Final answer:
To calculate the mass of products from the given reaction, convert the masses of reactants to moles, determine the limiting reagent using stoichiometry, then calculate the moles and mass of the desired products.
Step-by-step explanation:
To calculate the mass of each product formed in the reaction 2Al(s) + 6HNO₃(aq) → 2Al(NO₃)₃(aq) + 3H₂(g), a form of mass-mass stoichiometry must be used. According to the balanced equation, 2 moles of aluminum reacts with 6 moles of nitric acid to form 2 moles of aluminum nitrate and 3 moles of hydrogen gas. Since the problem provides us with the masses of reactants, we must use the molar masses of aluminum and nitric acid to convert these to moles to determine which reactant is the limiting reagent.
First, calculate the moles of each reactant:
- Aluminum (Al): Molar mass = 26.98 g/mol
- Nitric Acid (HNO₃): Molar mass = 63.01 g/mol
Moles of Al = mass of Al / molar mass of Al
Moles of HNO₃ = mass of HNO₃ / molar mass of HNO₃
Next, determine the limiting reagent by comparing the mole ratios from the balanced equation to the calculated moles of the reactants. Then, use the mole ratio between the limiting reagent and the desired product to find out how many moles of product can be formed. Multiply the moles of product with its molar mass to find the mass of the product formed.