Question

Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas:

2 Al(s) + 6 HCl(aq) -> 2 AlCl₃(aq) + 3 H₂(g)
What mass of H₂(g) is prodced from the reaction of 1.5 g Al(s) with excess hydrochloric acid?

Answer 1

To find the mass of hydrogen gas produced from 1.5 g of aluminum reacting with excess hydrochloric acid, first calculate the moles of aluminum, then use the stoichiometric ratios to find the moles of hydrogen gas, and finally convert those moles to grams.

Step-by-step explanation:

The question relates to the stoichiometry of the reaction between aluminum, Al(s), and hydrochloric acid, HCl(aq), which produces aluminum chloride, AlCl3(aq), and hydrogen gas, H2(g).

The balanced equation for this reaction is 2 Al(s) + 6 HCl(aq) -> 2 AlCl3(aq) + 3 H2(g). To find the mass of H2(g) produced from 1.5 g of Al(s), we need to calculate the number of moles of Al(s) and then use the molar ratio between Al and H2 from the equation. The first step is to convert the mass of Al to moles by using aluminum's molar mass (approximately 26.98 g/mol).

Then using the molar ratio 2:3 from the equation, we calculate the moles of H2. Finally, since the molar mass of H2 is approximately 2.02 g/mol, we convert moles of H2 to grams to find the desired mass.