`

Thus 3.65 moles of
`HCl` give =
`(1)/(2)* 3.65=1.825moles` of
`H_2`

Thus 1.825 moles of hydrogen gas are produced.