Question

Consider the following reaction:

Answer 1

Answer: 1.825 moles of hydrogen gas are produced.

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=$\frac{1}{2}\times 3.65=1.825moles$  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 =$\frac{1}{2}\times 3.65=1.825moles$  of $H_2$

Thus 1.825 moles of hydrogen gas are produced.