Final answer:
In high school-level Chemistry, we use the provided balanced chemical equation and stoichiometry to calculate the mass of aluminum chloride produced from a given amount of hydrochloric acid by using molar ratios and the molar mass of aluminum chloride.
Step-by-step explanation:
The subject of this question is Chemistry, specifically relating to stoichiometry which deals with the calculation of reactants and products in chemical reactions. The balanced chemical equation we are provided with is crucial for determining the mass of aluminum chloride formed. Given 0.112 mol of hydrochloric acid and knowing that hydrochloric acid reacts with aluminum to produce aluminum chloride, we can use the molar ratios from the balanced equation to solve for the mass of aluminum chloride produced.
We are dealing with the reaction that follows the stoichiometry of 2 Al (s) + 6 HCl (aq) → 2 AlCl₃ (s) + 3 H₂ (g). From this equation, we see that 6 moles of HCl would produce 2 moles of AlCl₃. To find out how much AlCl₃ can be formed from 0.112 mol HCl, we use the molar ratio (0.112 mol HCl * (1 mol AlCl₃ / 6 mol HCl)). Once we find the moles of AlCl₃, we then convert that to mass by multiplying by its molar mass (133.33 g/mol). The final step gives us the mass in grams of the aluminum chloride produced.