Answer:
82.21 g of Fe₃F₂ and 11,2 g of N₂.
Explanation:
- The reaction between Fe₃N₂ and F₂ is represented as:
Fe₃N₂ + F₂ → Fe₃F₂ + N₂.
- it is clear that 1.0 mole of Fe₃N₂ reacts with 1.0 mole of F₂ to produce 1.0 mole of Fe₃F₂ and 1.0 mole of N₂.
- We need to calculate the no. of moles of Fe₃N₂ (78.50 g) and F₂ (15.67 g) using the relation:
n = mass/molar mass,
n of Fe₃N₂ = mass/molar mass = (78.50 g)/(195.5484 g/mol) = 0.4 mol.
n of F₂ = mass/molar mass = (15.67 g)/(37.99681 g/mol) = 0.41 mol ≅ 0.4 mol.
∴ Fe₃N₂ reacts with F₂ with a (1:1) molar ratio.
So, the products will be Fe₃F₂ (0.4 mol) and N₂ (0.4 mol).
- Now, we can get the masses of each product using the relation:
mass = n x molar mass.
∴ mass of Fe₃F₂ = n x molar mass = (0.4 mol)(205.5318 g/mol) = 82.21 g.
∴ mass of N₂ = n x molar mass = (0.4 mol)(28.0 g/mol) = 11,2 g.
