2.007grams
The balanced reaction between aluminium and hydrochloric acid is given as:
[tex]2Al+6HCl\rightarrow3H_2+2AlCl_3[/tex]Determine the moles of Hydrogen gas
[tex]\begin{gathered} mole=\frac{mass}{molar\text{ mass}} \\ mole=\frac{0.10}{2.016} \\ mole=0.0496mole\text{ of }H_2 \end{gathered}[/tex]According to stoichiometry, 2 moles of Aluminium produces hydrogen 3 moles of hydrogen:
[tex]\begin{gathered} moles\text{ }of\text{ }Al=00496mole\times\frac{3}{2} \\ moles\text{ of Al}=0.07441mole \end{gathered}[/tex]
Determine the mass of Aluminium
[tex]\begin{gathered} Mass\text{ of Al}=mole\times molar\text{ mass} \\ Mass\text{ of Al}=0.7441\times\frac{26.98g}{mol} \\ Mass\text{ of Al}=2.007grams \\ \end{gathered}[/tex]Hence the mass of Al required to produce 0.10grams of H2 is 2.007grams
